Question 1

Which solution is the most 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 2

Which one of the following compounds would be least soluble in water?

Accepted Answer

A) CH3NH2 
B) CH3CH2OH 
C) CH3COOH 
D) CH3OCH3 
E) CH3CH2CH2CH2CH3 
A) CH3NH2 
B) CH3CH2OH 
C) CH3COOH 
D) CH3OCH3 
E) CH3CH2CH2CH2CH3

Question 3

Which has the lowest boiling point?

Accepted Answer

A) 0.1 M Na2SO4 
B) 0.1 M glucose,C6H12O6 
C) 0.1 M MgCl2 
D) 0.1 M Al(NO3)3 
E) pure water 
A) 0.1 M Na2SO4 
B) 0.1 M glucose,C6H12O6 
C) 0.1 M MgCl2 
D) 0.1 M Al(NO3)3 
E) pure water

Question 4

Match the following.
-saturated

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

Adding solute to a solution increases each of the following except

Accepted Answer

A) molality. 
B) boiling point. 
C) osmotic pressure. 
D) freezing point. 
A) molality. 
B) boiling point. 
C) osmotic pressure. 
D) freezing point.

Question 6

Which statement comparing solutions with pure solvents is not correct?

Accepted Answer

A) A solution containing a non-volatile solute has a lower vapor pressure than pure solvent. 
B) A solution containing a non-volatile solute has a lower boiling point than pure solvent. 
C) A solution containing a non-volatile solute has a lower freezing point than pure solvent. 
D) A solution will have a greater mass than an equal volume of pure solvent if the solute has a molar mass greater than the solvent. 
E) none of the above 
A) A solution containing a non-volatile solute has a lower vapor pressure than pure solvent. 
B) A solution containing a non-volatile solute has a lower boiling point than pure solvent. 
C) A solution containing a non-volatile solute has a lower freezing point than pure solvent. 
D) A solution will have a greater mass than an equal volume of pure solvent if the solute has a molar mass greater than the solvent. 
E) none of the above

Question 7

When a solid dissolves,each molecule is removed from the crystal by interaction with the solvent.This process of surrounding each ion with solvent molecules is called

Accepted Answer

A) dilution. 
B) solvation. 
C) electrolysis. 
D) hemolysis. 
E) crenation. 
A) dilution. 
B) solvation. 
C) electrolysis. 
D) hemolysis. 
E) crenation.

Question 8

Which has the highest boiling point?

Accepted Answer

A) 0.1 M Na2SO4 
B) 0.1 M glucose,C6H12O6 
C) 0.1 M MgCl2 
D) 0.1 M Al(NO3)3 
E) pure water 
A) 0.1 M Na2SO4 
B) 0.1 M glucose,C6H12O6 
C) 0.1 M MgCl2 
D) 0.1 M Al(NO3)3 
E) pure water

Question 9

Which of the following statements about the solubility of gases in liquids is not correct?

Accepted Answer

A) A warm can of soda fizzes more than a cold can of soda when opened because gases are less soluble at higher temperature. 
B) An opened can of soda goes "flat" because the partial pressure of carbon dioxide is lower in the atmosphere than in the unopened can. 
C) A solution stored under an atmosphere of pure nitrogen will contain more dissolved nitrogen than the same solution stored under air because air is only 80% nitrogen. 
D) Fish kills may occur in the summertime because an inadequate amount of oxygen is dissolved in the water. 
E) none of the above 
A) A warm can of soda fizzes more than a cold can of soda when opened because gases are less soluble at higher temperature. 
B) An opened can of soda goes "flat" because the partial pressure of carbon dioxide is lower in the atmosphere than in the unopened can. 
C) A solution stored under an atmosphere of pure nitrogen will contain more dissolved nitrogen than the same solution stored under air because air is only 80% nitrogen. 
D) Fish kills may occur in the summertime because an inadequate amount of oxygen is dissolved in the water. 
E) none of the above

Question 10

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

Accepted Answer

A) 11.2 mL 
B) 50.0 mL 
C) 178 mL 
D) 281 mL 
E) 891 mL 
A) 11.2 mL 
B) 50.0 mL 
C) 178 mL 
D) 281 mL 
E) 891 mL

Question 11

How many milliequivalents of chloride ion are contained in a sample that is determined to contain  
Of chloride ion?

Accepted Answer

A) 48.9 mEq 
B) 41.0 mEq 
C) 25.7 mEq 
D) 20.5 mEq 
E) 10.3 mEq 
A) 48.9 mEq 
B) 41.0 mEq 
C) 25.7 mEq 
D) 20.5 mEq 
E) 10.3 mEq

Question 12

What is the osmolarity of a 0.20 M solution of KCl?

Accepted Answer

A) 0.10 Osmol 
B) 0.20 Osmol 
C) 0.30 Osmol 
D) 0.40 Osmol 
E) 0.80 Osmol 
A) 0.10 Osmol 
B) 0.20 Osmol 
C) 0.30 Osmol 
D) 0.40 Osmol 
E) 0.80 Osmol

Question 13

How many mL of a 5.00% (w/v)glucose solution are needed to provide 20.0 g of glucose?

Accepted Answer

A) 5.00 mL 
B) 20.0 mL 
C) 4.00 mL 
D) 200.mL 
E) 400.mL 
A) 5.00 mL 
B) 20.0 mL 
C) 4.00 mL 
D) 200.mL 
E) 400.mL

Question 14

Consider the following four liquids:
Water: highly polar;H-bonding
Hexanol: slightly polar;some H-bonding
Chloroform: slightly polar;no H-bonding
Octane: non-polar;no H-bonding
Which pair of liquids is immiscible?

Accepted Answer

A) water and octane 
B) water and hexanol 
C) hexanol and chloroform 
D) chloroform and octane 
E) none of the above 
A) water and octane 
B) water and hexanol 
C) hexanol and chloroform 
D) chloroform and octane 
E) none of the above

Question 15

Match the following.
-weak electrolyte

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 16

The term miscible is used to describe which type of solution?

Accepted Answer

A) liquid/liquid 
B) liquid/solid 
C) gas/liquid 
D) gas/gas 
E) all of the above 
A) liquid/liquid 
B) liquid/solid 
C) gas/liquid 
D) gas/gas 
E) all of the above

Question 17

Considering 0.10 M solutions of each substance,which contains the smallest concentration of ions?

Accepted Answer

A) (NH4)3PO4 
B) Ca(NO3)2 
C) FeSO4 
D) K2CO3 
E) Na2SO4 
A) (NH4)3PO4 
B) Ca(NO3)2 
C) FeSO4 
D) K2CO3 
E) Na2SO4

Question 18

Which of the following would be immiscible with carbon tetrachloride,CCl4?

Accepted Answer

A) C6H12 
B) CH3CH2OH 
C) Br2 
D) C3H8 
E) C4H10 
A) C6H12 
B) CH3CH2OH 
C) Br2 
D) C3H8 
E) C4H10

Question 19

How many grams of Fe(NO3)3 are present in a 20.0 mL sample of a 0.500 M solution?

Accepted Answer

A) 2.14 g 
B) 9.68 g 
C) 4.84 g 
D) 2.42 g 
E) 1.21 g 
A) 2.14 g 
B) 9.68 g 
C) 4.84 g 
D) 2.42 g 
E) 1.21 g

Question 20

The passage of a solvent across a semipermeable membrane because of concentration differences is called

Accepted Answer

A) dialysis. 
B) hemolysis. 
C) hydration. 
D) osmosis. 
E) solvation. 
A) dialysis. 
B) hemolysis. 
C) hydration. 
D) osmosis. 
E) solvation.

Exam 9: Solutions

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

Which one of the following compounds would be least soluble in water?

Which has the lowest boiling point?

Match the following. -saturated

Adding solute to a solution increases each of the following except

Which statement comparing solutions with pure solvents is not correct?

When a solid dissolves,each molecule is removed from the crystal by interaction with the solvent.This process of surrounding each ion with solvent molecules is called

Which has the highest boiling point?

Which of the following statements about the solubility of gases in liquids is not correct?

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

How many milliequivalents of chloride ion are contained in a sample that is determined to contain Of chloride ion?

What is the osmolarity of a 0.20 M solution of KCl?

How many mL of a 5.00% (w/v)glucose solution are needed to provide 20.0 g of glucose?

Consider the following four liquids: Water: highly polar;H-bonding Hexanol: slightly polar;some H-bonding Chloroform: slightly polar;no H-bonding Octane: non-polar;no H-bonding Which pair of liquids is immiscible?

Match the following. -weak electrolyte

The term miscible is used to describe which type of solution?

Considering 0.10 M solutions of each substance,which contains the smallest concentration of ions?

Which of the following would be immiscible with carbon tetrachloride,CCl4?

How many grams of Fe(NO3)3 are present in a 20.0 mL sample of a 0.500 M solution?

The passage of a solvent across a semipermeable membrane because of concentration differences is called

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

Which of the following would be immiscible with carbon tetrachloride,CCl₄?

How many grams of Fe(NO₃)₃ are present in a 20.0 mL sample of a 0.500 M solution?