Question 1

Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL of pure water.

Accepted Answer

A) 27.3 
B) 72.3 
C) 47.0 
D) 37.6 
E) none of the above 
A) 27.3 
B) 72.3 
C) 47.0 
D) 37.6 
E) none of the above

Question 2

A saturated solution holds the maximum amount of solute under the solution conditions.

Accepted Answer

A) True 
 B)False

Question 3

When preparing sodium hydroxide solution,it is best to use water that does not contain any dissolved carbon dioxide as it reacts with the sodium hydroxide.Removing the carbon dioxide can be accomplished by:

Accepted Answer

A) vigorously stirring the solution. 
B) using water fresh out of the purification system. 
C) boiling the water. 
D) Nothing can be done to remove dissolved gases. 
E) none of the above 
A) vigorously stirring the solution. 
B) using water fresh out of the purification system. 
C) boiling the water. 
D) Nothing can be done to remove dissolved gases. 
E) none of the above

Question 4

The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.

Accepted Answer

A) True 
 B)False

Question 5

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker,the solution would be considered ________.

Accepted Answer

A) unsaturated 
B) saturated 
C) supersaturated 
D) thermally saturated 
E) none of the above 
A) unsaturated 
B) saturated 
C) supersaturated 
D) thermally saturated 
E) none of the above

Question 6

A sugar solution is an example of a weak electrolyte solution.

Accepted Answer

A) True 
 B)False

Question 7

Which of the following statements about colligative properties is FALSE?

Accepted Answer

A) The boiling point of a solution is increased by the addition of salt. 
B) The freezing point of a solution is lowered by the addition of salt. 
C) The change in temperature is proportional to the molality. 
D) The identity of the solute is not a factor. 
E) All of the above statements are true. 
A) The boiling point of a solution is increased by the addition of salt. 
B) The freezing point of a solution is lowered by the addition of salt. 
C) The change in temperature is proportional to the molality. 
D) The identity of the solute is not a factor. 
E) All of the above statements are true.

Question 8

How many mL of 0.112 M Pb(NO3)2 are needed to completely react with 25.0 mL of 0.105 M KI? 
Given:

Accepted Answer

A) 11.7 
B) 23.4 
C) 0.147 
D) 5.85 
E) none of the above 
A) 11.7 
B) 23.4 
C) 0.147 
D) 5.85 
E) none of the above

Question 9

The tragedy at Lake Nyos in Cameroon,West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water.

Accepted Answer

A) True 
 B)False

Question 10

Which among the following is NOT true about the solubility of a solid in water?

Accepted Answer

A) The solubility is not affected by pressure. 
B) The solubility generally increases as temperature increases. 
C) Solid crystallizes when a saturated solution is prepared at a higher temperature and then cooled. 
D) A saturated solution prepared at a lower temperature becomes unsaturated when heated to a higher temperature. 
E) none of the above 
A) The solubility is not affected by pressure. 
B) The solubility generally increases as temperature increases. 
C) Solid crystallizes when a saturated solution is prepared at a higher temperature and then cooled. 
D) A saturated solution prepared at a lower temperature becomes unsaturated when heated to a higher temperature. 
E) none of the above

Question 11

Which of the following compounds is a strong electrolyte?

Accepted Answer

A) HCl 
B) NaCl 
C) NH4Cl 
D) NaC2H3O2 
E) all of the above 
A) HCl 
B) NaCl 
C) NH4Cl 
D) NaC2H3O2 
E) all of the above

Question 12

Given that the freezing point depression constant for water is 1.86°C kg/mol,calculate the change in freezing point for a 0.907 mugar solution.

Accepted Answer

A) 0.488°C 
B) 2.05°C 
C) 0.592°C 
D) 1.69°C 
E) none of the above 
A) 0.488°C 
B) 2.05°C 
C) 0.592°C 
D) 1.69°C 
E) none of the above

Question 13

The solubility of a gas in a liquid can always be increased by:

Accepted Answer

A) increasing the temperature of the solvent. 
B) decreasing the polarity of the solvent. 
C) decreasing the pressure of the gas above the solvent. 
D) increasing the pressure of the gas above the solvent. 
E) none of the above 
A) increasing the temperature of the solvent. 
B) decreasing the polarity of the solvent. 
C) decreasing the pressure of the gas above the solvent. 
D) increasing the pressure of the gas above the solvent. 
E) none of the above

Question 14

The minor component in a solution is called the solvent.

Accepted Answer

A) True 
 B)False

Question 15

The major component in a solution is called the solute.

Accepted Answer

A) True 
 B)False

Question 16

Which of the following substances is NOT a solution?

Accepted Answer

A) homogenized milk 
B) bronze 
C) sea water 
D) soda 
E) All of the above are solutions. 
A) homogenized milk 
B) bronze 
C) sea water 
D) soda 
E) All of the above are solutions.

Question 17

A solution contains 100.0 g water,10.0 g NaCl,and 15.0 g methanol.What is the mass percent of methanol in the solution?

Accepted Answer

A) 8.00% 
B) 10.0% 
C) 12.0% 
D) 15.0% 
E) none of the above 
A) 8.00% 
B) 10.0% 
C) 12.0% 
D) 15.0% 
E) none of the above

Question 18

A stock solution is a more concentrated form than what is typically used in a lab.It often requires further dilution.

Accepted Answer

A) True 
 B)False

Question 19

What are the ion concentrations in a 0.12 M solution of AlCl3?

Accepted Answer

A) 0.36 M Al3+ ions and 0.12 M Cl- ions 
B) 0.12 M Al3+ ions and 0.040 M Cl- ions 
C) 0.12 M Al3+ ions and 0.36 M Cl- ions 
D) 0.040 M Al3+ ions and 0.040 M Cl- ions 
E) none of the above 
A) 0.36 M Al3+ ions and 0.12 M Cl- ions 
B) 0.12 M Al3+ ions and 0.040 M Cl- ions 
C) 0.12 M Al3+ ions and 0.36 M Cl- ions 
D) 0.040 M Al3+ ions and 0.040 M Cl- ions 
E) none of the above

Question 20

Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of 500 mL .

Accepted Answer

A) 0.331 
B) 0.663 
C) 0.166 
D) 6.04 
E) none of the above 
A) 0.331 
B) 0.663 
C) 0.166 
D) 6.04 
E) none of the above

Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL of pure water.

A saturated solution holds the maximum amount of solute under the solution conditions.

When preparing sodium hydroxide solution,it is best to use water that does not contain any dissolved carbon dioxide as it reacts with the sodium hydroxide.Removing the carbon dioxide can be accomplished by:

The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker,the solution would be considered ________.

A sugar solution is an example of a weak electrolyte solution.

Which of the following statements about colligative properties is FALSE?

How many mL of 0.112 M Pb(NO₃)₂ are needed to completely react with 25.0 mL of 0.105 M KI? Given:

The tragedy at Lake Nyos in Cameroon,West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water.

Which among the following is NOT true about the solubility of a solid in water?

Which of the following compounds is a strong electrolyte?

Given that the freezing point depression constant for water is 1.86°C kg/mol,calculate the change in freezing point for a 0.907 mugar solution.

The solubility of a gas in a liquid can always be increased by:

The minor component in a solution is called the solvent.

The major component in a solution is called the solute.

Which of the following substances is NOT a solution?

A solution contains 100.0 g water,10.0 g NaCl,and 15.0 g methanol.What is the mass percent of methanol in the solution?

A stock solution is a more concentrated form than what is typically used in a lab.It often requires further dilution.

What are the ion concentrations in a 0.12 M solution of AlCl₃?

Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of 500 mL .

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Exam 13: Solutions

Calculate the mass percent of a NaCl solution prepared by mixing 47.0 g NaCl with 125.0 mL of pure water.

A saturated solution holds the maximum amount of solute under the solution conditions.

When preparing sodium hydroxide solution,it is best to use water that does not contain any dissolved carbon dioxide as it reacts with the sodium hydroxide.Removing the carbon dioxide can be accomplished by:

The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker,the solution would be considered ________.

A sugar solution is an example of a weak electrolyte solution.

Which of the following statements about colligative properties is FALSE?

How many mL of 0.112 M Pb(NO3)2 are needed to completely react with 25.0 mL of 0.105 M KI? Given:

The tragedy at Lake Nyos in Cameroon,West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water.

Which among the following is NOT true about the solubility of a solid in water?

Which of the following compounds is a strong electrolyte?

Given that the freezing point depression constant for water is 1.86°C kg/mol,calculate the change in freezing point for a 0.907 mugar solution.

The solubility of a gas in a liquid can always be increased by:

The minor component in a solution is called the solvent.

The major component in a solution is called the solute.

Which of the following substances is NOT a solution?

A solution contains 100.0 g water,10.0 g NaCl,and 15.0 g methanol.What is the mass percent of methanol in the solution?

A stock solution is a more concentrated form than what is typically used in a lab.It often requires further dilution.

What are the ion concentrations in a 0.12 M solution of AlCl3?

Calculate the molarity of a KCl solution made by dissolving 24.7 g of KCl in a total volume of 500 mL .

The Chemical World

Measurement and Problem Solving

Matter and Energy

Atoms and Elements

Molecules and Compounds

Chemical Composition

Chemical Reactions

Quantities in Chemical Reactions

Electrons in Atoms and the Periodic Table

Chemical Bonding

Gases

Liquids, solids, and Intermolecular Forces

Acids and Bases

Chemical Equilibrium

Oxidation and Reduction

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

How many mL of 0.112 M Pb(NO₃)₂ are needed to completely react with 25.0 mL of 0.105 M KI? Given:

What are the ion concentrations in a 0.12 M solution of AlCl₃?