Terms : Hide Images
| 6705014489 | aqueous solution | a solution in which the water is the dissolving medium | 0 | |
| 6705014490 | solution | homogeneous mixture of two or more substances | 1 | |
| 6705014491 | solvent | substance present in the greatest quantity and the one the dissolves the other substances | 2 | |
| 6705014492 | solute | the substances in a solution that are being dissolved (of the least quantity) | 3 | |
| 6705014493 | dissociation | the separation into component ions that occurs when an ionic compound dissolves | 4 | |
| 6705014494 | electrolyte | a substance whose aqueous solutions contain ions, commonly with ionic compounds | 5 | |
| 6705014495 | nonelectrolyte | a substance that does not form ions in solution, commonly molecular compounds | 6 | |
| 6705014496 | solvation | process that helps stabilize the ions in solution and prevents the cations and anions from recombining; this process is symbolized by aq in reactions and causes ions to become dispersely uniform throughout a solution | 7 | |
| 6705014497 | strong electrolytes | solutes that exist in solution completely or nearly completely as separate ions; fully or almost fully dissociate; in chemical equations, represented by a full arrow | 8 | |
| 6705014498 | weak electrolytes | solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions; do not completely dissociate; in a chemical equation, represented by two half arrows | 9 | |
| 6705014499 | chemical equilibrium | balance that produces a state in which the relative numbers of each type of ion or molecule in the reaction are constant over time | 10 | |
| 6705014500 | precipitation reaction | reaction that results in the formation of an insoluble product | 11 | |
| 6705014501 | precipitate | an insoluble solid formed by a reaction in solution | 12 | |
| 6705014502 | solubility | amount of substance that can be dissolved in a given quantity of solvent at the given temperature (at a given temperature) | 13 | |
| 6705014503 | insoluble | A substance is described as ______ if they have a solubility less than 0.01 mol/L | 14 | |
| 6705014505 | molecular equation | an equation that shows the complete chemical formulas of the reactants and products without indicating ionic behavior |  | 15 |
| 6705014506 | ionic equation | an equation written with all strong soluble electrolytes shown as ions |  | 16 |
| 6705014507 | spectator ions | ions that appear in identical forms among both the reactants and products of a complete ionic equation | 17 | |
| 6705014508 | net ionic equation | an equation for a reaction in solution showing only those particles that are directly involved in the chemical change |  | 18 |
| 6705014509 | acid | substance that ionizes in aqueous solutions to form hydrogen ions, thereby increasing the concentration of H+(aq) ions; often called proton donors | 19 | |
| 6705014510 | monoprotic acids | acids that yield one H+ per molecule of acid ex) HCl, HNO3 | 20 | |
| 6705014511 | diprotic acids | acids that yield two H+ per molecule of acid ex) H2SO4 | 21 | |
| 6705014512 | base | substance that accepts (reacts with) H+ ions and produce hydroxide ions (OH-) when they dissolve in water; there are common ____s that do not contain hydroxide, however, like NH4 | 22 | |
| 6705014513 | strong acids | acids that are strong electrolytes (completes ionized in solution) | 23 | |
| 6705014517 | weak acids | acids that are weak electrolytes (partly ionize in solution) | 24 | |
| 6705014519 | neutralization reaction | the reaction that occurs when a solution of an acid and a solution of a base are mixed | 25 | |
| 6705014520 | salt | any ionic compound whose cation comes from a base and whose anion comes from an acid; ____ and water are the products of neutralization reactions | 26 | |
| 6705014521 | oxidation-reduction (redox) reaction | reaction in which electrons are transferred between reactants | 27 | |
| 6705014522 | oxidation | loss of electrons by a substance | 28 | |
| 6705014523 | reduction | gain of electrons by a substance, and therefore increase in negative charge | 29 | |
| 6705014524 | oxidation number | either the actual charge of a monatomic ion or the hypothetical charge assigned to an atom in a neutral molecule or charged species | 30 | |
| 6705014525 | 0 | oxidation number of single elements | 31 | |
| 6705014529 | molarity units | mol/L | 32 | |
| 6705014530 | molarity | the concentration of a solution | 33 | |
| 6705014531 | dilution | process in which solutions of lower concentrations can be obtained by adding water | 34 |
