Conjugate Acid Base Pair Flashcards, test questions and answers
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Acids and Bases
Biology
Chemistry
Conjugate Acid Base Pair
Strong Acids And Bases
Weak Acids And Bases
Chemistry – Nomenclature of Covalent Compounds – Flashcards 23 terms
23 terms
Preview
Chemistry – Nomenclature of Covalent Compounds – Flashcards
question
Acids
answer
Increase concentration of H+ ions in aqueous (water) solution
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Bases
answer
Increases concentration of OH- ions in aqueouse solution
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Naming bindary acids (acids that conatin exactly two atoms)
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Start with hydro- to indicate H, Add the root of the nonmetal, add -ic
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Naming oxyacids (acids that contain polyatomic ions, which contain one or more oxygen atoms)
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-ate anions make -ic acids, -ite anions make -ous acids
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Naming Bases
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Covalent bases are usually amines-Derivatives of ammonia, A hydrogen ion can attach to a lone pair of electrons, naming is based on the number of groups attached to N, Ionic bases follow the same naming rule as other ionic compounds
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SO2
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sulfur dioxide
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H2SO4
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sulfuric acid
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HBr (as a compound)
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hydrogen bromide
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HBr (as an acid)
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hydrobromic acid
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Carbon tetrabromide
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CBr4
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Chlorine monofluoride
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ClF
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Sulfur dioxide
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SO2
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Phosphorus trichloride
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PCl3
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Which rule is used for writing the name of an ionic base?
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The chemical name ends with "hydroxide."
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Which is the formula for dinitrogen pentoxide?
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N2O5
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Which is the IUPAC name for NO?
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nitrogen monoxide
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Which formula stands for boric acid?
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H3BO3
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Which is an IUPAC name for a covalent compound?
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carbon dioxide
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Which is the formula for iodine tribromide?
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IBr3
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Which is the name for SO3?
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sulfur trioxide
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Which rule should be followed when naming binary acids?
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Start the name with hydro-
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Which formula correctly represents antinomy trichloride?
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SbCl3
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Based on the name, which substance is a covalent compound?
answer
dinitrogen pentoxide
Acids and Bases
Chemistry
Coal Burning Power Plants
Conjugate Acid Base Pair
Physical Science
HBCS 9th Grade Physical Science Final exam study guide – Flashcards 76 terms
76 terms
Preview
HBCS 9th Grade Physical Science Final exam study guide – Flashcards
question
acid
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substance that produces hydrogen ions (H+) in a water solution
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base
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a substance that produces hydroxide ions (OH-) in a water solution
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properties of acids
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sour tasting; can burn; corrosive; react with indicators to produce color change (red)
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properties of bases
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crystalline solids; slippery; bitter tasting; corrosive; can burn; react with indicators to produce color change (blue)
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salt
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compound formed when negative ions from an acid combine with positive ions from a base
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ionization
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process in which electrolytes dissolve in water and separate into charged particles
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hydronium ion
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H3O+ ion, forms when an acid dissolves in water and H+ ions interact with water
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hydroxide ion
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OH- ion; forms when a base dissolves in water
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pH scale
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a measure of the concentration of hydronium ions in a solution using a scale ranging from 0-14 with 0 being the most acidic and 14 being the most basic
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neutralization reaction
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a chemical reaction that occurs when H3O+ ions from an acid react with the OH- ions from a base to produce water molecules and salt
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electrolyte
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compound that breaks apart in water, producing charged particles (ions) that can conduct electricity
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strong acids
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any acid that dissociates completely in solution
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weak acids
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any acid that only partly dissociates in solution
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weak bases
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any base that does not dissociate completely in solution
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strong bases
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any base that dissociates completely in solution
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indicator
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organic compound that changes colors in acids and bases
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motion
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a change in an object's position relative to a reference point
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displacement
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distance and direction of an object's change in position from the starting point
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vector
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a quantity that has both magnitude and direction
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scalar
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a physical quantity that is completely described by its magnitude
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velocity
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the speed and direction of a moving object
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momentum
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property of a moving object that equals its mass times its velocity
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acceleration
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rate of change of velocity;
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force
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a push or pull exerted on an object
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friction
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force that opposes the sliding motion between touching surfaces
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net force
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sum of all of the forces that are acting on an object
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balanced forces
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forces on an object that are equal in size and opposite in direction; net force will be zero and object won't move
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unbalanced forces
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two forces on an object that are not equal in size and are opposite in direction; the direction of the net force will be the same as the larger force
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gravity
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attractive forces between two objects that depends on the masses of the objects and the distance between them
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weight
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gravitational force exerted on an object
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inertia
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tendency of an object to resist any change to its motion
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work
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transfer of energy when a force is applied over a distance; measure in joules
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machine
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device that makes doing work easier by increasing the force applied to an object, changing the direction of an applied force, or increasing the distance over which a force can be applied
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simple machine
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machine that does work with only one movement; (lever, pulley, wheel & axle, inclined plane, screw, and wedge)
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pulley
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a simple machine that uses grooved wheels and a rope to raise, lower or move a load. (a modified lever)
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power
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rate at which energy is converted; measured in watts
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screw
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a simple machine that is an inclined plane wrapped around a pole which holds things together or lifts materials.
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inclined plane
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a simple machine consisting of a slanting surface connecting a lower level to a higher level
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wedge
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a simple machine that is an object with at least one slanting side ending in a sharp edge
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block and tackle
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a system of two or more pulleys with a rope or cable threaded between them, usually used to lift or pull heavy loads.
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energy
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the ability to cause change, measured in joules
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potential energy
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energy that is stored due to the interaction between objects
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kinetic energy
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energy a moving object has because of its motion;
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Law of Conservation of Energy
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states that energy cannot be created or destroyed
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temperature
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measure of the average kinetic energy of all the particles that make up an object
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thermal energy
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sum of the kinetic and potential energy of the particles that make up an object
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heat
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energy that is transferred between objects due to a temperature difference between those objects
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conduction
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transfer of thermal energy by collisions between the particles that make up matter
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convection
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transfer of thermal energy in a fluid by the movement of warmer and cooler fluid from one place to another
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radiation
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transfer of energy by electromagnetic waves
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specific heat
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amount of heat needed to raise the temperature of 1kg of a material 1 degrees Celsius
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insulator
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material in which electrons and thermal energy are not able to move easily
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conductor
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material, such as copper wire, through which electrons can move easily
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voltage
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force an electrical current; measure in volts
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resistance
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tendency for a material to oppose electron and to convert electrical energy into other forms of energy; measured in ohms
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electric current
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the net movement of electric charges in a single direction, measured in amperes
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capacitor
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a device used to store an electric charge, consisting of one or more pairs of conductors separated by an insulator
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induction
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the rearrangement of electrons on a neutral object by a nearby charged object
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static electricity
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the accumulation of excess electric charge on an object
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electric circuit
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a closed path that an electric current follows
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parallel circuit
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circuit in which an electric current has more than one path to follow
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series circuit
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circuit in which electric current has only one path to follow
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circuit breaker
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a device that prevents a circuit from overheating and causing a fire; a switch is automatically flipped when the current becomes too great
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fuse
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a small piece of metal that melts if a current becomes to high causing a break in the circuit and stopping the current
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switch
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a device for making and breaking the connection in an electric circuit
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calculate momentum
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momentum p = mass x velocity; [p=mv] example 1: a car with a mass of 1300 kg is traveling south at a speed of 28m/s p = 1300kg x 28m/s; p=36,400kg.m/s south
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calculate potential energy
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gravitational potential energy (J) = mass (kg) x gravity (N/kg) x height (m) [GPE=mgh] example: mass = 4kg; gravity = 9.8N/kg; height = 2.5m GPE = 4kg x 9.8N/kg x 2.5m GPE = 98 N.m or 98J
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calculate kinetic energy
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kinetic energy (in joules) = 1/2 mass (in kg) x [speed (in m/s)]2 [KE = 1/2mv2] mass = 60kg; speed = 3.0m/s KE = 1/2 60kg x( 3m/s)2 1/2 60kg x 9m/s KE = 270J
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calculate force
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Force (net) = mass x acceleration [F=ma] example: mass = .6kg acceleration = 5000m/s2 F = .6kg(5000m/s20 F = 300 kg.ms/s2 F = 300N
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calculate work
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work (in joules) = applied force (in newton) x distance (in meters) [W=Fd] applied force = 100N distance = 5m W = 100N x 5m W = 500J
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solve for weight
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weight (N) = mass (kg) x gravitational strength (N/kg) [Fg = mg] example: mass = 5,000kg gravitational strength = 9.8N/kg Fg = 5000kg x 9.8N/kg Fg(weight) = 49,000N
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solve for acceleration
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acceleration (in meters/second2) = net force (in newtons) divided by mass (kg) [a=F/m] example: mass = 12kg net force = 6N south a = 6Nsouth/12kg a == .5m/s2
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calculate net force
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forces in the same direction are added together; subtract forces in opposite directions; forces NOT in the same direction or in opposite directions cannot be directly added together
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calculate velocity
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velocity is calculated when you take the displacement of an object with its direction and divide it by a change in time
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calculate Ohm's Law
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current (amperes) = voltage difference (volts) / resistance (ohms) [I=V/R] example: voltage difference = 6V resistance = 1,200Ohms I = 6V/1200 Ohms I = .005V/Ohms or .005 A
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temperature conversions
answer
Acids
Acids and Bases
Chemistry
Conjugate Acid Base Pair
Strong Acids
Weak Acids And Bases
PA 502: Medical Physiology- Acid Base Physiology – Flashcards 44 terms
44 terms
Preview
PA 502: Medical Physiology- Acid Base Physiology – Flashcards
question
Acids
answer
-H+ donors -strong acids dissociate completely in solution -weak acids do not dissociate completely
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Bases
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-H+ acceptors -can be classified as strong or weak
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pH
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-measure of H+ concentration
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How can the pH of the ECF be measured?
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Henderson-Hasselbach equation pH=pKa + log[HCO3-]/[CO2]
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What are the cells of the body constantly producing?
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H+
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How much H+ do healthy individuals make a day?
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50-100 mEq/L
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What are the 3 ways to control pH?
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1. Buffer System 2. Respiratory Regulation 3. Renal Regulation
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What is the Buffer System?
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-takes a strong base or acid and converts it to weak base or acid -reaction occurs within seconds -prevent changes in pH by binding H+ (acting like bases) whenever the pH of the ECF drops below normal and releasing H+ (acting like acids) whenever the pH of the ECF climbs above normal
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What are the 3 main buffer systems?
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1. Bicarbonate Buffer System 2. Phosphate Buffer System 3. Protein/Amino Acid Buffer System
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Bicarbonate Buffer System
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-If ECF is acidotic, weak acid created: HCL +HCO3- = HCL and carbonic acid -If ECF is alkalotic, weak base created: NaOH + carbonic acid = H2O and sodium bicarbonate
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Phosphate Buffer System
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-If ECF is acidotic, weak acid created: HCL + disodium hydrogen Phosphate (Na2HPO4) = Salt (NaCl) + Sodium dihydrogen phosphate (Na2H2PO4) -If ECF is alkalotic, weak base created: Sodium Hydroxide (NaOH) + Sodium dihydrogen (NaH2PO4) + H2O and Disodium Hydrogen Phosphate (Na2HPO4)
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Protein/Amino Acid Buffer System
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-If ECF is acidotic: the amine group acts as a BASE and picks up an H+ from the fluid -If ECF is alkalotic: carboxyl group acts as an ACID by donating H+ to the fluid
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Respiratory Regulation of pH *memorize this equation!*
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-increases or decreases the amount of CO2 expelled from lungs depending on what is needed by the body -reaction occurs in minutes -Using the equation: CO2 + H2O H2CO3 H+ + HCO3- Hypoventilation: increased CO2, pushing the equation to the right and increased H+ concentration Hyperventilation: decreased CO2, reversing the equation to the left and decreased H+ concentration
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Renal Regulation of pH
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-only process that physically removes H+ or adds HCO3- in the body -reactions occurs in hours to days -If someone is in metabolic acidosis and it won't regulate fast enough, they will die before it gets controlled -Renal Tubules Functionals in 3 ways
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What are the 3 ways Renal Tubules function?
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1. Regulating H+ levels 2. Regulating HCO2- levels 3. Synthesizing HCO3-
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Acidotic conditions:
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-kidneys secret H+ and reabsorb HCO3- -causes urine to become more acidic and blood more basic -Synthesizing HCO3-: renal cells lining the proximal convoluted tubule can also synthesize HCO3- to a certain extent which is then released into the blood stream
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Alkalotic conditions:
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-kidneys reabsorb H+ and secrete HCO3- -causes blood to become more acidic
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Acidemia
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decrease in arterial pH below 7.35
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Acidosis
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condition resulting from acidemia
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Alkalemia
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increase in arterial pH above 7.45
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Alkalosis
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condition resulting from alkalemia
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Arterial Blood Gases: What is this test used to assess the adequacy of?
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-Oxygenation, pO2 -Ventilation, pH and CO2 -Acid-Base Balance, pH, CO2, HCO3-
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What is the normal range of pH?
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7.35-7.45
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What is less that 7.35 pH considered?
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Acidosis
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What is more than 7.45 pH considered?
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Alkalosis
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What is a pH of less than 7.0 or more than 7.8 considered?
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incompatible with life
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What is pCO2?
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-partial pressure of CO2 in arterial blood -the level controlled by the respiratory system -tells how the patient is ventilating normal is: 45-45mmHg
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What is hypocarbia?
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less than 35 pCO2
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What is hypercarbia?
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more than 45 pCO2
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What is Respiratory Alkalosis?
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Increased Respirations, Decreased CO2 -causes hyperventilation (fear, pain, anxiety, crying in babies, exercise, etc.) -stimulation of respiratory center (brain injury, overdose, encephalitis, etc.) -mechanical over-ventilation
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What is Respiratory Acidosis
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Decreased Respirations, Increased CO2 -hypoventilation -COPD, Pneumonia, Atelectasis- collapsed alveoli, Respiratory muscle wall weakness Mechanical under-ventilation, Barbiturate or Sedative OD, Near drowning, Suffocation (choking), Chest wall abnormality (kyphosis, obesity)
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Metabolic Alkalosis
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patient is alkalotic and it is not respiratory alkalosis -accumulation of too much base -loss of too much acid -CO2 should be normal or high, >45 -HCO3- should be high >28 *If the pH is off, but the oxygen level is okay, you need to check! *excessive gastric suctioning *severe vomiting of stomach contents only *Potassium deficit *Medications: Antacids, Diuretics
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Metabolic Acidosis
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-patient is acidotic and it is not respiratory acidosis -accumulation of too much acid and loss of too much base -CO2 normal or low <35 -HCO3- should be low <22 *If the pH is off, but the oxygen level is okay, you need to check! *Diabetic Ketoacidosis- body is starving, even though they do have enough glucose, body moves to ketones, Lactic Acidosis- not enough oxygen, Renal tubular acidosis, Renal failure, Severe diarrhea- body losing stool so fast, body has to replace enzymes in there, Starvation, Poisoning (e.g. methanol, ethylene glycol)
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What is HCO3-?
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-measure of bicarbonate ion in arterial blood -a Base -regulated by kidneys -Normal range: 22-28 mmol/L
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Alkalosis
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-leads to tissue hypoxia -causes vasoconstriction -causes O2 to bind tighter to Hgb, not released to tissues -Remember Oxygen-Hemoglobin Disassociation curve
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pO2, PaO2
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-partial pressure of oxygen in arterial blood -Range 80-100mmHg, age and altitude dependent -values increase with supplemental O2 -tells how well patient is oxygenated
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O2 Saturation, SaO2
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-percentage of hemoglobin actually binding, saturated with oxygen 90-100% age dependent
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FiO2
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fraction inspired air that is oxygen -FiO2 of room air is 21% 2 liters = 28% 3 liters = 32% 4 liters = 36%
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What is the FiO2 of a simple face mask?
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40-60%
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What is the FiO2 of a Nonrebreather mask?
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60-100% (for seizures, no oxygen into their blood...)
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What is the FiO2 of a Bag-Mask Ventilation?
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100%
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Respiratory Failure
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pCO2 greater than 50 pO2 less than 50
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Chronic Respiratory Failure
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pCO2 greater than 50, pH 7.35-7.45 pO2 less than 50, pH 7.35-7.45
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Acute Respiratory Failure
answer
-pCO2 greater than 50, pH less than 7.35 or greater than 7.45 -pO2 less than 50, pH less than 7.35 or greater than 7.45
Acid Base Reactions
Acids and Bases
Chemistry
Conjugate Acid Base Pair
Acids And Bases Terms – Flashcards 22 terms
22 terms
Preview
Acids And Bases Terms – Flashcards
question
| Alkaline |
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| Term used to describe when a base completely dissociates in water to yield aqueous OH ions |
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| Arrhenius acid |
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| A chemical compound that increases the concentration of hydrogen ions in aqueous solution |
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| Arrhenius base |
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| A substance that increases the concentration of hydroxide ions in aqueous solution |
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| Binary acid |
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| An acid that contains only two different elements: hydrogen and one of the more-electronegative elements |
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| Oxyacid |
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| An acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal |
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| Strong acid |
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| Acid that ionizes completely in aqueous solution |
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| Weak acids |
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| Acids that are weak electrolytes |
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| Amphoteric |
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| Any species that can react as either an acid or a base |
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| Bronsted-Lowry acid |
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| A molecule or ion that is a proton donor |
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| Bronsted-Lowry acid-base reaction |
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| Protons are transferred from one reactant (the acid) to another (the base) |
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| Bronsted-Lowry base |
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| A molecule or ion that is a proton acceptor |
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| Conjugate acid |
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| The species that is formed when a Bronsted-Lowry base gains a proton |
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| Conjugate base |
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| The species that remains after a Bronsted-Lowry acid has given up a proton |
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| Diprotic acid |
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| Can donate two protons per molecule |
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| Monoprotic acid |
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| An acid that can donate only one proton (hydrogen ion) per molecule |
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| Polyprotic acid |
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| An acid that can donate more than one proton per molecule |
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| Triprotic acid |
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| An acid able to donate three protons per molecule |
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| Lewis acid |
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| An atom, ion, or molecule that accepts an electron pair to form a covalent bond |
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| Lewis acid-base reaction |
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| The formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor |
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| Lewis base |
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| An atom, ion, or molecule that donates an electron pair to form a covalent bond |
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| Neutralization |
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| The reaction of hydronium ions and hydroxide ions to form water molecules |
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| Salt |
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| An ionic compound composed of a cation from a base and an anion from an acid |
Acids and Bases
Chemistry
Conjugate Acid Base Pair
Weak Acids And Bases
Acids and Bases key terms – Flashcards 22 terms
22 terms
Preview
Acids and Bases key terms – Flashcards
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| alkaline |
answer
| the solution formed when a base completley dissociates in water to yield aqueous OH- ions |
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| arrhenius acid |
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| a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solutions |
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| arrhenius base |
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| a substance that increases the concentration of hydroxide ions, OH-, in aqueous solutions |
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| binary acid |
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| an acid that contains only two different elements: hydrogen and one of the more electronegtive elements |
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| oxyacid |
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| an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal |
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| strong acid |
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| one that ionizes completley in aqueous solutions |
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| weak acids |
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| acids that are weak electrolytes |
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| amphoteric |
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| any species that can react as either an acid or a base |
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| Bronsted-Lowry acid |
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| is a molecule or ion that is a proton donor |
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| Bronsted-Lowry Base |
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| is a molecule or ion that is a proton acceptor |
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| Bronsted-Lowry Acid-base reactions |
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| protons are transferred from one reactant (the acid) to another (the base) |
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| monoprotic acid |
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| an acid that can donate only one proton (hydrogen ion) per molecule |
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| polyprotic acid |
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| ana tom that can donate more than one proton per molecule |
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| diprotic acid |
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| can donate two protons per molecule |
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| triprotic acid |
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| an acid able to donate three protons per molecule |
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| Lewis acid |
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| an atom, ion, or molecule that accepts an electron pair to form a covalent bond |
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| Lewis base |
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| an atom, ion, or molecule that donates an electron pair to form a covalent bond |
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| Lewis acid-base reaction |
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| the formation of one or more covalent bonds between an electron-pair donor and electron pair acceptor |
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| conjugate base |
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| the species left after a Bronsted-Lowry acid has given up a proton |
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| Conjugate acid |
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| species left after a Bronsted-Lowry base gains a proton |
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| neutralization |
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| the reaction of hydronium ions and hyroxide ions to form water molecules |
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| salt |
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| ionic compound composed of a cation rom a base and an anion from an acid |
Acids and Bases
Conjugate Acid Base Pair
Loss And Gain
Weak Acids And Bases
Chapter 17 Additional Aspects of Aqueous Equilibria – Flashcards 46 terms
46 terms
Preview
Chapter 17 Additional Aspects of Aqueous Equilibria – Flashcards
question
| What happens when NaC2H3O2 is added to a solution of HC2H3O2? |
answer
| Because C2H3O2- is a weak base, the pH of the solution increases; that is, [H+] decreases. |
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| In which direction will the equilibrium of this reaction shift to? |
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| This equilibrium will shift to the left, thereby decreasing the equilibrium concentration of [H+]. |
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| What is the common-ion effect? |
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| The extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte. |
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| Is the ionization of a weak base also decreased by the addition of a common ion? |
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| Yes |
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| What is a buffered solution (or buffer)? |
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| A solution which contains a weak conjugate acid-base pair that can resist drastic changes in pH upon the addition of small amounts of strong acid or strong base. |
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| Why does a buffer resist changes in pH? |
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| A buffer resists changes in pH because it contains both an acidic species to neutralize OH- ions and a basic one to neutralize H+ ions. |
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| Why does a buffer resist changes in pH? |
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| A buffer resists changes in pH because it contains both an acidic species to neutralize the [OH-] ions and a basic one to neutralize [H+] ions. |
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| How are buffers prepared? |
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| Buffers are prepared by mixing a weak acid or a weak base with a salt of that acid or base. |
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| Under what conditions will buffers most effectively resist a change in pH in either direction? |
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| When the concentrations of weak acid and conjugate base are about the same. |
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| What are the two important characteristics of a buffer? |
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| Its capacity and its pH. |
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| What is buffer capacity? |
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| Buffer capacity is the amount of acid or base the buffer can neutralize before the pH begins to change to an appreciable degree. |
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| What determines a buffer's capacity? |
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| The amount of acid and base from which the buffer is made. |
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| What determines the pH of the buffer? |
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| The pH of the buffer depends on the Ka for the acid and on the relative concentrations of the acid and base that comprise the buffer. |
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| What is the Henderson-Hasselbach equation? |
answer
| pH = pKa + log ([base] / [acid]) |
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| Explain why a mixture of HC2H3O2 and NaC2H3O2 can act as a buffer while a mixture of HCl and NaCl cannot. |
answer
In a mixture of HC2H3O2 and NaC2H3O2, HC2H3O2 reacts with added base and C2H3O2- combines with added acid, leaving [H+] relatively unchanged.; Although HCl and Cl- are a conjugate acid-base pair, Cl- has no tendency to combine with added acid to form undissociated HCl.; Any added acid simply increases [H+] in an HCl-NaCl mixture. |
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| Do reactions between strong acids and weak bases or strong bases and weak acids essentially proceed to completion?; Under what conditions? |
answer
| Yes, as long as the buffering capacity of the buffer is not exceeded, we can assume the strong acid or strong base is completely consumed by reaction with the buffer. |
question
| What are the steps to calculate how the pH of a buffer will respond to the addition of a strong acid or a strong base? |
answer
1.; Consider the acid-base neutralization reaction, and determine its effect on [HX] and [X-].; (Stoichiometry calculation) 2.; Use Ka and the new concentrations of [HX] and [X-] from step 1 to calculate [H+].; (Equilibrium calculation) |
question
| What is a pH titration curve? |
answer
| It is the graph of the pH as a function of the volume of the added titrant. |
question
For a strong acid-strong base titration, what determines the initial pH of the solution before the addition of a strong base (or strong acid)? ; |
answer
| The pH of the solution is determined by the inital concentration of the strong acid, if the titrant is a strong base, or the initial concentration of the strong base, if the titrant is a strong acid. |
question
| For a strong acid-strong base titration, what determines the pH of the solution after a strong base or strong acid is being added but before the equivalence point? |
answer
| The pH of the solution is determined by the concentration of acid or base that has not yet been neutralized. |
question
| For a strong acid-strong base titration, what is the pH of the solution at the equivalence point? |
answer
| The pH of the solution is 7.00 (neutral). |
question
| For a strong acid-strong base titration, what determines the pH of the solution after the equivalence point? |
answer
| The pH of the solution is determined by the concentration of the excess strong base or excess strong acid in the solution (concentration of titrant). |
question
| What is the end point of a titration? |
answer
| It is the point in a titration where the indicator changes color to distinguish it from the actual equivalence point that it closely approximates. |
question
| For a weak acid-strong base titration, what determines the pH of the solution prior to the addition of the strong base titrant? |
answer
| The inital pH is determined by the pH of just the weak acid. |
question
| For a weak acid-strong base titration, what determines the pH of the solution just prior to the equivalence point? |
answer
| The pH of the solution just prior to reaching the equivalence point is determined by the concentrations of the weak acid and its conjugate-base. |
question
| For a weak acid-strong base titration, what is the pH of the solution?; What determines this pH? |
answer
| The pH of the solution at the equivalence point is greater than 7.00, which is determined by the conjugate-base of the weak acid, a weak base. |
question
| For a weak acid-strong base titration, what determines the pH of the solution after the equivalence point? |
answer
| The pH of the solution after the equivalence point is determined by the concentration of [OH-] from the excess strong base. |
question
| How does a pH titration curve for a weak acid-strong base titration differ from a strong acid-strong base titration?; (There are 3 differences.) |
answer
1.; The solution of the weak acid has a higher inital pH than a solution of a strong acid of the same concentration. 2.; The pH change at the rapid-rise portion of the curve near the equivalence point is smaller for the weak acid than it is for the strong acid. 3.; The pH at the equivalence point is above 7.00 for the weak acid-strong base titration. |
question
| Why is the choice of indicator for a weak acid-strong base titration more critical than it is for a strong acid-strong base titration? |
answer
| The pH change near the equivalence point becomes smaller as Ka decreases. |
question
| What is the solubility-product constant (or simply the solubility product)? |
answer
| It is the equilibrium constant (Ksp) for the equilibrium that exists between a solid ionic solute and its ions in a saturated aqueous solution. |
question
| Do solids, liquids, and solvents appear in the equilibrium-constant expressions for heterogeneous equilibria? |
answer
| No |
question
| Why is the concentration of undissolved solid not explicitly included in the expression for the solubility-product constant? |
answer
| The concentration of undissolved solid does not appear in the solubility product expression because it is constant as long as there is solid present. |
question
| What is the difference between solubility and the solubility-product constant? |
answer
| The solubility of a substance is the quantity that dissolves to form a saturated solution.; The solubility-product constant (Ksp) is the equilibrium constant for the equilibrium between an ionic solid and its saturated solution. |
question
| Besides temperature, name three other factors that affect the solubility of ionic compounds? |
answer
| The presence of common ions, the pH of the solution, and the presence of complexing agents. |
question
| How is the common-ion effect related to the solubility of a slighly soluble salt? |
answer
| The solubility of a slightly soluble salt is decreased by the presence of a second solute that furnishes a common ion. |
question
| The concentrations of ions calculated from Ksp sometimes deviate appreciably from those found experimentally.; What three factors contribute to this deviation? |
answer
| The deviations are due to electrostatic interactions between ions in solution (which can lead to ion pairs), ignoring other equilibria that occur simultaneously in the solution, and the assumption that ionic compounds dissociate completely into their component ions when they dissolve. |
question
| Will the solubility of any substance whose anion is basic be affected to some extent by the pH of the solution? |
answer
| Yes |
question
| The solubility of almost any ionic compound is affected if the solution is made sufficiently acidic or basic.; Under what condition are the effects noticeable? |
answer
| The effects are very noticeable when one or both ions involved are at least moderately acidic or basic. |
question
| What effect does an increase in [H+] (as pH is lowered) have on the solubility of slightly soluble salts containing basic anions? |
answer
| The solubility of slightly soluble salts containing basic anions increases as [H+] increases (as pH is lowered).; The more basic the anion, the more the solubility is influenced by pH.; Salts with anions of negligible basicity (the anions of strong acids) are unaffected by pH changes. |
question
| What is a complex ion? |
answer
| A complex ion is an assembly of a metal ion and the Lewis bases bonded to it. |
question
| How is the stability of a complex ion in aqueous solution judged? |
answer
| Stability of a complex ion in aqueous solution can be judged by the size of the equilibrium constant for its formation from the hydrated metal ion. |
question
| What is Kf? |
answer
| Kf is the formation constant. |
question
| What effect does the presence of suitable Lewis bases (NH3, CN-, or OH-, for example) have on the solubility of metal salts? |
answer
| The solubility of metal salts increases in the presence of suitable Lewis bases, if the metal forms a complex with the base. |
question
| Some metal hydroxides and oxides that are relatively insoluble in neutral water dissolve in what kind of solutions? |
answer
| Strongly acidic and strongly basic solutions. |
question
| Substances that are soluble in strong acids and bases because they capable of behaving as either an acid or base are called what? |
answer
| Amphoteric |
question
| Name four amphoteric substances that are metal hydroxides and oxides. |
answer
| The hydroxides and oxides of Al3+, Cr3+, Zn2+, and Sn2+. |
Acids and Bases
Chemistry
Conjugate Acid Base Pair
Red Litmus Paper
Modern Chemistry Chapter 15 Acids and Bases – Flashcards 75 terms
75 terms
Preview
Modern Chemistry Chapter 15 Acids and Bases – Flashcards
question
| What contains acetic acid? |
answer
| Vinegar |
question
| What contains lactic acid? |
answer
| sour milk |
question
| What does phosphoric acid do to many carbonated beverages? |
answer
| It gives a tart flavor |
question
| What foods contain citric acid? |
answer
| Lemons, oranges, grapefruits |
question
| What contains malic acid? |
answer
| Apples |
question
| What contains tartaric acid? |
answer
| Grapejuice |
question
| What is the common name for Sodium Hydroxide NaOH? |
answer
| lye |
question
| Acids were first recognized as what? |
answer
| a distinct class of compounds because of the common properties of their acqeous solutions. |
question
| What are the properties of an acid? |
answer
| 1. Acqeous solutions of acids have a sour taste. 2. Acids change the color of acid-base indicators. 3. Some acids react w/active metals to release hydrogen gas, H2. 4. Acuds react with bases to produce salts and water. (salt- the reaction products are water and an ionic compound called a salt). 5. Some acids conduct electric current. 6. Contains H30 |
question
| What is a binary acid? |
answer
| An acid that contains only two different elements: hydrogen and one of the more electronegative elements. ex: HF, HCl, HBr, and HI. |
question
| How do you name binary acids? |
answer
| by using the Binary Acid Nomenclature: 1. THe name of a binary acid begins with the prefix, hydro-. 2. The root of the name of the second element follows this prefix. 3. The name that ends with the suffix -ic. Ex: HF- Hyrdrofluoric acid, HCl-hydrochloric acid, HI- Hydroiodic acid, H2S- Hydrosulfuric acid |
question
| What is an oxyacid? |
answer
| An acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal. Ex: HNO3 (nitric acid) |
question
| What kind of class does oxyacids belong to? |
answer
| Ternary acids- which are acids that contain three different elements. |
question
| What does an oxyacid's name depend on? |
answer
| it is based on its anion |
question
| What are the five common industrial acids? |
answer
| sulfuric acid, nitric acid, phosporic acid, hydrochloric acid, and acetic acid |
question
| What is the most commonly produced industrial chemical in the world? What are some uses of this acid? Why is this acid effective? |
answer
| Sulfuric acid. It is used in large quantities in petroleum refining and metallurgy as well as in the manufacture of fertilizer. Production of metals, paper, paint, dyes. Because it attracts water, concentrated sulfuric acid is an effective dehydration (water removing) agent. |
question
| What is Nitric Acid? What is its characteristics? what is it used for? what happens when it is left standing? |
answer
| it is a volatile, unstable liquid that is rarely used in industry or laboratories. Dissolving the acid in water provides stabilitu. It also turns proteins yellow. Use to make explosives, rubber, platics, dyes, and pharmaceuticals. Usually the solutions are colorless, but left standing, they become yellow because of slight decompisition to brown nitrogen dioxide gas. |
question
| Along w/nitrogen and potassium, Phosporus is what? What is phosphoric acid used for? |
answer
| It is an essential element for plants and animals. Most of the phosporic acid produced each year is directly for manufacturing fertilizers and animal feed. Dilute p.acid has a pleasant but sour taste that is not toxic. It is used in flavoring agents in beverages. It is important in the manufacture of detergents and ceramics. |
question
| What is hydrochloric acid used for? Industrially? and what about its dilute solution? |
answer
| HCl is produced by the stomack to aid digestion. Industrially, it is used for "pickling" (immerison of metals in a. solutions to remove surface impurities) iron and steel. It is used as a cleaning agent, food processing, activation of oil wells, recover Mg from sea water. The dilute solution is referred to as muriatic acid (found in hardware stores. to maintain the correct acidity in swimming pools) |
question
| What are some characteristics of acetic acid? What is its concetrated solution called? How does it get its name? How is it used? |
answer
| Concentrated acetic acid is clear, colorless, pungent smelling liquid called glacial acetic acid. the name derives from the fact that pure acetic acid has freezing point of only 17C. IT can form crystals in a cold room. The fermentation of plants sometimes produce this acid. It is important industrially in synthesizing chemicals used in the manufacture of plastics. It is also used as a fungicide. |
question
| How do bases differ from acids? What are its characteristics? |
answer
| 1. Aqueous solutions of bases taste bitter. 2. Bases change the color of acid-base indicators. 3. Dilute acqeous solutions feel slippery. 4. Bases react with acids to produce salts and water. 5. Bases conduct electric current. 6. It contains OH |
question
| Who is Svante Arrhenius? |
answer
| A Swedish chemist who lived from 1859-1927, understood that acqeous solutions of acids and bases conduct electric current. He came up w/the Arrhenius acids and bases. |
question
| What is an Arrhenius acid? |
answer
| A chemical compound that increases the concentration of hydrogen ions. H+, in acqeous solutions. An acid will ionize in solution, increasing the number of hydrogens present. |
question
| What is an Arrhenius base? |
answer
| a substance that increases the concentration of hydroxide ions OH-, in acqeous solutions. These bases dissociate in solution to release OH ions into the solutions. |
question
| What are all pure acqeous acids? |
answer
| electrolytes |
question
| Why do acids form hydronium? |
answer
| because acid molecules are polar, so that one or more hydrogen ions are attracted by ater molecules. Negatively charged anions are left behind. Ex: HNO3 + H2O = H3O + NO3 |
question
| What is a strong acid? |
answer
| One that ionizes completely in acqeous solutions. Ex: HCl (hydrochloric acid), HClO4 (perchloric acid), HNO3 (nitric acid). Ex: H2SO4 + H2O = H3O + HSO4 |
question
| What do strength of acids depend on? |
answer
| the polarity of the bond between hydrogen and the element to which it is bonded and the ease with which that bond can be broken. Acid strength increases with increasing polarity and decreasing bond energy. |
question
| What are weak acids? |
answer
| Acids that are weak electrolytes. The aqeous solution of weak acid contains hydronium ions, anions, and dissolved acid molecules. Ex: Hydrocyanic acid (HCN) Ex: HSO4 + H2O = H3O + SO4 |
question
| What do organic acids contain? |
answer
| the acidic carboxyl grou: COOH. |
question
| How many hydrogen atoms does a molecule of acetic acid contain? What is its characteristics? |
answer
| contains four. Only one of the hydrogen atoms is ionizable. The hydrogen atom in the carboxyl group in acetic acid is the one that is acidic and forms the hydronium ion. |
question
| What are most bases? |
answer
| They are ionic compounds containing metal cations and the OH anion. because these bases are ionic, they dissociate to some extent. |
question
| When a base completely dissociates in water to yiel aqueous OH- ions, the solution is referred to as...? |
answer
| Alkaline. Ex: Sodium hydroxide (NaOH) is the common laboratory base. NaOH - Na + OH |
question
| What other hydroxides form alkaline solutions? |
answer
| Li, Na, K, Rb, and Cs |
question
| What is a base commonly used in household cleaners? |
answer
| NH3. Ammonia is a base because it produces hydroxide ions when it reacts with water molecules. |
question
| What do the strength of bases depend on? |
answer
| the extent to which the base dissociates, or adds hydroxide ions to the solutions. Ex of strong base: KOH. - Strong bases are strong electrolytes. Ex: Ca(OH)2 = Ca + 2OH Weak base: NH3 + H2O = NH4 + OH |
question
| What happens when a base is not very soluble? |
answer
| They do not produce a large number of hydroxie ions when added to water. ex: Cu(OH)2. |
question
| What do the alkalinity of aqueous solutions depend on? |
answer
| The concentration of OH ions in solution. |
question
| Who expanded the Arrhenius acid definition? |
answer
| (1923) Danish chemist JN Bronsted and English chemist TM Lowry. |
question
| What is a Bronsted-Lowry acid? |
answer
| A molecule or ion that is a proton donor. Like hydrogen chloride and water. Ex: HCl + NH3 = NH4 + Cl Ex: H2O + NH3 = NH4 + OH |
question
| What is a bronsted-lowry base? |
answer
| a molecule or ion that is a proton acceptor. The arrhenius hydroxide base such as NaOH is not a bronsted-lowry base because its species cannot accept a proton. |
question
| What happens in a Bronsted-Lowry acid-base reaction? |
answer
| protons are transferred from one reactant (the acid) to another (the base). |
question
| What is a monoprotic acid? |
answer
| An acid that can donate only one proton (hydrogen ion) per molecule. Ex: Perchloric acid (HClO4), hydrochloric acid (HCl), and nitric acid (HNO3). Ex: HCl + H2O = H3O + Cl |
question
| What is a polyprotic acid? |
answer
| an acid that can donate more than one proton per molecule. Ex: Sulfuric acid (H2SO4) and phosphoric acid (H3PO4). |
question
| The ionization of polyprotic acid occur in what? |
answer
| Stages because an acid can only donate a hydrogen atom one at a time. |
question
| What is a diprotic acid? |
answer
| can donate two protons per molecule. Ex of ionization:(sulfuric acid) H2SO4 + H20 = H30 + HSO4- HSO4 + H20 = H30 + SO4 2- |
question
| What is a triprotic acid? |
answer
| An acid able to donate three protons per molecule. Ex: H3PO4 + H20 = H30 + H2PO4 - H2PO4 + H20 = H30 + HPO4 2- HPO4 + H20 = H30 + PO4 3- |
question
| Which stage of ionization is greatest concentration of ions formed with most polyprotic acids |
answer
| the first |
question
| What is the third classifcation of acids and bases based on? |
answer
| the bonding and structure. includes substances that do not contain hydrogen at all. |
question
| Who was GN Lewis? |
answer
| The American chemist whose name was give to electron dot structures and famous for third classification. |
question
| What is a Lewis Acid? |
answer
| An atom, ion, or molecule that accpets and electron pair to form a covalent bond. |
question
| which of the three acid definitions is the broadest? Explain. |
answer
| The Lewis definition is the broadest of the 3 acid definitions. It applies to any species that can accept an electron pair to form a covalent bond iwht another species. Ex: H + NH3 = NH4 Ag + 2NH3 = Ag(NH3)2 |
question
| Any compound in which the central atom has 3 valence electrons and forms three covalent bonds can react as a ___? How does it do it? |
answer
| Lewis acid. It odes so by accepting a pair of electrons to form a fourth covalent bond, completing an electron octet. |
question
| What is a Lewis base? |
answer
| An atom, ion, or molecule that donates an electron pair to form a covalent bond. Ex: BF3 + F = BF4 |
question
| what is a Lewis acid-base reaction? |
answer
| It is the formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor. |
question
| The Bronsted-Lowry definitions of acids and bases provide a bases for ___? |
answer
| studying proton transfer reaction. |
question
| What is the conjugate base? |
answer
| the species that remains after a Bronsted-Lowry acid has given up a proton. Ex: HF (acid) + H20 = F (conj b) + H30 |
question
| What is the conjugate acid? |
answer
| The species that is formed when a Bronsted-Lowry base gains a proton. |
question
| What is mean when it is siad that Bronsted-Lowry acid-base reaction are equilibrium system? |
answer
| That both and forward reverse reactions occur. They involve two acid-base pairs, known as conjugate acid-base pairs. HF (acid 1) + H20 (base 2) = F (base 1) + H30 (acid 2) |
question
| In every conjugate acid-base pair, the acid has __ more proton than its conjugate base. |
answer
| one |
question
| The extent of the reaction between a bronsted-lowry acid and base depend on ___. |
answer
| the relative strenghts of the acids and bases involved. |
question
| What is the relationship between the strength of an acid and that of its conjugate base? |
answer
| the stronger an acid is, the weaker its conjugate base. |
question
| What is the relationship between the strength of a base and its conjugate acid? |
answer
| the stronger a base is, the weaker its conjugate acid. |
question
| Proton-transfer reactions favor the production of ____. |
answer
| weaker acid and weaker base. |
question
| A violent proton transfer reaction could result from ____. |
answer
| bringing together a very strong acid and very strong base in certain proportions becaus the reaction has almost no tendency to go in the reverse direction. |
question
| What is amphoteric? |
answer
| Any species that can react as either an acid or a base is described. Ex: H2S04 (acid) + H20 = H30 = HS04. NH3 + H20 = NH4 + 0H |
question
| Molecular compounds containing -OH groups can be ___ and ____. |
answer
| Acidic or amphoteric |
question
| What is a hydroxyle group? |
answer
| it is the covalently bonded OH group in an acid. |
question
| What needs to happen for the compound to be acidic? |
answer
| a water molecule must be able to attract a hydrogen atom from a hydroxyl group. |
question
| Where are the small, more electronegative atoms of nonmetals located? |
answer
| at the upper right in the periodic table. form compounds with acidic hydroxyl group. |
question
| The behavior of a compound is affected by the number of ___. |
answer
| oxygen atoms bonded to the atom connected to the -OH group. |
question
| The larger the number of such oxygen atoms is ___ |
answer
| the more acidic the compound is likely to be. |
question
| An acid-base reaction occurs in aqueous solution between ____. |
answer
| hydrochloric acid, a strong acid that completely dissociates to produce H30 and sodium hydroxide, a strong base that completely dissociates to produce OH. |
question
| What is neutralization? |
answer
| The reaction of hydronium ions and hydroxide ions to form water molecules. |
question
| Water is not hte only product of a neutralization. A salt is also produced. What is a salt? |
answer
| an ionic compound composed of a cation from a base and an anion from an acid. |
Acids and Bases
Chemistry
Conjugate Acid Base Pair
Semester 2 – Flashcards 92 terms
92 terms
Preview
Semester 2 – Flashcards
question
Acid |
answer
| A substance that is a hydrogen ion donor when dissolved in water or involved in a reaction. |
question
Activation Energy |
answer
| The minimum amount of energy required to initiate a chemical reaction. |
question
Activity Series |
answer
| A list of elements ranked according to their reactivity, or the ease with which they undergo a chemical reaction. |
question
Alkaline |
answer
| A term used to describe a solution or substance that has the properties of a base. |
question
Alkane |
answer
| A saturated hydrocarbon which means that all of the carbons are bonded with single bonds. |
question
| Alkene |
answer
| An unsaturated hydrocarbon containing a carbon-carbon double bond. |
question
Alkyne |
answer
| An unsaturated hydrocarbon containing a carbon-carbon triple bond. |
question
Alpha Particle |
answer
| A particle consisting of two protons and two neutrons, like the nucleus of a helium atom, that is given off by certain radioactive elements during nuclear decay. |
question
Angular Momentum Quantum Number |
answer
| Symbolized by l, indicates the sublevel, or type of orbital, an electron is in. |
question
Base |
answer
| A substance that is a hydrogen acceptor in a reaction, or a substance that produces hydroxide ions when dissolved in water. |
question
Beta Particle |
answer
| An electron, or positron, given off when a nucleus breaks down during the nuclear decay of certain radioactive elements. |
question
Biochemistry |
answer
| The study of the chemistry involved with living organisms. |
question
| Biotechnology |
answer
| The application of the knowledge of biochemistry to create new processes or products that are useful to humans. |
question
Buret |
answer
| A measuring instrument made of a long, graduated glass tube with a tap at the bottom that is used to dispense accurate amounts of fluid. |
question
Boiling |
answer
| The change of a liquid to a gas/vapor, both within the liquid and at its surface. |
question
Boiling Point |
answer
| The temperature at which a heated substance changes from a liquid to a gas; the temperature at which the vapor pressure of the liquid is equal to the atmospheric pressure. |
question
Catalyst |
answer
| A substance that speeds up the rate of a chemical process without being consumed by it. |
question
Chain Reaction |
answer
| A series of reactions in which the material or substance that starts a reaction is also produced by the reaction and is available to start another reaction. |
question
Colligative property |
answer
| A property of a solvent that depends on the number of solute particles dissolved in it, but not on the identity or nature of those solute particles. |
question
| Diffusion |
answer
| The gradual mixing of two gases because of the spontaneous, random motion of their particles. |
question
| Condensation Point |
answer
| The temperature at which a given substance changes from a gas to a liquid. |
question
| Condensing |
answer
| Changing a gas/vapor to a liquid. |
question
Dilute |
answer
| Decrease the concentration of a solution by adding additional solvent. |
question
Dynamic Equilibrium |
answer
| A state of balance in which the rates of the forward and reverse reactions are equal even though the forward and reverse reactions continue to occur. |
question
Dipole-Dipole Forces |
answer
| Intermolecular attractions between polar molecules. |
question
Endothermic Process |
answer
| A chemical or physical change that absorbs energy from the surroundings. |
question
Energy |
answer
| The ability to cause change or the ability to do work. |
question
Entropy |
answer
| The property that describes the disorder of a system (S). |
question
| Enzyme |
answer
| A molecule that catalyzes biological reactions. |
question
Equilibrium Constant |
answer
| The value obtained when equilibrium concentrations are plugged into the law of mass action equilibrium expression. The equilibrium constant is represented by the letter K and is constant for a given system at a given temperature. |
question
Equilibrium Position |
answer
A given set of equilibrium concentration values. |
question
Evaporating |
answer
| The change of a liquid to a gas, or vapor, which occurs at the surface of the liquid. |
question
Fission |
answer
| A nuclear reaction in which an atomic nucleus splits into fragments, usually two fragments of comparable mass, with the release of large amounts of energy in the form of heat and radiation. |
question
Free Energy |
answer
| The combined enthalpy-entropy function of a system (G) that helps predict spontaneity. |
question
| Freezing |
answer
| Changing a liquid to a solid. |
question
Freezing Point |
answer
| The temperature at which a given substance changes from a liquid to a solid. |
question
| Fusion |
answer
| A nuclear reaction in which the nuclei of two very small atoms, such as two hydrogen isotopes, combine together into one larger nucleus. |
question
Gamma Rays |
answer
| High-frequency electromagnetic radiation that is emitted by the nuclear decay of a radioactive element. |
question
Gas |
answer
| The state or phase of matter that has an indefinite shape and volume. |
question
Hess's Law; |
answer
| If a process can be written in multiple steps, the enthalpy change of the overall process will be equal to the sum of the enthalpy changes of all the steps. |
question
Heterogeneous Mixture; |
answer
| A mixture in which the composition and properties are not uniform throughout the mixture. |
question
Homogeneous Mixture; |
answer
| A mixture in which the composition and properties are uniform, or the same, throughout the mixture. |
question
Hydrogen Bonding; |
answer
| Intermolecular attractions between two molecules that both contain a hydrogen atom covalently bonded to a strongly electronegative atom (N, O, or F). |
question
Ideal Gas; |
answer
| A model gas that conforms perfectly to all of the assumptions of the kinetic theory. |
question
Indicator; |
answer
| A weak acid or base that changes colors with a change in pH. |
question
Intermolecular Forces; |
answer
| The forces of attraction that occur between individual molecules. |
question
Ion-Dipole Forces; |
answer
| The attraction between the partially charged poles of a polar molecule and charged ions. |
question
| Joule; |
answer
| The SI derived unit used to measure energy or work. |
question
| Law of Conservation of Energy |
answer
| Energy can be converted form one form to another, but it is not created or destroyed in ordinary physical and chemical processes. |
question
Law of Mass Action; |
answer
| A general description of the equilibrium condition, including an equation that defines the equilibrium constant. |
question
LeCh;telier's Principle |
answer
| If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that helps to reduce the effect of that change. |
question
| Liquid |
answer
| The state or phase of matter that has an indefinite shape but a definite volume. |
question
London Dispersion Forces |
answer
| Intermolecular attractions resulting from the constant motion of electrons that create instantaneous and temporary dipoles. |
question
Melting |
answer
| Changing a solid to a liquid. |
question
Melting Point |
answer
| The temperature at which a given substance changes from a solid to a liquid. |
question
Metabolism |
answer
| All of the biochemical reactions occur within a given organism. |
question
Mixture |
answer
| A combination of two or more substances, each retaining its individual composition and properties. |
question
| Molality |
answer
| The concentration of a solution in moles of solute per kilogram of solvent. |
question
Molarity |
answer
| The number of moles of solute in one liter of solution. |
question
Nonrenewable Resources |
answer
| Natural resources that are used at a faster rate than they can be replaced. |
question
Oxidation |
answer
| When a substance loses one or more electrons during a reaction, therefore attaining a higher, more positive, oxidation number. |
question
Oxidation-Reduction Reaction |
answer
| A reaction in which electrons are exchanged from one substance to another, also called redox. |
question
Oxidizing Agent |
answer
| A reactant species containing the element being reduced, causing another substance to be oxidized. |
question
Partial Pressure |
answer
| The individual pressure exerted by one gas in a mixture. |
question
Phase |
answer
| A distinct form of matter in which all chemical and physical properties are identical for a given sample, such as solid, liquid, and gas. |
question
Plasma |
answer
| The state or phase of matter in which the electrons have been separated from the atoms, often called ionized gas. |
question
Precipitate |
answer
| A solid that separates from a solution, usually an insoluble product formed from a chemical reaction in an aqueous solution. |
question
Quantization |
answer
| The concept that energy exists in discrete units or levels. |
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| Quantized |
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| The concept that energy exists in discrete units or levels. |
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Quantum Numbers |
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| Numbers that specify the properties of atomic orbitals and of their electrons. |
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Radioactive Decay |
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| The process by which unstable atomic nuclei break down and release radiation. |
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Reducing Agent |
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| A reactant species containing the element being oxidized in the reaction, causing another substance to be reduced. |
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| Reduction |
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| When a substance gains one or more electrons during a reaction, therefore attaining a lower, more negative, oxidation number. |
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| Renewable Resources |
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| Natural resources that can be replaced at the same rate or even faster than they are used. |
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Saturated Solution |
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| A solution containing the maximum amount of solute able to be dissolved under those conditions. |
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Solid |
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| The state or phase of matter that has a definite shape and volume. |
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Solute |
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| In a solution, the substance that is in a lower quantity, the substance being dissolved. |
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Solution |
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| A homogeneous mixture of two or more substances. |
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Solvent |
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| In a solution, the substance that is in a greater quantity, the dissolving medium. |
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Specific Heat Capacity |
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| The quantity of heat required to raise the temperature of a one gram of the substance by one degree Celsius. |
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Spontaneous |
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| A change in a system that proceeds without a net input of energy from an outside source. |
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Spontaneous Generation |
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| An obsolete theory that organisms can originate from inanimate matter. |
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Thermochemistry |
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| The study of the changes in energy that accompany chemical reactions and physical changes. |
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| Titrant |
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| The solution being added from the buret in a titration. |
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Titration |
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| The controlled addition and measurement of the amount of a solution with a known concentration to a measured volume of a solution with unknown concentration to determine the unknown concentration. |
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Unsaturated Solution |
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| A solution containing less solute than a saturated solution under the given conditions. |
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Vapor |
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| Gas |
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Vapor Pressure |
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| The pressure exerted by the vapor particles that evaporate from a liquid (or solid). |
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Work |
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| The process of causing matter to move against an opposing force. |
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Closed System |
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| A system in which energy is exchanged between the system and surroundings but matter is not exchanged. |
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Open System |
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| A system in which both matter and energy are exchanged freely between the system and the surroundings. |
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| Percent by Mass |
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| The number of grams of solute in 100 grams of solution. |
Acids and Bases
Chemistry
Conjugate Acid Base Pair
chemistry : acids bases and salts 26 terms
26 terms
Preview
chemistry : acids bases and salts
question
t/f: an aqueous solution of acids causes red litmus paper to turn blue.
answer
false
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t/f: an acidic solution contains more hydroxide ions than hydrogen ions.
answer
false
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t/f: acids add flavor to many beverages and foods.
answer
true
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t/f: acid solutions taste bitter and basic solutions taste sour.
answer
false
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t/f: acids and bases have the ability to conduct electricity.
answer
true
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t/f: the relative amounts of hydrogen and hydroxide ions determine whether an aqueous solution is acidic, basic or neutral.
answer
true
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t/f: a conjugate acid is produced when an acid accepts a hydrogen ion.
answer
false
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t/f: substances that can act both an acid and a base are said to be amphoteric.
answer
true
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t/f: the Arrhenius model states that acids and bases share electron pairs.
answer
false
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t/f: An acid is an ion or molecule with a lone electron pair tat it can donate or share.
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false
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t/f: an acid anhydride is an oxide that can combine with water to form a base.
answer
false
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t/f: conjugate acid and bases react to form Bronsted- Lowry acids and bases.
answer
false
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t/f: in solution, strong acids and bases ionize completely, but weak acids and bases ionize only partially.
answer
true
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t/f: a single arrow in a reaction means that the reaction goes to completion.
answer
true
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t/f: weak acids produce fewer ions than strong acids and cannot conduct electricity as well.
answer
true
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t/f: in a typical reaction, if the reacting acid is strong, the base produced is strong.
answer
false
question
t/f: An aqueous solution of acids causes red litmus paper to turn blue.
answer
false
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t/f: a neutral solution contains more hydroxide ion than hydrogen ions.
answer
false
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when acids react with metals, they produce _____ gas.
answer
hydrogen
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a basic solution contains more ____ions than hydrogen.
answer
hydroxide
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a __ Is produced when a base accepts a hydrogen ion from an acid.
answer
conjugate acid
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the ___ of a weak acid is strong.
answer
conjugate base
question
what is the pH of blood, given the hydrogen ion concentration is 4.0 x 10^-8M?
answer
7.4
question
calculate the hydrogen ion concentration of an aqueous solution, given the concentration of hydroxide ions is 1 X 10^-5 and the ion constant for water is 1 X 10^-14.
answer
1 X 10^-9
question
an acid that can donate only one hydrogen ion is called a _____ acid.
answer
monoprotic
question
in the bronsted- lowry model of acids and bases, an ___ is a hydrogen donor and a ___ is a hydrogen acceptor.
answer
acid, base
Acids and Bases
Chemistry
Conjugate Acid Base Pair
Revision for Acids and Bases 36 terms
36 terms
Preview
Revision for Acids and Bases
question
What is the difference between acids and bases?
answer
An acid is a substance that donates H+ ions and a base that donates OH- ions
question
What is the difference between dilute and concentrated?
answer
A concentrated solution has many molecules (less water and more acid/base), whereas a dilute solution has less molecules (more water and less acid/base)
question
What is the unit of concentration?
answer
Molar (M)
question
What is the pH scale?
answer
A scale used for measuring the number of hydrogen ions in solution. Runs from 0-7: 7 > acidic 7 - neutral 7 < Basic
question
What is the proper term for a base?
answer
Alkali
question
What colour changes occur when Universal Indicator is added to an acid and a base?
answer
Acid: Red Base: Blue
question
What are 3 common household bases?
answer
Bleach Nail remover Soap Cement Antacids Washing powders (Most) cleaning products
question
What happens when acids and bases react?
answer
Neutralisation occurs, and water and salt are created as by-products.
question
What happens when acids and metals react?
answer
Hydrogen gas and a salt are produced
question
What are 2 natural occurances of acidic reactions?
answer
acid rain and ocean acidification
question
How does Molarity relate to concentration? (Eg... 2M compared to 0.5M. Which is more concentrated?)
answer
The higher the Molarity the more concentrated the solution is.
question
List examples ratios explaining the difference between dilute and concentrated.
answer
Concentrated- 6 parts water to 4 parts cordial Dilute- 6 parts water to 1 parts cordial
question
How do you read a pH scale? What sections represent acid, base, and neutral?
answer
Read according to the colours. Left section (0-6) is acidic, middle section (7) is neutral and the right section (8-14) is basic.
question
What is another name for a basic solution?
answer
Alkali.
question
How do liquid pH indicators work?
answer
Chemicals in the indicators change colour when they are added to the acid or base.
question
What is a way to produce more reliable results when measuring pH?
answer
By conducting multiple trials and/or using different indicators.
question
How does acid rain affect structures around the world?
answer
The slight acidity in rain (caused by pollution in the air) destroys marble structures and other stones/metals/objects.
question
What are 3 differences between acids and bases?
answer
An acid is a substance that releases hydrogen ions into an aqueous solution. A base is a substance that releases hydroxide ions. Acids have a pH of less than 7. Bases have a pH of more than seven. Bases are caustic and acids are corrosive. Acids have a sour taste and bases have a bitter taste.
question
What does Molarity (M) refer to?
answer
Molar (M) refers to the concentration of the acid or base. The higher the Molarity, the higher the concentration.
question
What causes natural chemicals to become indicators? (What is the agent in these natural chemicals?)
answer
Natural chemicals such as cabbage juice all contain a chemical called anthocyanin. Anthocyanin is a pigment/colouring agent that is a complex molecule. It changes its structure and reaction according to the acidity of the environment it is exposed to.
question
What are different types of indicators that can be used to determine pH?
answer
Universal indicator, methyl orange, red cabbage juice, bromothymol blue, phenol red, azolitmin.
question
How does Ocean Acidification impact oceans?
answer
Ocean acidification is also a huge issue, changing the acidity levels that fish are adapted to - therefore causing many fish to die and affecting humanity's supply of fish.
question
What happens to a solution when a universal indicator is added to it?
answer
The solution changes colour and the pH can be determined by comparing the colour of the solution to the pH chart.
question
Can red cabbage juice be used to determine the pH of solutions?
answer
Red cabbage juice CAN be used as a pH indicator. A specific indicator chart is needed.
question
What happens if you mix a base with a pH level of 8 with an acid with a pH level of 6?
answer
Neutralisation occuurs: the solution becomes Neutral- with a pH level of 7.
question
I have 2 beakers filled with the same volume of acid. I added 200mL of water to beaker A and 100mL of water to beaker B. Which acid would be more diluted?
answer
Beaker A would be more diluted, as there would be less acid molecules in the solution compared to beaker B.
question
For every number you move DOWN the pH scale the concentration of hydrogen ions increases. By what factor does this number increase?
answer
The concentration increases by 10 every number you move down the pH scale.
question
Most pH indicators are made from natural substances, name two fruits or vegetables that can be utilized as a pH indicator.
answer
Red Cabbage, Blue berries, Carrots, Grapes, etc.
question
How do you identify the pH of a substance using a pH scale?
answer
The concentration of hydrogen ions (H+) in a solution is measured using the pH scale. Using the pH scale, substances matching to the colour of pH 7 are neutral, substances matching to the colour of pH more than 7 are basic and substances matching to the colour of pH less than 7 are acidic.
question
What are pH indicators?
answer
pH indicators are chemicals (often natural) and indicate the concentration of H+ ions in a solution via colour change. With the colour change the substance being tested can be identified as acidic, basic, or neutral .
question
List 4 common types of acid/base indicators used to determine pH.
answer
Methyl orange Universal indicator Litmus paper Phenolphthalein pH meter
question
How does ocean acidification affect the environment? Give an example of how it affects an organism.
answer
Marine organisms that use calcium carbonate for the creation of their shells or skeletons will be in danger because increased acidity will make their shells/skeletons dissolve.
question
The more diluted a mixture is, the more water it has in it , the more concentrated a mixture is, the less water it has in it. True or false?
answer
True.
question
The unit of concentration is molar (M). If a mixture is 3M, it would be more concentrated than a mixture of 1M. True of false?
answer
True
question
Name an impact that acid has on the environment and how this impact is caused.
answer
Ocean Acidification- caused by COâ‚‚ being dumped in the ocean, mixing with water and forming an acid Acid Rain- caused by pollution Global Warming- greenhouse gases forming a hole in the ozone layer
question
What are 3 common household acids?
answer
Lemon juice (any juice) Vinegar Vitamin C Apples Bananas Tea
