Question 1

What is the molality of a solution that is 3.68 % by mass calcium chloride.

Accepted Answer

A) 0.0332 m 
B) 0.332 m 
C) 0.344 m 
D) 0.464 m 
E) 0.506 m 
A) 0.0332 m 
B) 0.332 m 
C) 0.344 m 
D) 0.464 m 
E) 0.506 m

Question 2

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

Accepted Answer

Question 3

The solubility of gases in water always decreases with increasing temperature.

Accepted Answer

A) True 
 B)False

Question 4

In which of the following solvents would you expect KBr to be most soluble?

Accepted Answer

A) C6H14 (hexane) 
B) CH3CH2OH (ethanol) 
C) C6H6 (benzene) 
D) CCl4 (carbon tetrachloride) 
E) C6H12 (cyclohexane) 
A) C6H14 (hexane) 
B) CH3CH2OH (ethanol) 
C) C6H6 (benzene) 
D) CCl4 (carbon tetrachloride) 
E) C6H12 (cyclohexane)

Question 5

When 12.1 g of the sugar sucrose (a nonelectrolyte)is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082°C.What is the molar mass of sucrose? Kf of water is 1.86°C/m.

Accepted Answer

A) 426 g 
B) 99.2 g 
C) 178 g 
D) 266 g 
E) 343 g 
A) 426 g 
B) 99.2 g 
C) 178 g 
D) 266 g 
E) 343 g

Question 6

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

Accepted Answer

The answer of A 100.-mL sample of water is taken...

Question 7

How many liters of ethylene glycol antifreeze (C2H6O2)would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8°C? (The density of ethylene glycol is 1.1 g/mL.For water, Kf = 1.86°C/m.)

Accepted Answer

Question 8

How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Accepted Answer

Question 9

Consider a solution made from a nonvolatile solute and a volatile solvent.Which statement is true?

Accepted Answer

A) The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent. 
B) The boiling point of the solution is always greater than the boiling point of the pure solvent. 
C) The freezing point of the solution is always greater than the freezing point of the pure solvent. 
A) The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent. 
B) The boiling point of the solution is always greater than the boiling point of the pure solvent. 
C) The freezing point of the solution is always greater than the freezing point of the pure solvent.

Question 10

A solution made of pentane and hexane has a mole fraction, X = 0.250 of pentane.Which substance is the solvent?

Accepted Answer

The answer of A solution made of pentane and hexane...

Question 11

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.50m K2CO3 at this temperature (assume 100% dissociation)

Accepted Answer

A) 1.89 mmHg 
B) 5.39 mmHg 
C) 66.5 mmHg 
D) 70.0 mmHg 
E) 108 mmHg 
A) 1.89 mmHg 
B) 5.39 mmHg 
C) 66.5 mmHg 
D) 70.0 mmHg 
E) 108 mmHg

Question 12

What is the percent CdSO4 by mass in a 1.00 m aqueous CdSO4 solution?

Accepted Answer

A) 1.00 × 10-3 % 
B) 0.100 % 
C) 17.2 % 
D) 20.8 % 
E) 24.4 % 
A) 1.00 × 10-3 % 
B) 0.100 % 
C) 17.2 % 
D) 20.8 % 
E) 24.4 %

Question 13

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

Accepted Answer

A) 0.03097 M 
B) 0.4133 M 
C) 0.4646 M 
D) 1.590 M 
E) 3.097 M 
A) 0.03097 M 
B) 0.4133 M 
C) 0.4646 M 
D) 1.590 M 
E) 3.097 M

Question 14

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Question 15

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O2(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 × 10-3 mol/L·atm.

Accepted Answer

A) 2.7 × 10-4 M 
B) 1.3 × 10-3 M 
C) 6.2 × 10-3 M 
D) 9.6 × 10-3 M 
E) 0.96 M 
A) 2.7 × 10-4 M 
B) 1.3 × 10-3 M 
C) 6.2 × 10-3 M 
D) 9.6 × 10-3 M 
E) 0.96 M

Question 16

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

Accepted Answer

Percent mass, mole f

Question 17

Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water.

Accepted Answer

A) 2.9% 
B) 6.9% 
C) 7.4% 
D) 22% 
E) 29% 
A) 2.9% 
B) 6.9% 
C) 7.4% 
D) 22% 
E) 29%

Question 18

A solution is 35.0% by mass carbon tetrachloride (CCl4)in benzene (C6H6)at 20°C.The vapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 74.61 mmHg and 91.32 mmHg, respectively.Calculate the vapor pressure of the solution at 20°C:

Accepted Answer

A) 58.1 mmHg 
B) 78.2 mmHg 
C) 80.5 mmHg 
D) 82.9 mmHg 
E) 83.0 mmHg 
A) 58.1 mmHg 
B) 78.2 mmHg 
C) 80.5 mmHg 
D) 82.9 mmHg 
E) 83.0 mmHg

Question 19

Using your knowledge of osmosis or osmotic pressure explain the following statement: Drinking salt water actually dehydrates our tissues.

Accepted Answer

The water passes fro

Question 20

Assuming 100% dissociation, which of the following compounds is listed correctly with its van't Hoff factor i?

Accepted Answer

A) Ca(ClO3)2, i = 2 
B) (NH4)2SO4, i = 3 
C) (NH4)3PO4, i = 5 
D) Urea, i = 2 
E) Sc2(SO4)3, i = 6 
A) Ca(ClO3)2, i = 2 
B) (NH4)2SO4, i = 3 
C) (NH4)3PO4, i = 5 
D) Urea, i = 2 
E) Sc2(SO4)3, i = 6

Exam 12: Physical Properties of Solutions

What is the molality of a solution that is 3.68 % by mass calcium chloride.

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

The solubility of gases in water always decreases with increasing temperature.

In which of the following solvents would you expect KBr to be most soluble?

When 12.1 g of the sugar sucrose (a nonelectrolyte)is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082°C.What is the molar mass of sucrose? Kf of water is 1.86°C/m.

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

How many liters of ethylene glycol antifreeze (C2H6O2)would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8°C? (The density of ethylene glycol is 1.1 g/mL.For water, Kf = 1.86°C/m.)

How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Consider a solution made from a nonvolatile solute and a volatile solvent.Which statement is true?

A solution made of pentane and hexane has a mole fraction, X = 0.250 of pentane.Which substance is the solvent?

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.50m K2CO3 at this temperature (assume 100% dissociation)

What is the percent CdSO4 by mass in a 1.00 m aqueous CdSO4 solution?

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O2(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 × 10-3 mol/L·atm.

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality.

Calculate the mass percent of HOCH2CH2OH in a solution made by dissolving 3.2 g of HOCH2CH2OH in 43.5g of water.

A solution is 35.0% by mass carbon tetrachloride (CCl4)in benzene (C6H6)at 20°C.The vapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 74.61 mmHg and 91.32 mmHg, respectively.Calculate the vapor pressure of the solution at 20°C:

Using your knowledge of osmosis or osmotic pressure explain the following statement: Drinking salt water actually dehydrates our tissues.

Assuming 100% dissociation, which of the following compounds is listed correctly with its van't Hoff factor i?

Chemistry: the Study of Change

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

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Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

When 12.1 g of the sugar sucrose (a nonelectrolyte)is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082°C.What is the molar mass of sucrose? K_f of water is 1.86°C/m.

How many liters of ethylene glycol antifreeze (C₂H₆O₂)would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8°C? (The density of ethylene glycol is 1.1 g/mL.For water, K_f = 1.86°C/m.)

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.50m K₂CO₃ at this temperature (assume 100% dissociation)

What is the percent CdSO₄ by mass in a 1.00 m aqueous CdSO₄solution?

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O₂(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 × 10^-3 mol/L·atm.

Calculate the mass percent of HOCH₂CH₂OH in a solution made by dissolving 3.2 g of HOCH₂CH₂OH in 43.5g of water.

A solution is 35.0% by mass carbon tetrachloride (CCl₄)in benzene (C₆H₆)at 20°C.The vapor pressure of pure benzene and pure carbon tetrachloride at this temperature is 74.61 mmHg and 91.32 mmHg, respectively.Calculate the vapor pressure of the solution at 20°C: