Chapter 13- Chapter 16 – Flashcards
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Soluble |
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| -capable of being dissolved |
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Solution |
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| - homogeneous mixture of two or more substance in a single phase |
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Solvent |
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| -the dissolving medium in a solution |
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Solute |
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| - substance dissolved in a solution |
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Suspension |
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| - if the particles in a solvent are so large that they settle out unless mixed |
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Colloids |
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| - particles that are intermediate in size between those in solutions and suspensions form mixtures known as colloidal dispersions |
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Tyndall Effect |
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| - the visible path of light produced by the scattering action of the particles in a colloidal solution on a beam of light passed through it |
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Electrolyte- |
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| a substance that dissolves in water to give a solution that conducts electric current (non electrolye) |
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Solution equilibrium |
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| - physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates |
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Saturated solution |
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| - a solution that contains the maximum amount of dissolved solute |
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Unsaturated solution |
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| - solution that contains less solute than a saturated solution under existing conditions |
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Supersaturated solution |
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| - a solution that contains more dissolved solute than a saturated solution contains under the same conditions |
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Solubility |
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| - amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature |
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Hydration |
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| - solution process with water as the solvent |
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Immiscible |
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| - liquid solutes and solvents that are not soluble in each other |
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Miscible |
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| - liquid that dissolve freely in one another in any proportion |
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Henry’s law |
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| - the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid |
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Effervescence |
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| - the rapid escape of a gas from a liquid (soda) |
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Solvated |
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| - a solute particle that is surrounded by solvent molecules |
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Heat of solution |
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| - the net amount of heat energy absorbed or released when a specific amount of solute dissolves in a solvent |
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Molarity |
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moles solute/volume of solution (L)
moles solute/mass of solvent (kg)
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Dissociation- |
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| the separate of ions that occurs when an ionic compound dissolves |
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Net ionic equation |
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| - includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution |
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Spectator ions |
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| - ions that do not take part in a chemical reaction and are found in solution both before and after the reaction |
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Ionization |
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| -ions are formed from solute molecules by the action of the solvent (process) |
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Hydronium |
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| - h3o+ |
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Strong electrolyte |
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| - any compound of which all or almost all of the dissolved compound exists as ions in an aqueous solution |
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Weak electrolyte |
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| - compound of which a relatively small amount of the dissolved compound exists as ions in an aqueous solution |
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Colligative properties |
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| - properties that depend on the concentration of solte particles but not on their identity |
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Non-volatile substance |
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| one that has little tendency to become a gas under existing conditions |
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Semipermeable membranes |
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| - allow the movement of some particles, while blocking some |
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Osmosis |
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| - the movement of a solvent through a semipermeable membrane from the side of lower solute concentration to the side of higher concentration |
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Osmotic pressure |
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| - external pressure that must be applied to stop osmosis |
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Binary acid |
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| - acid that contains two elements: one hydrogen and one other more electronegative element (say hydro-) |
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Oxyacid |
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| : acid compound that contains hydrogen, oxygen, and a third element, usually a nonmetal (just say anion) |
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HF- HBr-
HClO- HNO3-
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Hydrofluoric Hydrobromic hypochlorous nitric
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| Acid prop: |
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Base prop- |
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Arrhenius acid- |
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| chem.. compound that increase the concentration of hydrogen ions in an aqueous solution |
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Strong acid |
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| - one that ionizes completely in an aqueous solution |
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Weak acid- |
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| acids that are weak electrolytes |
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Alkaline |
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| - when a base completely dissociates in water to yield aqueous OH- ions |
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Bronsted-lowry acid |
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| molecule or ion that is a proton donor |
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Bronsted lowry base |
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| : molecule or ion that is a proton acceptor, produces OH- |
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Monoprotic acid |
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| : an acid that can only donate 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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Diprotic acid: |
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| PP acid that can donate two protons per molecule |
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Triprotic: |
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| an acid that can donate three protons per molecule |
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Lewis acid: |
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| accepts electron pair to form a covalent bond |
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Lewis base: |
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| atom, ion, or molecule that donates an electron pair to form a cov. Bond |
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Lewis acid-base reaction |
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| : 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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| : species that remain after a bronsted lawry base has given up a proton |
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Conjugate acid |
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| : species that is formed when a bronsted lawry base gains a proton |
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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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Neutralization: |
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| reaction of hydronium ions and hydroxide ions to form water |
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Salt |
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| - ionic compound composed of a cation from a base and an anion from an acid |
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Self-ionization of water: |
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| two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton |
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pH- |
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| negative of the common logarithm of the hydronium ion concentration |
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pOH- |
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| negative of the common log of the hydroxide concentration |
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Acid-base indicator |
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| - compounds whose color are sensitive to pH |
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Transition interval |
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| - pH range over which an indicator changes color |
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pH meter- |
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| determines the pH of a solution by measuring the voltage between the two electrode that are placed in the solution |
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Titration |
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| controlled addiction and measurement of the amount of a solution of known concentration required to react completely with a measured amount of solution of unknown concentration |
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Equivalence point |
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| - the point at which the two solutions used in a titration are present in chemically equivalent amounts |
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End point |
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| - the point in a titration at which an indicator changes color |
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| standard solution: |
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| the solution that contains precisely known concentration of a solute |
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Primary standard- |
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| highly purified solid compound used to check the concentration of the known solution in a titration |
