| A | B |
|---|
| aqueous solution | A solution in which water is the dissolving medium or solvent |
| half-reactions | The two parts of an oxidation-reduction reaction, one representing oxidation, the other reduction. |
| hydration | The interaction between solute particles and water molecules. |
| solubility | The amount of a substance that dissolves in a given volume of solvent at a given terperature. |
| solute | A substance dissolved in a liquid to form a solution. |
| solvent | The dissolving medium in a solution. |
| electrical conductivity | The ability to conduct an electric current. |
| strong electrolyte | A meterial that, when dissolved in water, gives a solution that conducts an electric current very efficiently. |
| weak electrolyte | A material which, when dissolved in water, gives a solution that conducts only a small electric current. |
| nonelectrolyte | A substance that, when dissolved in water, gives a nonconducting solution. |
| acid | A substance that produces hydrogen ions in solution; a proton donor. |
| strong acid | An acid that completely dissociates to produce an H+ ion and the conjugate base. |
| strong base | A metal hydroxide salt that completely dissociates into its ions in water. |
| weak acid | An acid that dissociates only slightly in aqueous solution. |
| weak base | A base that reacts with water to produce hydroxide ions to only a slight extent in aqueous solution. |
| molarity | Moses of solute per volume of solution in liters. |
| standard solution | A solution whose concentration is accurately known. |
| dilution | The process of adding solvent to lower the concentration of solute in a solution. |
| precipitation reaction | A reaction in which an insoluble substance forms and separates from the solution. |
| precipitate | An insoluble substance that forms when two solutions are mixed. |
| molecular equation | An equation representing a reaction in solution showing the reactants and products in undissociated form, whether they are strong or weak electrolytes. |
| complete ionic equation | An equation that shows all substances that are strong electrolyes as ions. |
| spectator ions | Ions present in solution that do not participate directly in a reaction. |
| net ionic equation | An equation for a reaction in solution, where strong electrolytes are written as ions, showing only those components that are directly involved in the chemical change. |
| polar molecule | A molecule that has a permanent dipole moment |
| neutralization reaction | An acid-base reaction. |
| volumetric analysis | A process involving titration of one solution with another. |
| titration | A technique in which one solution is used to analyze another. |
| stoichiometric (equivalence) point | The point in a titration when enough titrant has been added to react exactly with the substance in solution being titrated. |
| indicator | A chemical that changes color and is used to mark the end point of a titration. |
| endpoint | The point in a titration at which the indicator changes color. |
| oxidation-reduction (redox) reaction | A reaction in which one or more electrons are transferred. |
| oxidation state | A concept that provides a way to keep track of electrons in oxidation-reduction reactions according to certain rules. |
| oxidation | An increase in oxidation state (a loss of electrons). |
| reduction | A decrease in oxidation state (a gain of electrons). |
| oxidizing agent (electron acceptor) | A reactant that accepts electrons from another reactant. |
| reducing agent (electron donor) | A reactant that donates electrons to another substance to reduce to reduce the oxidation state of one of its atoms. |
| base | A substance that produces hydroxide ions in aqueous solution; a proton acceptor. |
