1. Chapter 16 Review
=“Solutions”

2. Chapter 16 Review
If the solubility of a particular solute is 10 g/100 g H2O at 20 oC, which of the following would represent a supersaturated solution of that solute: a) 9 g/100 g H2O at 20 oC, or b) 11 g/100 g H2O at 20 oC.
If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.

3. Chapter 16 Review Colligative properties depend upon the ____.
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) CO2(g), or b) KBr(s)?

4. Chapter 16 Review
The solubility of a gas in a liquid is ____ proportional to ____.
To what concentration variable is change in boiling point directly proportional?
What usually occurs to solubility as temperature increases?
What units are generally used to express solubility?

5. Chapter 16 Review
What factors will usually make a substance dissolve faster in a solvent?
In a concentrated solution, there is a ____ amount of solute.
What are the three colligative properties of a solution we have studied?

6. 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 oC? (the solubility of KCl is 34 g/100 g H2O at 20 oC)
What does NOT change when a solution is diluted by the addition of more solvent?

7. 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

8. 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 ____.

9. Chapter 16 Review
What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb = oC/m; molar mass of water = 18 g/mol)
What mass of KCl (solubility 34 g/100 g H2O at 20 oC) can dissolve in 3.30 x 102 g of water?

10. Chapter 16 Review
What is the freezing point of a solution that has 5.0 mol of NaI in 1250 g of water? (Kf = 1.86 oC/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?

11. 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 molarity of a solution containing 1.2 g of solute in 450 mL of solution? (molar mass of solute = 24 g/mol)
How many liters of a 0.30 M solution are needed to give 2.7 mol of solute?

12. 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 mL, what is the solute’s percent by volume?

13. What is the number of moles of solute in 650 mL of a 0.40 M solution?
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?

14. 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?

15. Chapter 16 Review
Calculate the molality of a solution prepared by dissolving 175 g KNO3 in 750 g of water.
End of Chapter 16 Review