Chapter 16 Review

=“Solutions”

Chapter 16 Review

 If the solubility of a particular solute is 10 g/100 g H

2

O at 20

o

C, which of the following would represent a

supersaturated

solution of that solute: a) 9 g/100 g H

2

O at 20

o

C, or b) 11 g/100 g H

2

O at 20

o

C.

 If a crystal added to an aqueous solution causes many particles to come

out of the solution

, the original solution was ____.

Chapter 16 Review



Colligative

the ____.

properties depend upon  What happens to the

solubility

of a gas in a liquid, if the partial pressure of the gas above the liquid

decreases

?

 Which of the following substances is

less soluble

in hot water than in cold water: a) CO

2(g)

, or b) KBr

(s)

?

Chapter 16 Review

 The

solubility

of a gas in a liquid is ____ proportional to ____.

 To what

concentration variable

change in boiling point directly proportional?

is  What usually occurs to solubility as temperature

increases

?

 What

units

are generally used to express solubility?

Chapter 16 Review

 What factors will usually make a substance solvent?

dissolve faster

in a  In a

concentrated

solution, there is a ____ amount of solute.

 What are the three

colligative properties

studied?

of a solution we have

Chapter 16 Review

 What are the solution concentration units used to express

molarity

?

 What is the maximum amount of KCl that

can dissolve

in 200 g of water at 20

o

C? (the solubility of KCl is 34 g/100 g H

2

O at 20

o

C)  What does NOT change when a solution is

diluted

by the addition of more solvent?

Chapter 16 Review

 If the percent by volume is 2.0 % and the volume of solution is 250 mL, what is the

volume of solute

in solution?

 What

two factors

affect the solubility of a particular substance?

 Which of the following equations yields the number of

moles?

a) M x L, or b) M x mass of solution

Chapter 16 Review

 The

volume of alcohol

present in 620 mL of a 40.0 % (v/v) solution of alcohol is ____.

 A solute

depresses

the freezing point because the solute ____.

 To

increase the solubility

of gas at constant temperature from 1.20 g/L at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.

Chapter 16 Review

 What is the

boiling point

of a solution that contains 3 moles of KBr in 2000 g of water? (K

b

= 0.512

o

C/m; molar mass of water = 18 g/mol)  What mass of KCl (solubility 34 g/100 g H

2

O at 20

o

C)

can dissolve

in 3.30 x 10

2

g of water?

Chapter 16 Review

 What is the

freezing point

of a solution that has 5.0 mol of NaI in 1250 g of water? (K

f

= 1.86

o

C/m; molar mass of water = 18.0 g/mol)  How many

kilograms

of solvent are in a sample of 0.30 molal solution, if the sample contains 13 moles of solute?

Chapter 16 Review

 What is the

molality

of a solution containing 5.0 mol of solute in 3.2 kg of solvent?

 What is the 24 g/mol)

molarity

of a solution containing 1.2 g of solute in 450 mL of solution? (molar mass of solute =  How many

liters

of a 0.30 M solution are needed to give 2.7 mol of solute?

Chapter 16 Review

 How many

liters

of a 1.5 M solution are required to yield 5.0 g of solute? (molar mass of solute = 30.0 g/mol)  If the volume of solute is 6.0 mL and the volume of solution is 300.0 mL, what is the solute’s

percent

by volume?

Chapter 16 Review

 If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the

solubility

of the gas when the pressure is 202 kPa?

 What is the number of

moles

of solute in 650 mL of a 0.40 M solution?

Chapter 16 Review

 What is the number of

moles

of solute in a 0.3 molal solution containing 0.10 kg of solvent?

 If 1.0 mL of 6.0 M HCl is added to 499 mL of water to give exactly a 500 mL solution, what is the

molarity

of the dilute solution?

Chapter 16 Review

 Calculate the

molality

of a solution prepared by dissolving 175 g KNO

3

in 750 g of water.