202-NYB-05: Course Notes Problems
Chapter 11: Properties of Solutions. (Zumdahl/Zumdahl, 10th Ed)
Problem 1: Fluoride ions are used in toothpaste in order to help prevent cavities.
Sodium fluoride (NaF) is a commonly used source of fluoride ions in toothpaste.
Determine the amount of NaF in a tube of 130.0 g of toothpaste. The mass
percent of NaF is 0.243%.
Problem 2: Determine the amount of alcohol (ethanol, C2H6O) in one glass of
beer (5.00% v/v) and in one glass of pina colada (60.0 mL of Rum, 40.0% v/v).
One glass is equal to 250.0 mL.
Problem 3: A solution is prepared by mixing 1.00 g of ethanol (C2H6O) with
100.0 g of water to give a final volume of 101 mL. Calculate the molarity, mass
percent, mole fraction, and molality of ethanol in this solution.
Problem 4: A 3.75 M sulphuric acid (H2SO4) solution has a density of 1.230
g/mL. Calculate the mass percent and the molality of the sulphuric acid solution.
Problem 5: A certain soft drink is bottled so that a bottle at 25°C contains CO2
gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure
of CO2 in the atmosphere is 4.0 x 10-4 atm, calculate the equilibrium
concentrations of CO2 in the soda both before and after the bottle is opened.
The Henry’s Law constant for CO2 in aqueous solution is 3.1 x 10-2 mol/L.atm at
25°C.
Problem 6: Calculate the expected vapor pressure at 25°C for a solution
prepared by dissolving 158.0 g of sucrose (molar mass = 342.3 g/mol) in 643.5
mL of water. At 25°C, the density of water is 0.9971 g/mL and the vapor
pressure is 23.76 torr.
Chapter 11: Properties of Solutions. (Zumdahl/Zumdahl, 10th Ed)
Problem 1: Fluoride ions are used in toothpaste in order to help prevent cavities.
Sodium fluoride (NaF) is a commonly used source of fluoride ions in toothpaste.
Determine the amount of NaF in a tube of 130.0 g of toothpaste. The mass
percent of NaF is 0.243%.
Problem 2: Determine the amount of alcohol (ethanol, C2H6O) in one glass of
beer (5.00% v/v) and in one glass of pina colada (60.0 mL of Rum, 40.0% v/v).
One glass is equal to 250.0 mL.
Problem 3: A solution is prepared by mixing 1.00 g of ethanol (C2H6O) with
100.0 g of water to give a final volume of 101 mL. Calculate the molarity, mass
percent, mole fraction, and molality of ethanol in this solution.
Problem 4: A 3.75 M sulphuric acid (H2SO4) solution has a density of 1.230
g/mL. Calculate the mass percent and the molality of the sulphuric acid solution.
Problem 5: A certain soft drink is bottled so that a bottle at 25°C contains CO2
gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure
of CO2 in the atmosphere is 4.0 x 10-4 atm, calculate the equilibrium
concentrations of CO2 in the soda both before and after the bottle is opened.
The Henry’s Law constant for CO2 in aqueous solution is 3.1 x 10-2 mol/L.atm at
25°C.
Problem 6: Calculate the expected vapor pressure at 25°C for a solution
prepared by dissolving 158.0 g of sucrose (molar mass = 342.3 g/mol) in 643.5
mL of water. At 25°C, the density of water is 0.9971 g/mL and the vapor
pressure is 23.76 torr.
