Term
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Definition
| -capable of being dissolved |
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Term
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Definition
| - homogeneous mixture of two or more substance in a single phase |
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Term
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Definition
| -the dissolving medium in a solution |
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Definition
| - substance dissolved in a solution |
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Term
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Definition
| - if the particles in a solvent are so large that they settle out unless mixed |
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Term
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Definition
| - particles that are intermediate in size between those in solutions and suspensions form mixtures known as colloidal dispersions |
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Term
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Definition
| - 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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Term
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Definition
| a substance that dissolves in water to give a solution that conducts electric current (non electrolye) |
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Term
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Definition
| - physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates |
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Term
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Definition
| - a solution that contains the maximum amount of dissolved solute |
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Term
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Definition
| - solution that contains less solute than a saturated solution under existing conditions |
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Term
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Definition
| - a solution that contains more dissolved solute than a saturated solution contains under the same conditions |
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Term
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Definition
| - amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature |
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Term
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Definition
| - solution process with water as the solvent |
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Term
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Definition
| - liquid solutes and solvents that are not soluble in each other |
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Term
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Definition
| - liquid that dissolve freely in one another in any proportion |
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Term
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Definition
| - 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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Term
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Definition
| - the rapid escape of a gas from a liquid (soda) |
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Term
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Definition
| - a solute particle that is surrounded by solvent molecules |
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Term
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Definition
| - the net amount of heat energy absorbed or released when a specific amount of solute dissolves in a solvent |
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Term
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Definition
moles solute/volume of solution (L) moles solute/mass of solvent (kg) |
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Term
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Definition
| the separate of ions that occurs when an ionic compound dissolves |
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Term
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Definition
| - includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution |
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Term
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Definition
| - 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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Term
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Definition
| -ions are formed from solute molecules by the action of the solvent (process) |
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Term
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Definition
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Term
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Definition
| - any compound of which all or almost all of the dissolved compound exists as ions in an aqueous solution |
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Term
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Definition
| - compound of which a relatively small amount of the dissolved compound exists as ions in an aqueous solution |
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Term
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Definition
| - properties that depend on the concentration of solte particles but not on their identity |
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Term
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Definition
| one that has little tendency to become a gas under existing conditions |
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Term
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Definition
| - allow the movement of some particles, while blocking some |
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Term
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Definition
| - 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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Term
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Definition
| - external pressure that must be applied to stop osmosis |
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Term
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Definition
| - acid that contains two elements: one hydrogen and one other more electronegative element (say hydro-) |
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Term
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Definition
| : acid compound that contains hydrogen, oxygen, and a third element, usually a nonmetal (just say anion) |
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Term
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Definition
Hydrofluoric Hydrobromic hypochlorous nitric |
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Term
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Definition
- sour taste,
- change color of acid-base indicators,
- acids react with metals to produce hydrogen gas,
- acids react with base to produce salts and water
- some conduct electricity
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Term
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Definition
- bitter taste,
- chance color of acid-base,
- feel slippery when dilute,
- reacts with acids to produce salts and water,
- always conduct
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Term
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Definition
| chem.. compound that increase the concentration of hydrogen ions in an aqueous solution |
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Term
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Definition
| - one that ionizes completely in an aqueous solution |
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Term
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Definition
| acids that are weak electrolytes |
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Term
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Definition
| - when a base completely dissociates in water to yield aqueous OH- ions |
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Term
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Definition
| molecule or ion that is a proton donor |
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Term
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Definition
| : molecule or ion that is a proton acceptor, produces OH- |
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Term
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Definition
| : an acid that can only donate one proton (hydrogen ion) per molecule |
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Term
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Definition
| : an acid that can donate more than one proton per molecule |
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Term
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Definition
| PP acid that can donate two protons per molecule |
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Term
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Definition
| an acid that can donate three protons per molecule |
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Term
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Definition
| accepts electron pair to form a covalent bond |
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Term
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Definition
| atom, ion, or molecule that donates an electron pair to form a cov. Bond |
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Term
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Definition
| : formation of one or more covalent bonds between an electron-pair donor and electron-pair acceptor |
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Term
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Definition
| : species that remain after a bronsted lawry base has given up a proton |
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Term
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Definition
| : species that is formed when a bronsted lawry base gains a proton |
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Term
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Definition
| : any species that can react as either an acid or a base |
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Term
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Definition
| reaction of hydronium ions and hydroxide ions to form water |
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Term
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Definition
| - ionic compound composed of a cation from a base and an anion from an acid |
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Term
Self-ionization of water: |
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Definition
| two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton |
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Term
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Definition
| negative of the common logarithm of the hydronium ion concentration |
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Term
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Definition
| negative of the common log of the hydroxide concentration |
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Term
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Definition
| - compounds whose color are sensitive to pH |
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Term
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Definition
| - pH range over which an indicator changes color |
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Term
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Definition
| determines the pH of a solution by measuring the voltage between the two electrode that are placed in the solution |
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Term
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Definition
| 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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Term
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Definition
| - the point at which the two solutions used in a titration are present in chemically equivalent amounts |
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Term
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Definition
| - the point in a titration at which an indicator changes color |
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Term
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Definition
| the solution that contains precisely known concentration of a solute |
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Term
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Definition
| highly purified solid compound used to check the concentration of the known solution in a titration |
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