Chapter 11: Solutions

Question 1

solution

Answer 1

a homogeneous mixture involving two or more substances

Question 2

solute

Answer 2

the substance that is dissolved in a solution

Question 3

solvent

Answer 3

the liquid in which the solute dissolves (the major component of the solution)

Question 4

dilute

Answer 4

low amounts of solute per amount of solution

Question 5

concentrated

Answer 5

high amounts of solute per amount of solution

Question 6

concentration

Answer 6

the amount of solute that is present in a solution

Question 7

saturated solution

Answer 7

a solution contains the maximum amount of dissolved solute in a specific amount of solvent

Question 8

unsaturated solution

Answer 8

a solution that contains less than the maximum amount of dissolved solute in a specific amount of solvent

Question 9

supersaturated solution

Answer 9

an unstable condition in which there is more solute present in solution than its solubility would indicate

Question 10

solubility

Answer 10

a measure of the maximum amount of a solute that dissolves in a specific amount of solvent at a given temperature

Question 11

miscible liquids

Answer 11

liquids that mix completely to form a solution

Question 12

immiscible liquids

Answer 12

liquids that do not mix and form separate layers, neither liquids dissolve into the other

Question 13

“like dissolves like”

Answer 13

nonpolar (or weakly polar) substances are generally soluble in nonpolar solvents & ionic and polar compounds are generally soluble in polar solvents

Question 14

mass percent

Answer 14

the ratio of the mass of solute that is present in a solution relative to the mass of the solution as a whole; mass of solute / mass of solution * 100%

Question 15

volume percent (v/v)

Answer 15

the ratio of the volume of solute that is present in a solution relative to the volume of the solution as a whole; volume of solute / volume of solution * 100%

Question 16

parts per million (ppm)

Answer 16

how many parts a certain molecule or compound makes up within the one million parts of the whole solution; 1 ppm = 1g of solute per 1,000,000 grams of solution or 1 mg/L of solution

Question 17

parts per million (ppm) formula

Answer 17

mass of solute / mass of solution x 10^6

Question 18

parts per billion (ppb)

Answer 18

how many parts a certain molecule or compound makes up within the one billion parts of the whole solution; 1 ppb = 1g of solute per 1,000,000,000 grams of solution or 1 Mg/L of solution

Question 19

parts per billion (ppb) formula

Answer 19

mass of solute / mass of solution x 10^9

Question 20

molarity (M)

Answer 20

a measure of concentration defined as moles of solute per liter of solution; M = moles of solute (or n) / volume (L)

Question 21

chemists prepare dilute solutions by

Answer 21

mixing the concentrated solution with additional solvent; doing this increases the volume of the solution, but the moles of the solute do not change

Question 22

the moles of a solute are equal to

Answer 22

molarity x volume

Question 23

the concentration of a solute uses

Answer 23

square brackets []

Question 24

electrolyte solution

Answer 24

an aqueous solution containing dissolved ions

Question 25

electrolyte concentration

Answer 25

the amount of dissolved ions in a solution, typically expressed in terms of molarity (moles per liter)

Question 26

colligative properties

Answer 26

properties of a solution that do not depend on the type of particles that are dissolved, but rather on the number of dissolved particles in the solution

Question 27

three common and important colligative properties

Answer 27

freezing point depression, boiling point elevation, and osmotic pressure

Question 28

freezing point depression

Answer 28

the presence of solute in an aqueous solution lowers the freezing point below that of pure water (e.g. salt trucks in winter)

Question 29

in freezing point depression, the more dissolved particles

Answer 29

the lower the freezing temperature

Question 30

boiling point elevation

Answer 30

the pressure of solute in an aqueous solution raises the boiling point above that of pure water

Question 31

the boiling point elevation depends on

Answer 31

the number of solute particles present

Question 32

osmotic pressure

Answer 32

the tendency of water to move toward regions of greater concentration

Question 32

hypotonic solution

Answer 32

low osmotic pressure solution in which water migrates into the cells, causing them to swell and possibly burst

Question 32

hypertonic solution

Answer 32

high osmotic pressure solution in which water flows out of the cells, causing them to shrivel

Question 33

isotonic solution

Answer 33

ideal solution where the concentration is the same both in and outside of the cell

Question 33

gravimetric analysis

Answer 33

a technique that uses the mass of a precipitate to determine the concentration of a reactant

Question 33

steps of gravimetric analysis

Answer 33

1. measure the volume of the unknown 2. precipitate the ion 3. filter and dry the precipitate 4. measure the mass of the precipitate

Question 34

metal displacement reaction

Answer 34

a reaction between two metals in which one metal is oxidized to its ionic form while the other metal ion is reduced to its elemental form (single displacement reaction)