Question 1

Considering 1.0 M solutions of each substance,which contains the largest concentration of ions?

Accepted Answer

A) K2SO4 
B) FeCl3 
C) NaOH 
D) NH3 
E) KCl 
A) K2SO4 
B) FeCl3 
C) NaOH 
D) NH3 
E) KCl B

Question 2

The solubility of nitrogen in water exposed to the atmosphere,where the partial pressure of nitrogen is 593 mm,is 5.3 × 10-4 M.At the same temperature,what would be the solubility of pure nitrogen,at a pressure of 760 mm?

Accepted Answer

A) 4.1 × 10-4 M 
B) 6.8 × 10-4 M 
C) 1500 M 
D) 2400 M 
E) none of the above 
A) 4.1 × 10-4 M 
B) 6.8 × 10-4 M 
C) 1500 M 
D) 2400 M 
E) none of the above B

Question 3

All of the following statements describing solutions are true except

Accepted Answer

A) making a solution involves a physical change. 
B) solutions are homogeneous. 
C) the particles in a solution are atomic or molecular in size. 
D) solutions are colorless. 
E) solutions are transparent. 
A) making a solution involves a physical change. 
B) solutions are homogeneous. 
C) the particles in a solution are atomic or molecular in size. 
D) solutions are colorless. 
E) solutions are transparent. D

Question 4

Match the following.
-hypotonic

Accepted Answer

A) an ionic compound which attracts water molecules from the atmosphere 
B) a solution in which no more solute will dissolve and in which excess solute is visible in the container 
C) a substance which dissociates completely in solution,providing a relatively large number of ions to conduct electricity 
D) refers to a solution having a lower osmolarity than 0.30 Osmol 
E) an ionic compound which holds water molecules within its crystalline structure
F)refers to two solutions having the same osmolarity
G)a substance which does not dissociate in solution and therefore does not conduct electricity
H)a solution in which more solute is dissolved than predicted for that particular temperature
I)refers to a solution having a greater osmolarity than 0.30 Osmol
J)the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself
K)the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself
L)a solution in which more solute can be dissolved
M)a substance which partially dissociates in solution,providing a relatively small number of ions to conduct electricity 
A) an ionic compound which attracts water molecules from the atmosphere 
B) a solution in which no more solute will dissolve and in which excess solute is visible in the container 
C) a substance which dissociates completely in solution,providing a relatively large number of ions to conduct electricity 
D) refers to a solution having a lower osmolarity than 0.30 Osmol 
E) an ionic compound which holds water molecules within its crystalline structure
F)refers to two solutions having the same osmolarity
G)a substance which does not dissociate in solution and therefore does not conduct electricity
H)a solution in which more solute is dissolved than predicted for that particular temperature
I)refers to a solution having a greater osmolarity than 0.30 Osmol
J)the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself
K)the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself
L)a solution in which more solute can be dissolved
M)a substance which partially dissociates in solution,providing a relatively small number of ions to conduct electricity

Question 5

Which is not an example of a solution?

Accepted Answer

A) the mixture of gases in a SCUBA diving tank 
B) a coin made from nickel and copper 
C) spring water purchased at a supermarket 
D) antifreeze in a car radiator 
E) none of the above 
A) the mixture of gases in a SCUBA diving tank 
B) a coin made from nickel and copper 
C) spring water purchased at a supermarket 
D) antifreeze in a car radiator 
E) none of the above

Question 6

Which one of the following would act like a strong electrolyte in an aqueous solution?

Accepted Answer

A) KNO3 
B) CH3OH 
C) CCl4 
D) NH3 
A) KNO3 
B) CH3OH 
C) CCl4 
D) NH3

Question 7

How many grams of NaOH are needed to make 750 mL of a 2.5% (w/v)solution?

Accepted Answer

A) 3.9 g 
B) 7.5 g 
C) 19 g 
D) 20 g 
E) 50 g 
A) 3.9 g 
B) 7.5 g 
C) 19 g 
D) 20 g 
E) 50 g

Question 8

What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?

Accepted Answer

A) 1.2 M 
B) 1.5 M 
C) 6.0 M 
D) 24 M 
E) 30 M 
A) 1.2 M 
B) 1.5 M 
C) 6.0 M 
D) 24 M 
E) 30 M

Question 9

The solubility of gases in liquids

Accepted Answer

A) increases as temperature increases and increases as pressure increases. 
B) decreases as temperature increases and increases as pressure increases. 
C) decreases as temperature increases and decreases as pressure increases. 
D) increases as temperature increases and decreases as pressure increases. 
E) is independent of temperature and increases as pressure increases. 
A) increases as temperature increases and increases as pressure increases. 
B) decreases as temperature increases and increases as pressure increases. 
C) decreases as temperature increases and decreases as pressure increases. 
D) increases as temperature increases and decreases as pressure increases. 
E) is independent of temperature and increases as pressure increases.

Question 10

Which solution is the least concentrated? Each choice refers to the same solute and solvent.

Accepted Answer

A) 2.4 g solute in 2 mL solution 
B) 2.4 g solute in 5 mL solution 
C) 20 g solute in 50 mL solution 
D) 30 g solute in 150 mL solution 
E) 50 g solute in 175 mL solution 
A) 2.4 g solute in 2 mL solution 
B) 2.4 g solute in 5 mL solution 
C) 20 g solute in 50 mL solution 
D) 30 g solute in 150 mL solution 
E) 50 g solute in 175 mL solution

Question 11

In a mixture of 5 mL water,10 mL alcohol,and 50 mL acetone the solvent(s)is(are)

Accepted Answer

A) acetone. 
B) alcohol. 
C) water. 
D) acetone and alcohol. 
E) alcohol and water. 
A) acetone. 
B) alcohol. 
C) water. 
D) acetone and alcohol. 
E) alcohol and water.

Question 12

How many grams of CaCl2 are needed to prepare 125 mL of a 1.50 M solution?

Accepted Answer

A) 0.188 g 
B) 1.69 g 
C) 3.00 g 
D) 20.8 g 
E) 37.0 g 
A) 0.188 g 
B) 1.69 g 
C) 3.00 g 
D) 20.8 g 
E) 37.0 g

Question 13

What is the molarity of a solution prepared by dissolving 10.0 g of acetone,C3H6O,in enough water to make 125 mL of solution?

Accepted Answer

A) 4.65 M 
B) 1.38 M 
C) 0.0465 M 
D) 0.0214 M 
E) 0.0125 M 
A) 4.65 M 
B) 1.38 M 
C) 0.0465 M 
D) 0.0214 M 
E) 0.0125 M

Question 14

All of the statements about molarity are correct except

Accepted Answer

A) the abbreviation is M. 
B) the interpretation of the symbol is "moles of solute per mole of solvent." 
C) moles = molarity × volume. 
D) volume = moles/molarity. 
E) the molarity of a diluted solution is less than the molarity of the original solution. 
A) the abbreviation is M. 
B) the interpretation of the symbol is "moles of solute per mole of solvent." 
C) moles = molarity × volume. 
D) volume = moles/molarity. 
E) the molarity of a diluted solution is less than the molarity of the original solution.

Question 15

What is the % (w/v)concentration of a solution containing 25.0 g of solute in 400.mL of solution?

Accepted Answer

A) 2.50% 
B) 5.00% 
C) 6.25% 
D) 12.5% 
E) 25.0% 
A) 2.50% 
B) 5.00% 
C) 6.25% 
D) 12.5% 
E) 25.0%

Question 16

A water solution of sodium chloride is a good conductor of electricity.Due to this property,table salt is classified as a(n)

Accepted Answer

A) weak electrolyte. 
B) strong electrolyte. 
C) non-electrolyte. 
D) semi-electrolyte. 
E) none of these. 
A) weak electrolyte. 
B) strong electrolyte. 
C) non-electrolyte. 
D) semi-electrolyte. 
E) none of these.

Question 17

How many mL of a 0.200 M HNO3 solution contains 10.0 g of HNO3?

Accepted Answer

A) 2.00 mL 
B) 31.7 mL 
C) 159 mL 
D) 315 mL 
E) 793 mL 
A) 2.00 mL 
B) 31.7 mL 
C) 159 mL 
D) 315 mL 
E) 793 mL

Question 18

Match the following.
-unsaturated

Accepted Answer

A) an ionic compound which attracts water molecules from the atmosphere 
B) a solution in which no more solute will dissolve and in which excess solute is visible in the container 
C) a substance which dissociates completely in solution,providing a relatively large number of ions to conduct electricity 
D) refers to a solution having a lower osmolarity than 0.30 Osmol 
E) an ionic compound which holds water molecules within its crystalline structure
F)refers to two solutions having the same osmolarity
G)a substance which does not dissociate in solution and therefore does not conduct electricity
H)a solution in which more solute is dissolved than predicted for that particular temperature
I)refers to a solution having a greater osmolarity than 0.30 Osmol
J)the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself
K)the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself
L)a solution in which more solute can be dissolved
M)a substance which partially dissociates in solution,providing a relatively small number of ions to conduct electricity 
A) an ionic compound which attracts water molecules from the atmosphere 
B) a solution in which no more solute will dissolve and in which excess solute is visible in the container 
C) a substance which dissociates completely in solution,providing a relatively large number of ions to conduct electricity 
D) refers to a solution having a lower osmolarity than 0.30 Osmol 
E) an ionic compound which holds water molecules within its crystalline structure
F)refers to two solutions having the same osmolarity
G)a substance which does not dissociate in solution and therefore does not conduct electricity
H)a solution in which more solute is dissolved than predicted for that particular temperature
I)refers to a solution having a greater osmolarity than 0.30 Osmol
J)the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself
K)the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself
L)a solution in which more solute can be dissolved
M)a substance which partially dissociates in solution,providing a relatively small number of ions to conduct electricity

Question 19

Match the following.
-hydrate

Accepted Answer

A) an ionic compound which attracts water molecules from the atmosphere 
B) a solution in which no more solute will dissolve and in which excess solute is visible in the container 
C) a substance which dissociates completely in solution,providing a relatively large number of ions to conduct electricity 
D) refers to a solution having a lower osmolarity than 0.30 Osmol 
E) an ionic compound which holds water molecules within its crystalline structure
F)refers to two solutions having the same osmolarity
G)a substance which does not dissociate in solution and therefore does not conduct electricity
H)a solution in which more solute is dissolved than predicted for that particular temperature
I)refers to a solution having a greater osmolarity than 0.30 Osmol
J)the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself
K)the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself
L)a solution in which more solute can be dissolved
M)a substance which partially dissociates in solution,providing a relatively small number of ions to conduct electricity 
A) an ionic compound which attracts water molecules from the atmosphere 
B) a solution in which no more solute will dissolve and in which excess solute is visible in the container 
C) a substance which dissociates completely in solution,providing a relatively large number of ions to conduct electricity 
D) refers to a solution having a lower osmolarity than 0.30 Osmol 
E) an ionic compound which holds water molecules within its crystalline structure
F)refers to two solutions having the same osmolarity
G)a substance which does not dissociate in solution and therefore does not conduct electricity
H)a solution in which more solute is dissolved than predicted for that particular temperature
I)refers to a solution having a greater osmolarity than 0.30 Osmol
J)the swelling and bursting of a red blood cell when placed in a solution of lower osmolarity than the cell itself
K)the shrinking of a red blood cell when placed in a solution of greater osmolarity than the cell itself
L)a solution in which more solute can be dissolved
M)a substance which partially dissociates in solution,providing a relatively small number of ions to conduct electricity

Question 20

Which solution has the greatest osmolarity?

Accepted Answer

A) 0.6 M NaCl 
B) 0.35 M AlCl3 
C) 0.14 M KF 
D) 0.2 M CaBr2 
E) 0.10 M KNO3 
A) 0.6 M NaCl 
B) 0.35 M AlCl3 
C) 0.14 M KF 
D) 0.2 M CaBr2 
E) 0.10 M KNO3

Exam 9: Solutions

Considering 1.0 M solutions of each substance,which contains the largest concentration of ions?

The solubility of nitrogen in water exposed to the atmosphere,where the partial pressure of nitrogen is 593 mm,is 5.3 × 10-4 M.At the same temperature,what would be the solubility of pure nitrogen,at a pressure of 760 mm?

All of the following statements describing solutions are true except

Match the following. -hypotonic

Which is not an example of a solution?

Which one of the following would act like a strong electrolyte in an aqueous solution?

How many grams of NaOH are needed to make 750 mL of a 2.5% (w/v)solution?

What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?

The solubility of gases in liquids

Which solution is the least concentrated? Each choice refers to the same solute and solvent.

In a mixture of 5 mL water,10 mL alcohol,and 50 mL acetone the solvent(s)is(are)

How many grams of CaCl2 are needed to prepare 125 mL of a 1.50 M solution?

What is the molarity of a solution prepared by dissolving 10.0 g of acetone,C3H6O,in enough water to make 125 mL of solution?

All of the statements about molarity are correct except

What is the % (w/v)concentration of a solution containing 25.0 g of solute in 400.mL of solution?

A water solution of sodium chloride is a good conductor of electricity.Due to this property,table salt is classified as a(n)

How many mL of a 0.200 M HNO3 solution contains 10.0 g of HNO3?

Match the following. -unsaturated

Match the following. -hydrate

Which solution has the greatest osmolarity?

Matter and Measurements

Atoms and the Periodic Table

Ionic Compounds

Molecular Compounds

Classification and Balancing of Chemical Reactions

Chemical Reactions: Mole and Mass Relationships

Chemical Reactions: Energy, rates, and Equilibrium

Gases, liquids, and Solids

Acids and Bases

Nuclear Chemistry

Introduction to Organic Chemistry: Alkanes

Alkenes, alkynes, and Aromatic Compounds

Some Compounds With Oxygen, sulfur, or a Halogen

Aldehydes and Ketones

Amines

Carboxylic Acids and Their Derivatives

Amino Acids and Proteins

Enzymes and Vitamins

Carbohydrates

The Generation of Biochemical Energy

Carbohydrate Metabolism

Lipids

Lipid Metabolism

Protein and Amino Acid Metabolism

Nucleic Acids and Protein Synthesis

Genomics

Chemical Messengers: Hormones, neurotransmitters, and Drugs

Body Fluids

Filters

The solubility of nitrogen in water exposed to the atmosphere,where the partial pressure of nitrogen is 593 mm,is 5.3 × 10^-4 M.At the same temperature,what would be the solubility of pure nitrogen,at a pressure of 760 mm?

How many grams of CaCl₂ are needed to prepare 125 mL of a 1.50 M solution?

What is the molarity of a solution prepared by dissolving 10.0 g of acetone,C₃H₆O,in enough water to make 125 mL of solution?

How many mL of a 0.200 M HNO₃ solution contains 10.0 g of HNO₃?