| A | B |
|---|
| solution | solvent + solute |
| solute | material being dissolved |
| solvent | material doing the dissolving |
| aqueous | in water |
| electrolyte | contains ions that conduct electricity |
| dissociate | come apart |
| soluble | will dissolve |
| KOH | a base |
| HCl | an acid |
| net ionic equation | balanced equation without spectator ions |
| spectator ions | ions found on both sides of a balanced equation |
| exchange reaction | double replacement reaction |
| precipitation reaction | produces a solid, insoluble product |
| insoluble | won't dissolve |
| acid-base reaction | also called a neutralization reaction |
| gas-forming reaction | usually involves a metal carbonate and acid to produce carbon dioxide |
| carbonic acid (H2CO3) | breaks down into water and carbon dioxide gas |
| salt | any ionic compound resulting from a basic cation and an acid anion |
| molarity | concentration found by dissolving moles of solute by liters of solution |
| dilution method | using a concentrated solution to make a less concentrated one |
| titration | method of determining the moles of a substance present in a solution |
| indicator | substance that changes color with pH |
| equivalence point | when the number of moles of OH- added equal the number of moles of H+ |
| hydronium ion | H3O+ (what happens to H+ in water) |
| standardization | determining the exact concentration of a substance by titration |
| oxidation | loss of an electron or H atom |
| reduction | gain of an electron or H atom |
| redox reaction | reaction in which electrons or H atoms are transferred |
| oxidation number | the charge that an element APPEARS to have WITHIN a compound |
| 0 (zero) | oxidation number of a free element |
