Chemistry Ch 16

Front 1

Saturated Solution

Back 1

A solution containing the maximum amount of solute for a given amount of solvent ata constant temperature and pressure; an equilibrium exists between undissolved solute and ions in solution.

Front 2

Solubility

Back 2

The amount of a substance that dissolves in a given quanity of solvent at specified conditions of temperature and pressure to produce a saturated solution.

Front 3

Unsaturated Solution

Back 3

A solution that contains less solute than a saturated solution at a given temperature and pressure.

Front 4

Miscible

Back 4

Describes liquids that dissolve in one another in all proportions.

Front 5

Immiscible

Back 5

Describes liquids that are insoluble in one another; oil and water are immiscible.

Front 6

Supersaturated Solution

Back 6

A solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure; an equilibrium exists between undissolved solute and ions in solution.

Front 7

Henry's Law

Back 7

At a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

Front 8

What factors determine the rate at which a substance dissolves?

Back 8

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.

Front 9

How is solubility usually expressed?

Back 9

Solubility is often expressed in grams of solute per 100 g of solvent.

Front 10

What conditions determine the amount of solute that will dissolve in a given solvent?

Back 10

Temperature affects the solubility of solid, liquid, and gaseous solutes in a solvent; both temperature and pressure affect the solubility of gaseous solutes.

Front 11

Concentration

Back 11

A soultion is a measure of the amount of solute that is dissolved in a given quantity of solvent.

Front 12

Dilute Solution

Back 12

One that contains a small amount of solute.

Front 13

Concentrated Solution

Back 13

Contains a large amount of solute.

Front 14

Molarity (M)

Back 14

The number of moles of solute dissolved in one liter of solution.

Front 15

How do you calculate the molarity of a solution?

Back 15

To calculate the molarity of a solution, divide the moles of solute by the volume of the solution.

Front 16

What effect does dilution have on the total moles of solute in solution?

Back 16

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.

Front 17

What are two ways to express the percent composition of a solution?

Back 17

The concentration of a solution in percent canbe expressed in two ways: as the ratio of the colume 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.

Front 18

Colligative Property

Back 18

A property of a solution that depends only upon the number of solute particles, and not upon their identites; boiling-point elevation, freezing-point depression, and vapor-pressure lowering are colligative properties.

Front 19

Freezing-point depression

Back 19

The difference in temperature between the freezing point of a solution and the freezing point of the pure solvent.

Front 20

Boiling-point elevation

Back 20

The difference in temperature between boiling point of a solution and the boiling point of the pure solvent.

Front 21

What are three colligative properties of solutions?

Back 21

Three important colligative properties of solutions are vapor-pressure lowering, boiling-point elevation, and freezing-point depression.

Front 22

What factor determines the amount by which a solution's vapor pressure, freezing point, and boiling-point elevation differ from those properties of the solvent?

Back 22

The decrease in a solution's vapor pressure is proportional to the number of particles the solute makes in soultion. 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 boiling-point elevation is proportional to the number of solute particles dissolved in the solvent.

Front 23

Molality (m)

Back 23

The number of moles of solute dissolved in 1 kilogram (1000 g) of solvent.

Front 24

Mole Fraction

Back 24

The ratio of the moles of solute in solution to the total number of moles of both solvent and solute.

Front 25

Molal freezing-point depression constant (Kf)

Back 25

The change in freezing point for a 1-molal solution of a nonvolatile molecular solute.

Front 26

Molal boiling-point elevation constant (Kb)

Back 26

The change in boiling point for a 1-molal solution of a nonvolatile molecular solute.

Front 27

What are two ways of expressing the concentration of a solution?

Back 27

The unit molality and mole fractions are two additional ways in which chemists express the concentration of a solution.

Front 28

How are freezing-point depression and boiling-point elevation related to molality?

Back 28

The magnitudes of the freezing-point depression (^Tf) and the boiling-point elevation (^Tb) of a solution are directly proportional to the centration (m), when the solute is molecular, not ionic.