Question 1

What happens to a supersaturated solution of potassium acetate once it is cooled and a small crystal of solid potassium acetate is added?

Accepted Answer

The portion of potassium aceta

Question 2

Why isn't pentanol (CH3CH2CH2CH2CH2OH)very soluble in water?

Accepted Answer

Even though the pentanol molecule contai

Question 3

To make a 0.500 M solution,one could take 0.500 moles of solute and add

Accepted Answer

A) 1.00 L of solvent. 
B) 1.00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution. 
A) 1.00 L of solvent. 
B) 1.00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution.

Question 4

Define molality.

Accepted Answer

The amount of solute

Question 5

A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Accepted Answer

A) 21.6 mm Hg 
B) 22.7 mm Hg 
C) 23.2 mm Hg 
D) 24.9 mm Hg 
A) 21.6 mm Hg 
B) 22.7 mm Hg 
C) 23.2 mm Hg 
D) 24.9 mm Hg

Question 6

Determine DHlattice for KBr if the ΔHsolution (KBr)= +19.9 kJ/mol and the
ΔHhydration (KBr)= -670.kJ/mol.

Accepted Answer

A) +650 kJ/mol 
B) -650 kJ/mol 
C) +690 kJ/mol 
D) -710 kJ/mol 
E) -690 kJ/mol 
A) +650 kJ/mol 
B) -650 kJ/mol 
C) +690 kJ/mol 
D) -710 kJ/mol 
E) -690 kJ/mol

Question 7

Match the following.
-0.0050 m CO2

Accepted Answer

A) largest van't Hoff factor 
B) solution of ionic compound with highest freezing point 
C) solution with ΔTb = 0.026°C 
D) highest boiling point 
E) solution that is most strongly dependent upon pressure 
A) largest van't Hoff factor 
B) solution of ionic compound with highest freezing point 
C) solution with ΔTb = 0.026°C 
D) highest boiling point 
E) solution that is most strongly dependent upon pressure

Question 8

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine,C8H10N4O2,in 75 g of benzene,C6H6?

Accepted Answer

A) 0.010% 
B) 0.011% 
C) 10% 
D) 11% 
A) 0.010% 
B) 0.011% 
C) 10% 
D) 11%

Question 9

Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.2 atm.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm.

Accepted Answer

A) 0.15 M 
B) 0.57 M 
C) 0.65 M 
D) 0.18 M 
E) 0.29 M 
A) 0.15 M 
B) 0.57 M 
C) 0.65 M 
D) 0.18 M 
E) 0.29 M

Question 10

A compound is found to have a molar mass of 598 g/mol.If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C,what is the osmotic pressure of the resulting solution?

Accepted Answer

A) 3.42 torr 
B) 6.36 torr 
C) 5.01 torr 
D) 5.99 torr 
E) 8.36 torr 
A) 3.42 torr 
B) 6.36 torr 
C) 5.01 torr 
D) 5.99 torr 
E) 8.36 torr

Question 11

Choose the situation below that would result in an exothermic ΔHsolution.

Accepted Answer

A) When  >   
B) When  Is close to   
C) When  >   
E) There isn't enough information to determine. 
A) When  >   
B) When  Is close to   
C) When  >   
E) There isn't enough information to determine.

Question 12

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

Accepted Answer

A) CCl4,Kb = 29.9°C/m 
B) C6H6,Kb = 5.12°C/m 
C) CH3CH2OCH2CH3,Kb = 1.79°C/m 
D) CH3CH2OH,Kb = 1.99°C/m 
E) CHCl3,Kb = 4.70°C/m 
A) CCl4,Kb = 29.9°C/m 
B) C6H6,Kb = 5.12°C/m 
C) CH3CH2OCH2CH3,Kb = 1.79°C/m 
D) CH3CH2OH,Kb = 1.99°C/m 
E) CHCl3,Kb = 4.70°C/m

Question 13

What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.

Accepted Answer

A) -0.93°C 
B) -1.9°C 
C) -2.8°C 
D) -6.5°C 
A) -0.93°C 
B) -1.9°C 
C) -2.8°C 
D) -6.5°C

Question 14

Choose the statement below that is true.

Accepted Answer

A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. 
B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. 
C) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. 
D) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. 
E) None of the above are true. 
A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. 
B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions. 
C) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions. 
D) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions. 
E) None of the above are true.

Question 15

Place the following solutions in order of increasing osmotic pressure.
I.0.15 M C2H6O2 
II.0.15 M MgCl2 
III.0.15 M NaCl

Accepted Answer

A) III < I < II 
B) II < III < I 
C) I < II < III 
D) II < I < III 
E) I < III < II 
A) III < I < II 
B) II < III < I 
C) I < II < III 
D) II < I < III 
E) I < III < II

Question 16

A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions.Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.

Accepted Answer

A) 2.8 ppm 
B) 7.2 ppm 
C) 3.6 ppm 
D) 1.8 ppm 
E) 5.4 ppm 
A) 2.8 ppm 
B) 7.2 ppm 
C) 3.6 ppm 
D) 1.8 ppm 
E) 5.4 ppm

Question 17

Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of
0.022 atm produces a solution with a concentration of 1.3 M.

Accepted Answer

A) 59 M/atm 
B) 0.017 M/atm 
C) 0.029 M/atm 
D) 35 M/atm 
E) 0.038 M/atm 
A) 59 M/atm 
B) 0.017 M/atm 
C) 0.029 M/atm 
D) 35 M/atm 
E) 0.038 M/atm

Question 18

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water.The vapor pressure of pure water at 55°C is 118.1 torr.

Accepted Answer

A) 115 torr 
B) 87.1 torr 
C) 108 torr 
D) 112 torr 
E) 92.8 torr 
A) 115 torr 
B) 87.1 torr 
C) 108 torr 
D) 112 torr 
E) 92.8 torr

Question 19

A solution is prepared by dissolving 16.2 g of benzene (C6H6)in 282 g of carbon tetrachloride (CCl4).The concentration of benzene in this solution is ________ molal.The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol,respectively.

Accepted Answer

A) 7.36 × 10-4 
B) 0.736 
C) 0.102 
D) 0.0543 
E) 5.43 
A) 7.36 × 10-4 
B) 0.736 
C) 0.102 
D) 0.0543 
E) 5.43

Question 20

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6)in 250.0 mL of water.The vapor pressure of pure water at 25°C is 23.8 torr.

Accepted Answer

A) 70.8 torr 
B) 72.9 torr 
C) 23.1 torr 
D) 22.9 torr 
E) 7.29 torr 
A) 70.8 torr 
B) 72.9 torr 
C) 23.1 torr 
D) 22.9 torr 
E) 7.29 torr

What happens to a supersaturated solution of potassium acetate once it is cooled and a small crystal of solid potassium acetate is added?

Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH)very soluble in water?

To make a 0.500 M solution,one could take 0.500 moles of solute and add

Define molality.

A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Determine DH_lattice for KBr if the ΔH_solution(KBr)= +19.9 kJ/mol and the ΔH_hydration(KBr)= -670.kJ/mol.

Match the following. -0.0050 m CO₂

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine,C₈H₁₀N₄O₂,in 75 g of benzene,C₆H₆?

Determine the solubility of CO₂ in soda water at 25°C if the pressure of CO₂ is 5.2 atm.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 M/atm.

A compound is found to have a molar mass of 598 g/mol.If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C,what is the osmotic pressure of the resulting solution?

Choose the situation below that would result in an exothermic ΔH_solution.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

What is the expected freezing point of a 0.50 m solution of Li₂SO₄ in water? K_f for water is 1.86°C/m.

Choose the statement below that is true.

Place the following solutions in order of increasing osmotic pressure. I.0.15 M C₂H₆O₂ II.0.15 M MgCl₂ III.0.15 M NaCl

A 1.00 L sample of water contains 0.0036 g of Cl^⁻ ions.Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.

Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water.The vapor pressure of pure water at 55°C is 118.1 torr.

A solution is prepared by dissolving 16.2 g of benzene (C₆H₆)in 282 g of carbon tetrachloride (CCl₄).The concentration of benzene in this solution is ________ molal.The molar masses of C₆H₆ and CCl₄ are 78.1 g/mol and 154 g/mol,respectively.

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C₆H₁₂O₆)in 250.0 mL of water.The vapor pressure of pure water at 25°C is 23.8 torr.

Matter, Measurement, and Problem Solving

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Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

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

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Chemical Kinetics

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Exam 12: Solutions

What happens to a supersaturated solution of potassium acetate once it is cooled and a small crystal of solid potassium acetate is added?

Why isn't pentanol (CH3CH2CH2CH2CH2OH)very soluble in water?

To make a 0.500 M solution,one could take 0.500 moles of solute and add

Define molality.

A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Determine DHlattice for KBr if the ΔHsolution (KBr)= +19.9 kJ/mol and the ΔHhydration (KBr)= -670.kJ/mol.

Match the following. -0.0050 m CO2

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine,C8H10N4O2,in 75 g of benzene,C6H6?

Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.2 atm.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 M/atm.

A compound is found to have a molar mass of 598 g/mol.If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C,what is the osmotic pressure of the resulting solution?

Choose the situation below that would result in an exothermic ΔHsolution.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 m nonelectrolyte solution.

What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.

Choose the statement below that is true.

Place the following solutions in order of increasing osmotic pressure. I.0.15 M C2H6O2 II.0.15 M MgCl2 III.0.15 M NaCl

A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions.Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.

Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water.The vapor pressure of pure water at 55°C is 118.1 torr.

A solution is prepared by dissolving 16.2 g of benzene (C6H6)in 282 g of carbon tetrachloride (CCl4).The concentration of benzene in this solution is ________ molal.The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol,respectively.

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6)in 250.0 mL of water.The vapor pressure of pure water at 25°C is 23.8 torr.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

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

Liquids, Solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH)very soluble in water?

Determine DH_lattice for KBr if the ΔH_solution(KBr)= +19.9 kJ/mol and the ΔH_hydration(KBr)= -670.kJ/mol.

Match the following. -0.0050 m CO₂

What is the weight percent of a caffeine solution made by dissolving 8.35 g of caffeine,C₈H₁₀N₄O₂,in 75 g of benzene,C₆H₆?

Determine the solubility of CO₂ in soda water at 25°C if the pressure of CO₂ is 5.2 atm.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 M/atm.

Choose the situation below that would result in an exothermic ΔH_solution.

What is the expected freezing point of a 0.50 m solution of Li₂SO₄ in water? K_f for water is 1.86°C/m.

Place the following solutions in order of increasing osmotic pressure. I.0.15 M C₂H₆O₂ II.0.15 M MgCl₂ III.0.15 M NaCl

A 1.00 L sample of water contains 0.0036 g of Cl^⁻ ions.Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.

A solution is prepared by dissolving 16.2 g of benzene (C₆H₆)in 282 g of carbon tetrachloride (CCl₄).The concentration of benzene in this solution is ________ molal.The molar masses of C₆H₆ and CCl₄ are 78.1 g/mol and 154 g/mol,respectively.

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C₆H₁₂O₆)in 250.0 mL of water.The vapor pressure of pure water at 25°C is 23.8 torr.