Question 1

How many moles of HCl are present in 75.0 mL of a 0.200 M solution?

Accepted Answer

A) 15.0 mol 
B) 2.67 mol 
C) 0.375 mol 
D) 0.275 mol 
E) 0.0150 mol 
A) 15.0 mol 
B) 2.67 mol 
C) 0.375 mol 
D) 0.275 mol 
E) 0.0150 mol

Question 2

The exothermic step in the dissolution of NaCl in water is

Accepted Answer

A) the separation of the ions in the salt. 
B) the separation of the water molecules. 
C) solvation (hydration)of the ions from the salt. 
D) separation of the ions in the salt and the separation of the water molecules. 
A) the separation of the ions in the salt. 
B) the separation of the water molecules. 
C) solvation (hydration)of the ions from the salt. 
D) separation of the ions in the salt and the separation of the water molecules.

Question 3

Match the following.
-crenation

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 4

Pressure has a large effect only on the solubility of ________ in liquids.

Accepted Answer

A) liquid 
B) solid 
C) gas 
D) all of the above 
E) none of the above 
A) liquid 
B) solid 
C) gas 
D) all of the above 
E) none of the above

Question 5

The number of components in a solution is

Accepted Answer

A) at least 2. 
B) 3. 
C) 4. 
D) 5. 
E) 6. 
A) at least 2. 
B) 3. 
C) 4. 
D) 5. 
E) 6.

Question 6

All of the water in a 0.200 M solution of NaCl was evaporated and 0.150 mole of NaCl was obtained.What was the original volume of the sample?

Accepted Answer

A) 30.0 mL 
B) 333 mL 
C) 750.mL 
D) 1000 mL (1.00 × 103 mL) 
E) 1330 mL 
A) 30.0 mL 
B) 333 mL 
C) 750.mL 
D) 1000 mL (1.00 × 103 mL) 
E) 1330 mL

Question 7

Which aqueous solution will have the lowest freezing point?

Accepted Answer

A) 0.60 molal sucrose 
B) 0.50 molal KF 
C) 0.60 molal glucose 
D) 0.24 molal FeI3 
A) 0.60 molal sucrose 
B) 0.50 molal KF 
C) 0.60 molal glucose 
D) 0.24 molal FeI3

Question 8

How many mL of water should be added to 50.0 mL of a 15.0 M H2SO4 solution to give a final concentration of 0.300 M?

Accepted Answer

A) 950 mL 
B) 1000 mL 
C) 2450 mL 
D) 2500 mL 
E) 2550 mL 
A) 950 mL 
B) 1000 mL 
C) 2450 mL 
D) 2500 mL 
E) 2550 mL

Question 9

Match the following.
-strong 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 10

If "A" contains 2% NaCl and is separated by a semipermeable membrane from "B" which contains 10% NaCl,which event will occur?

Accepted Answer

A) NaCl will flow from "A" to "B". 
B) NaCl will flow from "B" to "A". 
C) Water will flow from "A" to "B". 
D) Water will flow from "B" to "A". 
E) none of the above 
A) NaCl will flow from "A" to "B". 
B) NaCl will flow from "B" to "A". 
C) Water will flow from "A" to "B". 
D) Water will flow from "B" to "A". 
E) none of the above

Question 11

Match the following.
-supersaturated

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 12

How many moles of solute are present in 12.0 L of 3.00 M HCl?

Accepted Answer

A) 36.0 mol 
B) 4.00 mol 
C) 0.250 mol 
D) 3.00 mol 
E) 0.750 mol 
A) 36.0 mol 
B) 4.00 mol 
C) 0.250 mol 
D) 3.00 mol 
E) 0.750 mol

Question 13

A supersaturated solution

Accepted Answer

A) contains as much solvent as it can hold. 
B) contains no double bonds. 
C) contains dissolved solute in equilibrium with undissolved solid. 
D) will rapidly precipitate if a seed crystal is added. 
E) none of the above 
A) contains as much solvent as it can hold. 
B) contains no double bonds. 
C) contains dissolved solute in equilibrium with undissolved solid. 
D) will rapidly precipitate if a seed crystal is added. 
E) none of the above

Question 14

Explain the difference between osmosis and dialysis.

Accepted Answer

Osmosis is when solvent molecu

Question 15

How many mL of 14.5 M NH3 are needed to prepare 2.00 L of a 1.00 M solution?

Accepted Answer

A) 138 mL 
B) 69.0 mL 
C) 276 mL 
D) 29.0 mL 
E) 7.25 mL 
A) 138 mL 
B) 69.0 mL 
C) 276 mL 
D) 29.0 mL 
E) 7.25 mL

Question 16

Match the following.
-hygroscopic

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 17

A 50.0 mL sample of a 6.0 M solution of HCl is diluted to 200.mL.What is the new concentration?

Accepted Answer

A) 24.0 M 
B) 6.0 M 
C) 2.10 M 
D) 2.00 M 
E) 1.50 M 
A) 24.0 M 
B) 6.0 M 
C) 2.10 M 
D) 2.00 M 
E) 1.50 M

Question 18

Which of the following has the least effect on the solubility of a solid in a liquid solvent?

Accepted Answer

A) temperature 
B) pressure 
C) nature of the solvent 
D) nature of the solute 
E) concentration of solute 
A) temperature 
B) pressure 
C) nature of the solvent 
D) nature of the solute 
E) concentration of solute

Question 19

Which procedure will produce 250 mL of a solution that is 4% by volume alcohol in water?

Accepted Answer

A) 4 mL of alcohol is mixed with enough water to make 250 mL of solution. 
B) 10 mL of alcohol is mixed with enough water to make 250 mL of solution. 
C) 4 mL of alcohol is mixed with 250 mL of water. 
D) 10 mL of alcohol is mixed with 250 mL of water. 
E) none of the above 
A) 4 mL of alcohol is mixed with enough water to make 250 mL of solution. 
B) 10 mL of alcohol is mixed with enough water to make 250 mL of solution. 
C) 4 mL of alcohol is mixed with 250 mL of water. 
D) 10 mL of alcohol is mixed with 250 mL of water. 
E) none of the above

Question 20

After swimming in the ocean for several hours,the swimmers noticed that their fingers appeared to be very wrinkled or shriveled up.This is an indication that seawater is ________ relative to the fluid in cells.

Accepted Answer

A)  isotonic 
B) hypertonic 
C) hypotonic 
D) none of these 
A)  isotonic 
B) hypertonic 
C) hypotonic 
D) none of these

Exam 9: Solutions

How many moles of HCl are present in 75.0 mL of a 0.200 M solution?

The exothermic step in the dissolution of NaCl in water is

Match the following. -crenation

Pressure has a large effect only on the solubility of ________ in liquids.

The number of components in a solution is

All of the water in a 0.200 M solution of NaCl was evaporated and 0.150 mole of NaCl was obtained.What was the original volume of the sample?

Which aqueous solution will have the lowest freezing point?

How many mL of water should be added to 50.0 mL of a 15.0 M H2SO4 solution to give a final concentration of 0.300 M?

Match the following. -strong electrolyte

If "A" contains 2% NaCl and is separated by a semipermeable membrane from "B" which contains 10% NaCl,which event will occur?

Match the following. -supersaturated

How many moles of solute are present in 12.0 L of 3.00 M HCl?

A supersaturated solution

Explain the difference between osmosis and dialysis.

How many mL of 14.5 M NH3 are needed to prepare 2.00 L of a 1.00 M solution?

Match the following. -hygroscopic

A 50.0 mL sample of a 6.0 M solution of HCl is diluted to 200.mL.What is the new concentration?

Which of the following has the least effect on the solubility of a solid in a liquid solvent?

Which procedure will produce 250 mL of a solution that is 4% by volume alcohol in water?

After swimming in the ocean for several hours,the swimmers noticed that their fingers appeared to be very wrinkled or shriveled up.This is an indication that seawater is ________ relative to the fluid in cells.

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

How many mL of water should be added to 50.0 mL of a 15.0 M H₂SO₄ solution to give a final concentration of 0.300 M?

How many mL of 14.5 M NH₃ are needed to prepare 2.00 L of a 1.00 M solution?