Question 1

A solution of LiCl in water is 20.0 wt% LiCl. What is the mole fraction of LiCl? Assume the density of the solution is 1.00 g mL-1.

Accepted Answer

A)  0. 0960 
B)  0. 106 
C)  0. 472 
D)  4. 44 
A)  0. 0960 
B)  0. 106 
C)  0. 472 
D)  4. 44

Question 2

An aqueous solution has a normal boiling point of 10 3.0 °C. What is the freezing point of this solution? For water   and

Accepted Answer

A)  -0. 82 °C 
B)  -3.0 °C 
C)  -3.6 °C 
D)  -11 °C 
A)  -0. 82 °C 
B)  -3.0 °C 
C)  -3.6 °C 
D)  -11 °C

Question 3

Which of the following statements is TRUE?

Accepted Answer

A)  In general, the solubility of a solid in water decreases with increasing temperature. 
B)  In general, the solubility of a gas in water decreases with increasing temperature. 
C)  The solubility of a gas in water usually increases with decreasing pressure. 
D)  The solubility of an ionic solid in water decreases with increasing temperature. 
E)  None of the above statements is true. 
A)  In general, the solubility of a solid in water decreases with increasing temperature. 
B)  In general, the solubility of a gas in water decreases with increasing temperature. 
C)  The solubility of a gas in water usually increases with decreasing pressure. 
D)  The solubility of an ionic solid in water decreases with increasing temperature. 
E)  None of the above statements is true.

Question 4

Calculate the freezing point of a solution of 40.0 g salicylaldehyde, C7H6O2, dissolved in 800. g of benzene, C6H6.   and the freezing point is 5.50 °C for benzene.

Accepted Answer

A)  -2.09 °C 
B)  2.09 °C 
C)  3.41 °C 
D)  7.59 °C 
A)  -2.09 °C 
B)  2.09 °C 
C)  3.41 °C 
D)  7.59 °C

Question 5

A solution is prepared by dissolving 16.4 g of benzene (     ) in 282 g of carbon tetrachloride   The concentration of benzene in this solution is ________ molal. The molar masses of   and   are   and   respectively.

Accepted Answer

A)  0.704 
B)  5.50 
C)  0.0550 
D)  7.45 × 10-4 
E)  0.745 
A)  0.704 
B)  5.50 
C)  0.0550 
D)  7.45 × 10-4 
E)  0.745

Question 6

A solution is 0.0433 mol kg-1 LiF. What is the molarity of the solution if the density is 1.10 g mL-1?

Accepted Answer

A)  0.0441 mol L-1 
B)  0.0390 mol L-1 
C)  0.0519 mol L-1 
D)  0.0476 mol L-1 
E)  0.0417 mol L-1 
A)  0.0441 mol L-1 
B)  0.0390 mol L-1 
C)  0.0519 mol L-1 
D)  0.0476 mol L-1 
E)  0.0417 mol L-1

Question 7

How many moles of KF are contained in 347 g of water in a 0.175 mol kg-1 KF solution?

Accepted Answer

A)  1.65 × 10-2 mol KF 
B)  5.04 × 10-2 mol KF 
C)  6.07 × 10-2 mol KF 
D)  3.22 × 10-2 mol KF 
E)  1.98 × 10-2 mol KF 
A)  1.65 × 10-2 mol KF 
B)  5.04 × 10-2 mol KF 
C)  6.07 × 10-2 mol KF 
D)  3.22 × 10-2 mol KF 
E)  1.98 × 10-2 mol KF

Question 8

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl if the solution has a density of 1.20 g mL-1.

Accepted Answer

A)  39.0 mol kg-1 
B)  17.5 mol kg-1 
C)  6.39 mol kg-1 
D)  10.7 mol kg-1 
E)  9.44 mol kg-1 
A)  39.0 mol kg-1 
B)  17.5 mol kg-1 
C)  6.39 mol kg-1 
D)  10.7 mol kg-1 
E)  9.44 mol kg-1

Question 9

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

Accepted Answer

A)  0.360 bar 
B)  0.318 bar 
C)  0.0308 bar 
D)  0.0387 bar 
E)  0.00567 bar 
A)  0.360 bar 
B)  0.318 bar 
C)  0.0308 bar 
D)  0.0387 bar 
E)  0.00567 bar

Question 10

Define a colloid.

Accepted Answer

A colloid is a mixtu

Question 11

What is the expected van't Hoff factor for MgSO4? (Assume dilute conditions)

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 12

At a given temperature the vapour pressures of benzene and toluene are 183 mmHg and 59.2 mmHg, respectively. Calculate the total vapour pressure over a solution of benzene and toluene with Xbenzene = 0. 580.

Accepted Answer

A)  106 mmHg 
B)  121 mmHg 
C)  131 mmHg 
D)  242 mmHg 
A)  106 mmHg 
B)  121 mmHg 
C)  131 mmHg 
D)  242 mmHg

Question 13

Which of the following defines dynamic equilibrium of a solution?

Accepted Answer

A)  rate of dissolution = rate of deposition 
B)  rate of dissolution  rate of deposition 
D)  rate of bubbling > rate of dissolving 
E)  rate of evaporating > rate of condensing 
A)  rate of dissolution = rate of deposition 
B)  rate of dissolution  rate of deposition 
D)  rate of bubbling > rate of dissolving 
E)  rate of evaporating > rate of condensing

Question 14

A compound is found to have a molar mass of 190 g mol-1. If 0.0673 g of the compound is dissolved in enough water to make 200 mL of solution at 25 °C, what is the osmotic pressure of the resulting solution?

Accepted Answer

A)  1.21 × 10-2 bar 
B)  6.12 × 10-2 bar 
C)  4.39 × 10-2 bar 
D)  3.97 × 10-2 bar 
E)  2.28 × 10-2 bar 
A)  1.21 × 10-2 bar 
B)  6.12 × 10-2 bar 
C)  4.39 × 10-2 bar 
D)  3.97 × 10-2 bar 
E)  2.28 × 10-2 bar

Question 15

Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3 g of sucrose, C12H22O11, at a temperature of 25.0 °C. The vapour pressure of pure water at 25 °C is 31.7 mbar, the density of water is 1.00 g mL-1, and assume no change in volume occurs upon dissolution.

Accepted Answer

A)  204 mL 
B)  31.8 mL 
C)  286 mL 
D)  323 mL 
E)  516 mL 
A)  204 mL 
B)  31.8 mL 
C)  286 mL 
D)  323 mL 
E)  516 mL

Question 16

Identify the classification of milk.

Accepted Answer

A)  aerosol 
B)  solid aerosol 
C)  foam 
D)  emulsion 
E)  solid emulsion 
A)  aerosol 
B)  solid aerosol 
C)  foam 
D)  emulsion 
E)  solid emulsion

Question 17

A nonelectrolyte compound with a molar mass of 862 g mol-1 was dissolved in enough water to make 100 mL of solution at 25 °C and produced an osmotic pressure of 38.4 mbar. Calculate the mass of the compound, in mg, used to make this solution.

Accepted Answer

A)  116 mg 
B)  185 mg 
C)  134 mg 
D)  75.3 mg 
E)  84.3 mg 
A)  116 mg 
B)  185 mg 
C)  134 mg 
D)  75.3 mg 
E)  84.3 mg

Question 18

The Henry's law constant for helium gas in water at 30 °C is 3.70 ×   mol L-1 bar-1. When the partial pressure of helium above a sample of water is 0.450 bar, the concentration of helium in the water is ________ mol L-1.

Accepted Answer

A)  1.22 × 103 
B)  8.22 × 10-4 
C)  1.67 × 10-4 
D)  0.45 
E)  3.70 × 10-4 
A)  1.22 × 103 
B)  8.22 × 10-4 
C)  1.67 × 10-4 
D)  0.45 
E)  3.70 × 10-4

Question 19

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol-1 that is dissolved in enough water to create 20.0 mL of solution.

Accepted Answer

A)  288 K 
B)  293 K 
C)  278 K 
D)  314 K 
E)  299 K 
A)  288 K 
B)  293 K 
C)  278 K 
D)  314 K 
E)  299 K

Question 20

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Accepted Answer

A)  4.09 × 10-3 
B)  7.80 × 10-2 
C)  1.28 × 10-3 
D)  7.23 × 10-2 
E)  2.45 × 10-3 
A)  4.09 × 10-3 
B)  7.80 × 10-2 
C)  1.28 × 10-3 
D)  7.23 × 10-2 
E)  2.45 × 10-3

Exam 12: Solutions

A solution of LiCl in water is 20.0 wt% LiCl. What is the mole fraction of LiCl? Assume the density of the solution is 1.00 g mL-1.

An aqueous solution has a normal boiling point of 10 3.0 °C. What is the freezing point of this solution? For water and

Which of the following statements is TRUE?

Calculate the freezing point of a solution of 40.0 g salicylaldehyde, C7H6O2, dissolved in 800. g of benzene, C6H6. and the freezing point is 5.50 °C for benzene.

A solution is prepared by dissolving 16.4 g of benzene ( ) in 282 g of carbon tetrachloride The concentration of benzene in this solution is ________ molal. The molar masses of and are and respectively.

A solution is 0.0433 mol kg-1 LiF. What is the molarity of the solution if the density is 1.10 g mL-1?

How many moles of KF are contained in 347 g of water in a 0.175 mol kg-1 KF solution?

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl if the solution has a density of 1.20 g mL-1.

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

Define a colloid.

What is the expected van't Hoff factor for MgSO4? (Assume dilute conditions)

At a given temperature the vapour pressures of benzene and toluene are 183 mmHg and 59.2 mmHg, respectively. Calculate the total vapour pressure over a solution of benzene and toluene with Xbenzene = 0. 580.

Which of the following defines dynamic equilibrium of a solution?

A compound is found to have a molar mass of 190 g mol-1. If 0.0673 g of the compound is dissolved in enough water to make 200 mL of solution at 25 °C, what is the osmotic pressure of the resulting solution?

Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3 g of sucrose, C12H22O11, at a temperature of 25.0 °C. The vapour pressure of pure water at 25 °C is 31.7 mbar, the density of water is 1.00 g mL-1, and assume no change in volume occurs upon dissolution.

Identify the classification of milk.

A nonelectrolyte compound with a molar mass of 862 g mol-1 was dissolved in enough water to make 100 mL of solution at 25 °C and produced an osmotic pressure of 38.4 mbar. Calculate the mass of the compound, in mg, used to make this solution.

The Henry's law constant for helium gas in water at 30 °C is 3.70 × mol L-1 bar-1. When the partial pressure of helium above a sample of water is 0.450 bar, the concentration of helium in the water is ________ mol L-1.

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol-1 that is dissolved in enough water to create 20.0 mL of solution.

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

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Chemical Reactions and Stoichiometry

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The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

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Chemical Equilibrium

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Aqueous Ionic Equilibrium

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Filters

A solution of LiCl in water is 20.0 wt% LiCl. What is the mole fraction of LiCl? Assume the density of the solution is 1.00 g mL^-1.

Calculate the freezing point of a solution of 40.0 g salicylaldehyde, C₇H₆O₂, dissolved in 800. g of benzene, C₆H₆. and the freezing point is 5.50 °C for benzene.

A solution is 0.0433 mol kg^-1 LiF. What is the molarity of the solution if the density is 1.10 g mL^-1?

How many moles of KF are contained in 347 g of water in a 0.175 mol kg^-1 KF solution?

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl if the solution has a density of 1.20 g mL^-1.

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C₆H₁₂O₆) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

What is the expected van't Hoff factor for MgSO₄? (Assume dilute conditions)

At a given temperature the vapour pressures of benzene and toluene are 183 mmHg and 59.2 mmHg, respectively. Calculate the total vapour pressure over a solution of benzene and toluene with X_benzene = 0. 580.

A compound is found to have a molar mass of 190 g mol^-1. If 0.0673 g of the compound is dissolved in enough water to make 200 mL of solution at 25 °C, what is the osmotic pressure of the resulting solution?

A nonelectrolyte compound with a molar mass of 862 g mol^-1 was dissolved in enough water to make 100 mL of solution at 25 °C and produced an osmotic pressure of 38.4 mbar. Calculate the mass of the compound, in mg, used to make this solution.

The Henry's law constant for helium gas in water at 30 °C is 3.70 × mol L^-1 bar^-1. When the partial pressure of helium above a sample of water is 0.450 bar, the concentration of helium in the water is ________ mol L^-1.

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol^-1 that is dissolved in enough water to create 20.0 mL of solution.

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.