Term
|
Definition
| a compound that donates H+ ions to a solution; pH <7 |
|
|
Term
|
Definition
| a compound that removes H+ ions from aqueous solution or donates OH-; pH >7 |
|
|
Term
|
Definition
| describes how acidic or basic a solution is |
|
|
Term
|
Definition
| the study of energy changes that occur during chemical reactions and changes in state |
|
|
Term
|
Definition
| the process of adding a known amount of solution of known concentration to determine the concentration of another solution |
|
|
Term
|
Definition
| the theory that all matter is composed of particles (atoms and molecules) moving constantly in random directions |
|
|
Term
|
Definition
| direct relationship between temperature and volume |
|
|
Term
|
Definition
| inverse relationship between volume and pressure |
|
|
Term
|
Definition
| when the forward rate of a chemical reaction is the same as the reverse rate. This only takes place in reversible reactions because these are the only type of reaction in which the forward and backward reactions can both take place. |
|
|
Term
|
Definition
| the apparent charge on an atom. |
|
|
Term
|
Definition
| the art of figuring how much stuff you'll make in a chemical reaction from the amount of each reagent you start with. |
|
|
Term
|
Definition
| reaction that has both an oxidation and reduction. |
|
|
Term
|
Definition
| when a substance loses electrons. |
|
|
Term
|
Definition
| compound that turns different colors at different pH values. We generally like to have the color change at a pH of around seven because that's where the equivalence point of a titration is. |
|
|
Term
|
Definition
| time required for half of the radioactive atoms in a sample to decay. When talking about chemical reactions, it's the amount of time required to make half the reagent react. |
|
|
Term
|
Definition
| minimum amount of energy needed for a chemical reaction to take place. |
|
|
Term
|
Definition
| pressure of a gas varies directly with its temperature when volume is held constant |
|
|
Term
|
Definition
Ionic crystal is immersed in a solvent
Ions become solvated and break away from the crystal
The crystal is completly broken apart as all of the ions become solvated, and a solution of solvated (aqueous) ions results |
|
|
Term
|
Definition
| solute is dissolved in a solvent, it will not conduct electricity. |
|
|
Term
|
Definition
|
|
