Chapter 7 – Chemistry Test Questions – Flashcards
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| mixture |
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| combination of two or more pure substances, both retain identity |
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| homogeneous mixture |
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| synonym for solution has same composition throughout |
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| heterogeneous mixture |
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| mixture that does not have same composition throughout |
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| colloid |
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| homogeneous mixture that contains larger particles |
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| will a colloid settle |
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| no |
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| suspension |
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| heterogeneous mixture with larger particles |
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| will a suspension settle |
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| yes |
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| solvent |
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| liquid in which anouther substanc eis dissolved |
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| solute |
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| substance dissolved in a liquid |
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| solvation |
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| clustering of solvent molecules around a dissolved solutes molecules or ions |
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| example of when solvation would happen |
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| when salt is dissolved in water |
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| hygroscopic |
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| having the ability to ull water molecules from the surrounding atmosphere |
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| what do we call it when water is the solvent |
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| hydration |
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| saturated solution |
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| solution containing the maximum amoung of solute that will dissolve |
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| solubility |
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| maximum amount of a substance that will dissolce in a given amountof solvent at a particular temperature |
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| miscible |
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| mutally soluble in all proportions |
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| immiscible |
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| opposite of miscible (insolubility) |
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| which is clear, a solution or a colloid |
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| a solution |
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| what is the particle size in a solution |
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| less that 2.0 nm |
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| what is the particle size in a colloid? |
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| between 2.0 and 500 nm |
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| what is the particle size in a suspension |
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| more than 500 nm |
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| air,seawater and gas are all examples of |
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| solutions |
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| butter, milk and fog are examples of |
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| colloid |
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| blood and paint are examples of |
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| suspension |
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| characteristics of a solution |
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| transparent, not filterable, does not seperate |
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| could a solution be colored |
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| yes |
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| is a solution filterable |
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| no |
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| characteristic of colloids |
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| murky or opaque, does not seperate |
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| is a colloid filterable |
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| no |
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| characteristics of a suspension |
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| murky or opaque, seperates on standing |
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| is a suspension filterable |
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| yes |
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| are gases suspensions, solutions or colloids? |
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| solutions |
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| moving from a solution to a solid solute is called |
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| crystallization |
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| moving from a solid solute to a solution is called |
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| dissolution |
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| does heat generally increase or decrease solubility |
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| increase |
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| how would you make a supersaturated solution |
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| saturate the solution at a higher temperature, then let the solution cool undisturbed |
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| after a solution has been supersaturated and cooled, what would a disturbance do to the solution |
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| cause it to crystallize |
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| is supersaturation a stable state? |
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| no |
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| the solution process needs similar or compatible |
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| intermolecular forces |
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| what does "like dissolves like" mean |
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| non-polar substances will dissolve in non-polar solutions and polar substances will dissolce in polar substances |
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| heat change when dissolving can be |
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| positive or negative |
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| is dissolving a static process |
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| no, there is a lot of back and forth |
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| rate of dissolving is dependant on |
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| surface area (rock candy vs powdered sugar. |
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| what two factors can increase the rate of dissolving |
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| heat and stirring |
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| how do heat and stirring speed up rate of dissolving |
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| by increasing the rate at which molecules collide |
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| stirring also increases rate by |
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| moving solvaed molecules further from the pure solvent |
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| molarity |
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| moles of solution over liters solution |
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| weight/volume percent |
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| mass of solute/volume of solution |
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| what are the units for weight/volume percent |
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| grams of solute/100 mL solution |
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| how would you write weight volume as a conversion factor |
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| parts per one hundred (grams over 100 mL) |
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| dilution formula |
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| m1v1=m2v2 |
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| in a dilution formula, what do the variables stand for? |
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| m1=concentration of concetrated, v1=volume of concentrated, m2=concentration of diluted, v2= concentration of diluted |
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| what units do you need to use when using the dilution equation? |
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| it doesn't matter as long as they are the same on both sides |
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| Is the volume used in the dilution problem total volume or added volume? |
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| total volume |
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| what must be used as the common unit when doing stoichiometry equations? |
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| moles |
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| electrolytes |
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| produces ions when dissolved in water adn therefore conducts electricity. |
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| what has to happen for a dissolved compound to conduct electricity? |
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| the compound must dissociate into ions |
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| strong electrolytes |
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| dissociates completely in water |
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| weak electrolytes |
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| partially dissociates in water |
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| nonelectrolytes |
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| do not dissociate in water |
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| colligative particles depend only on |
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| the number of particles, not their chemical identity |
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| colligative properties (vapor pressure) |
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| lowers |
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| colligative properties (boiling point) |
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| elevation |
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| colligative properties (freezing point) |
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| depression |
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| colligative properties (osmosis) |
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| osmosis |
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| how do colligative properties lower vapor pressure? |
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| the solute makes the liquid less concentrated, therefore fewer particles will be in the vapor phase |
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| how do colligative properties elevate boiling points? |
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| if the vapor pressure is lower at a particular tamperature, to get the vapor pressure to atmospheric pressure, the temperature must be raised. |
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| The boiling point of 1 kg of water is increased by how many degrees celcius for each mole of particles? |
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| 0.51 degrees celcius |
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| How do colligative properties depress the freezing point? |
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| if there are contaminants in the liquid (solvent) it is harder for the liquid molecules to form a crysal lattice. |
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| the temperature water freezes at is lowered by how many degrees for each mol of particles per 1 kg of water? |
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| 1.86 degrees |
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| is osmosis only (blank) can pass through membrane |
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| solvent |
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| osmotic pressure |
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| the pressure that must be applied to the contaminated solution to half the flow of solvent into that chamber |
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| osmolarity is the sum of |
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| the molarities for all dissolved particles in a solution |
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| osmotic pressure equation |
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| osmotic pressure =nMRT |
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| what number is used for the constant (R) in the equation for osmotic pressure |
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| 62.4 L torr/k mol |
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| isotonic solution |
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| 0.30 osmol. Water will not flow in or out of cell, cell stays normal size |
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| hypotonic solution |
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| less than 0.30 osmol. water flows into the cell, the cell bursts |
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| hypertonic solution |
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| greater than 0.30 osmol. water flows out of the cell, cell creanates |
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| how does dialysis differ from osmosis |
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| small particles as well as solvent can diffuse through the semipermeable membrane |
