Term
| What factors determine the rate at which a substance dissolves? |
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Definition
| the compositions of the solvent and the solute determine whether a substance will dissolve. Stirring(agitation), temperature, and the surface area of the dissolving particles determine how fast the substance will dissolve. |
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Term
| How is solubility usually expressed? |
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Definition
| solubility is often expressed in grams of solute per 100g of solvent. |
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Term
| What conditions determine the amount of solute that will dissolve in a given substance? |
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Definition
| temperature affects the solubility of solid, liquid, and gaseous solutes in a solvent; both termperature and pressure affect the solubility of gaseous solutes. |
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Term
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Definition
| contains the maximum amount of solute for a given quantity of solvent at a constant temperature and pressure. |
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Term
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Definition
| the amount of solute that dissolves in a given quantity of a solvent at a specified temperature and pressure to produce a saturated solution. |
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Term
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Definition
| a solution that contains less solute than a saturated solution at a given temperature and pressure. |
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Term
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Definition
| pairs of liquids that disolve in each other in all proportions. |
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Term
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Definition
| liquids that are insoluble in one another. |
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Term
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Definition
| contains more solute than it can theoretically hold at a given temperature. |
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Term
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Definition
| states that at a given temperature, the solubility(S) of a gas in a liquid is directly proportional to the pressure(P) of the gas above the liquid. |
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Term
| How do you calculate the molarity of a solution? |
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Definition
| to calculate the molarity of a solution, divide the moles of solute by the volume of the solution. |
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Term
| What effect does the dilution have on the total moles of solute in solution? |
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Definition
| diluting a solution reduces the number of moles of solute per unit volume, but the total number of moles of solute in solution does not change. |
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Term
| What are two ways to express the percent concentration of a solution? |
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Definition
| the concentration of a solution in percent can be expressed in two ways: as the ratio of the volume of the solute to the volume of the solution or as the ratio of the mass of the solute to the mass of the solution. |
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Term
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Definition
| is a measure of the amount of solute that is dissolved in a given quantity of solvent. |
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Term
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Definition
| one that contains a small amount of solute. |
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Term
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Definition
| contains a large amount of solute. |
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Term
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Definition
| the number of moles of solute dissolved in one liter of solution. |
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Term
| What are three colligative properties of solution? |
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Definition
| three important colligative properties of solution are vapor-pressure lowering, boiling-point elevation, and freezing-point depression. |
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Term
| What factor determines the amount by which a solution's vapor pressure, freezing point, and boiling point differ from those properties of the solvent? |
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Definition
| The decrease in a solution's vapor pressure is proportional to the number of particles the solute makes in solution. the magnitude of the freezing-point depression is proportional to the number of solute particles dissolved in the solvent and does not depend upon their identity. the magnitude of the boiling-poit elevation is proportional to the number of solute particles dissolved in the solvent. |
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Term
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Definition
| a property that depends only upon the number of solute particles, and not upon their identity. |
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Term
| Freezing-point depression |
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Definition
| the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent. |
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Term
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Definition
| the difference in temperature between the boiling point of a solution and the noiling point of the pure solvent. |
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Term
| What are two ways of expressing the concentration of a solution? |
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Definition
| the unit molality and mole fractions are two additional ways in which chemists express the concentration of a solution. |
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Term
| How are freezing-point depression and boiling-point elevation related to molality? |
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Definition
| the magnitudes of the freezing-point depression(delta Tf) and the boiling-point elevation(delta Tb) of a solution are directly proportional to the molal concentration(m), when the solute is molecular, not ionic. |
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Term
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Definition
| the number of moles of solute dissolved in 1 kilogram (1000g) of solvent. |
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Term
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Definition
| the ratio of the moles of that solute to the total number of moles of solvent to solute. |
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Term
| Molal freezing-point depression constant (Kf) |
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Definition
| it is equal to the change in freezing point for a 1-molal solution of a nonvolatile molecular solute. |
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Term
| Molal boiling-point elevation constant (Kb) |
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Definition
| it is equal to the change in boiling point for a 1-molal solution of a nonvolatile molecular solute. |
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