| A | B |
|---|
| Soultion | A homogeneous mixture of two or more substances. A solution is composed of one or more solutes dissolved in a solvent. The particles of a solution are atomic, ionic, or molecular size. These particles are dispersed evenly (dissolved) throughout the medium. A minimum of two substances are needed to make a solution (a solvent and a solute). |
| Solvent | The medium in which the other substances are mixed or dissolved. The solvent is the component present in the largest quantity. It can be liquid, a solid, or a gas; but , ususally, it's a liquid. Water is the most common solvent and is considered the universal solvent of life |
| Solute | The substance that is dissolved by a solvent. The solute can be a gas as in club soda (CO2 in water), or a liquid as in antifreeze (ethylene glycol in water). The solute is the component present in the lesser quantity. The solute particles are less than 1 nm in size in a solution. |
| Solubility | The amount of a substance that will dissolve in a given volume of solvent at a specified temperature |
| Solvation | How fast solutes(s) will dissolve in solvent |
| Percent Concentration | Refers to a number of parts of solute in 100 parts of solution. It is used to express concentration in terms of weight per unit weight, weight per volume, and volume per unit volume. It is very simple simple of concentration expression |
| Saturated Solution | A solution in which it is not possible to dissolve more of the solute at a given temperature. If more solute is added, it will just stay separate and not be dissolved. |
| Unsaturated Solution | A solution in which more solute can be dissolved without having to change the temperature. The ratio of solute to solvent is lower in an unsaturated solution than a saturated solution |
| Supersaturated Solution | One that contains more dissolved solute than a saturated solution. The excess solute will precipitate upon cooling. Certain conditions such as temeprature of the solvent, atmospheric, pressure, and nature of solute and solvent affect the amount of solute that can be dissolved in a solvent. Solvents usually dissolve more solute at higher temperatures. |
| Colloidal Dispersion | A mixture consisting of solute particles evenly distributed throughout a solvent. The distribution is not completely homogenous. |
| Suspension | A suspension is a heterogeneous mixture that contains particles much larger than that of a coloidal dispersion. These particles may settle, forming a second phase. |
| Concentration | The amount of solute dissolved in a given amount of solution |
| Percent Concentration (weight per volume) | The amount of mass (grams or milligrams) in the amount of solution in volume (deciliters). The unit of report for this expression is typically g/dL or mg/dL |
| Molarity | Is defined as the number of moles of solute per liter of solution. The unit of report for this expression is mol/L, or mmol/L. Is often symbolized by the symbol M |
| Normality | Is equal to the number of Equivalents of solute per number of Liters of solutions. The unit of report for this expression is (Eg/L, mEq/L) |
| Vapor Pressure Lowering | Results from the escape of solvent particles from the liquid to the gaseous state. The presence of solute particles hinders the escape of solvent moleculesRaoult's Law states that when solute is added to sovlent, the vapor pressure of the solvent decreases. |
| Boiling point elevation | When solute is added to solvent, the boiling point of a solution is found to increase (higher temperature to form a gas) |
| Freezing point depression | When solute is added to solvent, the freezing point of the resulting soltuion decreases (lower temperature to convert liquid to a solid) |
| Osmotic Pressure | The movement of solvent from a dilute solution to a more concentrated solution through a semipermeable membrane. The amount of pressure applied by the more concentrated solution to stop the flow is the osmotic pressure. When concentrations of solutinos on both sides of a membrane are equal, the difference in osmotic pressure becomes zero, and movement of solvent ceases |
| Hypertonic Solution | If the solute concentration of the fluid surrounding red blood cells is higher than that insde the cell. Solvent flows from the cell causing it to collapse |
| Hypotonic Solution | If the solute concentration of the fluid surrounding red blood cells is, lower than that inside the cell. Water fows into the cell causing them to rupture |
| Isotonic Solution | To precent either of these effects the solute concentrations should be the same in both aqueous solutions. The cell size will remain unchanged, and solvent movement in and out of the cell will be equal. |
| Factors affecting solubility of a solution | Difference in polarity of solute and solvent Temperature |
| Factors affecting rate of solvation | Surface area- An increase in the surface area will increase the rate of solvation Agitation will increase the rate of solvation Solution concentration- Refers to the the mass or volume of the solute present in a specific amount of the solvent or solution Pressure- In a liquid solvent it has little effect on the solubility of solids and liquids, but will affect solubility of a gas in liquid; The mass of a gas dissolved by a given amount of a liquid is directly proportional to the pressure exerted by the gas when in equilibrium with the solution. |
| Concentrated | (High solutes/solvent ratio) may cause a slow solvation rate. |
| Dilute | (Low solute/solvent ration) may have a faster rate of solvation |
| Henry's Law | The solubility of a gas is directly proportional to the partial pressure of the gas above the solution |
