| A | B |
|---|
| heterogeneous mixture | one in which the substances are not spread uniformly |
| homogeneous mixture | one in which the substances are spread uniformly throughout |
| solution | homogeneous mixture composed of very small particles |
| properties of a solution | clear and transparent; will not separate on standing; is not changed by filtration |
| solute | dissolved substance of solution is present to a lesser degree |
| solvent | the dissolving substance of solution is present to a greater degree |
| aqueous solutions | solutions where the solvent is water |
| tinctures | solutions where the solvent is alcohol |
| gas solution | a mixture of gases or vapors |
| liquid solution | mixture in which a gas, liquid, or solid is dissolved in a liquid solvent |
| miscible | term used to describe liquids that can dissolve in one another |
| immiscible | term used to describe liquids that cannot dissolve in one another |
| solid solution | mixture of solids uniformly spread throughout one another at the atomic or molecular level |
| alloy | solid solution of two or more metals |
| brass | an alloy of copper and zinc |
| amalgam | an alloy in which one of the metals is mercury |
| solute and water | lowers freezing point and raises boiling point of water |
| hydrometer | instrument that measures the specific gravity of a substance |
| solubility | the maximum quantity of solute that can be dissolved in a certain quantity of solvent at a specific temperature |
| factors affecting solubility | nature of substances, temperature, pressure |
| effervescence | the escape of a dissolved gas from a solution |
| factors affecting rate of solution | particle size, stirring, solute already dissolved, temperature |
| rate of solution | measure of how quickly a solute dissolves in the solvent |
| hydrated ion | a charged particle surrounded by water molecules |
| solubility curve | graph that indicates how much solute will dissolve in a given amount of solvent over a range of temperatures |
| saturated solution | solution that has all the solute dissolved in it that it can normally hold at a certain temperature and pressure |
| solution equilibrium | physical state in which there is a continuous interchange between dissolved and undissolved solute |
| unsaturated solution | contains less solute than it can hold at a certain temperature and pressure |
| supersaturated solution | solutions which under special conditions can be forced to hold more solute than is present in their saturated solutions |
| dilute solution | one where the amount of solute dissolved is relatively small in relation to the amount of solvent |
| concentrated solution | one where the amount of solute dissolved is relatively large in relation to the amount of solvent |
| molarity | the number of moles of solute dissolved in one liter of solution |
| 1 molar solution (1M) | has one mole of the solute dissolved in one liter of solvent |
| molality | number of moles dissolved in one kilogram of solvent |
| electrolyte | an aqueous solution that conducts electricity |
| nonelectrolyte | an aqueous solution that does not conducts electricity |
| freezing point | temperature at which solid and liquid phases exist together without any net change in the amount of substance in either phase |
| freezing point depression | the lowering of a freezing point caused by dissolved substances |
| colligative property | property characteristic of a solvent that depends on the concentration of the solute |
| boiling point elevation | the raising of a boiling point caused by dissolved substances |
