Term
|
Definition
| The temperature difference between a solution's boiling point and a pure solvent's boiling point |
|
|
Term
|
Definition
| The jerky, random, rapid movements of colloid particles that results from collisions of particles of the dispersion medium with the dispersed particles |
|
|
Term
|
Definition
| a Physical property of a solution that depends on the number, but not the identity, of the dissolved solute particles; Example properties include vapor pressure lowering, osmotic pressure, and freezing point depression |
|
|
Term
|
Definition
| heterogeneous mixtures containing particles larger than solution particles but smaller than suspension particles that are categorized according to the phases of their dispersed particles and dispersing mediums |
|
|
Term
|
Definition
| a quantitative measure of the amount of solute in a given amount of solvent or solution |
|
|
Term
| Freezing Point depression |
|
Definition
| The difference in temperature between a solution's freezing point and the freezing point of its pure solvent |
|
|
Term
|
Definition
| the overall enery change that occurs during the solution formation process |
|
|
Term
|
Definition
| States that at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid |
|
|
Term
|
Definition
|
|
Term
|
Definition
| two or more substances that are not soluble in each other |
|
|
Term
|
Definition
| two or more substances that are soluble in each other |
|
|
Term
|
Definition
| the ratio of the number of moles of solute dissolved in one kilogram of solvent; also known as molal concentration |
|
|
Term
|
Definition
| the number of moles of solute dissolved per liter of solution; also known as molar concentration |
|
|
Term
|
Definition
| the ratio of the number of moles of solute in solution to the total number of moles of solute and solvation |
|
|
Term
|
Definition
| the diffusion of solvent particles across a semi-permeable membrane from an area of higher solvent concentration to an area of lower solvent concentration |
|
|
Term
|
Definition
| the additional pressure needed to reverse osmosis |
|
|
Term
|
Definition
| Contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure |
|
|
Term
|
Definition
| the maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure |
|
|
Term
|
Definition
| able to be dissolved; a solute must be soluble |
|
|
Term
|
Definition
| the substance being dissolved |
|
|
Term
|
Definition
|
|
Term
|
Definition
| The process of surrounding solute particles with solvent particles to form a solution. Can only occur where and when the solute and solvent particles come in contact with each other. |
|
|
Term
|
Definition
| the substance that dissolves the solute |
|
|
Term
|
Definition
| contains more dissolved solute than a saturated solution at the same temperature |
|
|
Term
|
Definition
| A type of heterogeneous mixture whose particles settle out over time and can be separated from the mixture by filtration |
|
|
Term
|
Definition
| The scattering of light by colloidal particles |
|
|
Term
|
Definition
| Contains less dissolved solute for a given temperature and pressure than a saturated solution; has a further capacity to hold more solute |
|
|
Term
|
Definition
| the lowering of vapor pressure of a solvent by the addition of a nonvolatile solute to the solvent |
|
|
Term
| Freezing Point depression |
|
Definition
| The difference in temperature between a solution's freezing point and the freezing point of its pure solvent |
|
|
