Term
|
Definition
| a uniform mixture of two or more substances |
|
|
Term
|
Definition
| the component present in the largest amount; in an aqueous solution this is water |
|
|
Term
|
Definition
| the components present in smaller amounts than the solvent; may contain one or more |
|
|
Term
|
Definition
| a concentration unit; it is the amount of solute (in moles) divided by the volume of a solution (in liters) |
|
|
Term
|
Definition
| a concentrated solution of a substance used to prepare solutions of lower concentrations |
|
|
Term
|
Definition
| the process of lowering the concentration of a solution by adding more solvent |
|
|
Term
|
Definition
| a substance that dissociates into ions when it dissolved, enhancing the conductivity of the solvent |
|
|
Term
|
Definition
| a substance that dissociates completely into ions when it dissolves in water |
|
|
Term
|
Definition
| a substance that does not form ions and does not enhance the conductivity of water when it dissolves |
|
|
Term
|
Definition
| only partly ionizes when it dissolves in water |
|
|
Term
|
Definition
| the form in which the hydrogen ion is found in an aqueous solution |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| takes place when an acid reacts with a base and produces a solution of salt in water |
|
|
Term
|
Definition
| the product of a neutralization reaction; a salt is made up of the cation characteristics of the base and anion characteristics of the acid in the reaction |
|
|
Term
|
Definition
| describes a reaction in solution in which the reactants are written as undissociated molecules |
|
|
Term
|
Definition
| shows all the species, both ionic and molecular, present in a reaction occurring in aqueous solution |
|
|
Term
|
Definition
| describes the actual reaction taking place in aqueous solution, and is found by eliminating the spectator ions |
|
|
Term
|
Definition
| present in, but remain unchanged by, the reaction taking place |
|
|
Term
|
Definition
| completely ionized in aqueous solution |
|
|
Term
|
Definition
| weak electrolyte and only partially ionized in aqueous solution, it has a limited capacity to donate protons to the medium |
|
|
Term
|
Definition
| completely ionized in aqueous solution |
|
|
Term
|
Definition
| weak electrolyte and only partially ionized in aqueous solution; has a limited capacity to accept protons in the medium |
|
|
Term
|
Definition
| substance can behave as either an acid or a base |
|
|
Term
|
Definition
| a solid product formed from a reaction in solution |
|
|
Term
|
Definition
| contains more than the quantity of a solute that is predicted to be soluble in a given volume of solution at a given temperature |
|
|
Term
|
Definition
| a process by which one ion is exchanged for another; usually carried out, 2+ ions in water that contribute to its hardness are removed from the water that in exchange for sodium ions |
|
|
Term
|
Definition
| natural crystalline minerals or synthetic material consisting of 3D networks of channels that contain sodium or other 1+ cations; they may function as ion exchanged |
|
|
Term
|
Definition
| a chemical change in which a species loses electrons; oxidation number decreases |
|
|
Term
|
Definition
| a chemical change in which a species gains electrons; oxidation number decreases |
|
|
Term
Oxidation Number
(Oxidation State) |
|
Definition
| a positive or negative number bases on the number of electrons that each atom of the element gains or loses when it forms an ion or that it shares when it forms a covalent bond with another element |
|
|
Term
|
Definition
| in a redox reaction accepts electrons from another species, thereby oxidizing that species; itself is reduced |
|
|
Term
|
Definition
| in a redoz reaction gives up electrons to another species, thereby reducing that species; itself is oxidezed |
|
|
Term
|
Definition
| one for the oxidation component and one for the reduction component |
|
|
Term
|
Definition
| an analytical method for precisely determining th e concentration of a solute in a sample by reacting it with a standard solution of known concentration |
|
|
Term
|
Definition
| a solution of known concentration |
|
|
Term
|
Definition
| the standard solution added to the sample in a titration |
|
|
Term
|
Definition
| the point where the number of moles of titrant added is stoichemetrically equal to the number of moles of the substance being analyzed |
|
|
Term
|
Definition
| reached when just enough standard solution has been added causing the indicator to change color |
|
|
