Question 1

A saturated solution is defined as

Accepted Answer

A) a concentrated solution. 
B) a solution that is in equilibrium with pure solute. 
C) a solution than is in equilibrium with undissolved solute. 
D) a solution that is not in equilibrium with both pure solvent and undissolved solute. 
A) a concentrated solution. 
B) a solution that is in equilibrium with pure solute. 
C) a solution than is in equilibrium with undissolved solute. 
D) a solution that is not in equilibrium with both pure solvent and undissolved solute.

Question 2

Sodium hydroxide is available commercially as a 50.0% by weight aqueous solution.Calculate the molality of this sodium hydroxide solution.

Accepted Answer

A) 0.450 m 
B) 19.1 m 
C) 25.0 m 
D) 125.m 
A) 0.450 m 
B) 19.1 m 
C) 25.0 m 
D) 125.m

Question 3

Although there are exceptions,which is most likely to be true for the dissolving of a solid in a liquid?

Accepted Answer

A) ΔHsoln is positive. 
B) ΔHsoln is negative. 
C) ΔSsoln is positive. 
D) ΔSsoln is negative. 
A) ΔHsoln is positive. 
B) ΔHsoln is negative. 
C) ΔSsoln is positive. 
D) ΔSsoln is negative.

Question 4

Freezing point depression,boiling point elevation,vapor pressure lowering,and osmotic pressure are examples of ________ properties,which depend on the amount but not the chemical identity of dissolved particles.

Accepted Answer

The answer of Freezing point depression,boiling point elevation,vapor pressure lowering,and...

Question 5

How will the osmotic pressure of an aqueous solution change as evaporation occurs?

Accepted Answer

A) The osmotic pressure will increase. 
B) The osmotic pressure will not change. 
C) The osmotic pressure will decrease. 
D) The osmotic pressure will increase or decrease until it equals the vapor pressure of water. 
A) The osmotic pressure will increase. 
B) The osmotic pressure will not change. 
C) The osmotic pressure will decrease. 
D) The osmotic pressure will increase or decrease until it equals the vapor pressure of water.

Question 6

A solution is prepared by dissolving 171 g of CdCl2 in enough water to make 250.0 mL of solution.If the density of the solution is 1.556 g/mL,what is the molarity of the solution?

Accepted Answer

A) 0.440 M 
B) 0.684 M 
C) 0.933 M 
D) 3.73 M 
A) 0.440 M 
B) 0.684 M 
C) 0.933 M 
D) 3.73 M

Question 7

Which ion-dipole interaction results in the larger (more negative)hydration energy?

Accepted Answer

A) diagram (a) 
B) diagram (b) 
C) diagram (c) 
D) diagram (d) 
A) diagram (a) 
B) diagram (b) 
C) diagram (c) 
D) diagram (d)

Question 8

Arrows in the energy diagram below represent enthalpy changes occurring in the endothermic formation of a solution:
ΔHS1U1B1solnS1U1B0 = enthalpy of solution
ΔHS1U1B1solute-soluteS1U1B0 = enthalpy change involving solute-solute interactions
ΔHS1U1B1solute-solventS1U1B0 = enthalpy change involving solute-solvent interactions
ΔHS1U1B1solvent-solventS1U1B0 = enthalpy change involving solvent-solvent interactions  
-Which arrow represents ΔHsoln?

Accepted Answer

A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d) 
A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d)

Question 9

How much water must be added to 36.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?

Accepted Answer

A) 48.6 g 
B) 66.9 g 
C) 97.2 g 
D) 103 g 
A) 48.6 g 
B) 66.9 g 
C) 97.2 g 
D) 103 g

Question 10

Drawings (1)and (2)show the equilibrium vapor pressures of two pure liquids.Which drawing (3)-(6)represents the equilibrium vapor pressure of a solution made by mixing equal moles of each liquid?

Accepted Answer

A) drawing (3) 
B) drawing (4) 
C) drawing (5) 
D) drawing (6) 
A) drawing (3) 
B) drawing (4) 
C) drawing (5) 
D) drawing (6)

Question 11

-What is the approximate boiling temperature of a mixture that is 0.70 XA and 0.30 XB?

Accepted Answer

A) 50°C 
B) 75°C 
C) 95°C 
D) 100°C 
A) 50°C 
B) 75°C 
C) 95°C 
D) 100°C

Question 12

A person is considered legally intoxicated with a blood alcohol level of 80 mg/dL.Assuming that blood plasma has a density of 1.025 g/mL,what is this concentration expressed in parts per million?

Accepted Answer

The answer of A person is considered legally intoxicated with...

Question 13

Calculate the freezing point of a solution when 370 grams of Ca3(PO4)is added to 3000mL of water.(density of water is 1.00 g/mL).The Kf for water is 1.86°C/m and normal freezing point of water is 0.00°C.

Accepted Answer

A) -0.74 
B) -0.0030 
C) -3.70 
D) -1.27 
A) -0.74 
B) -0.0030 
C) -3.70 
D) -1.27

Question 14

Which of the following should most favor the solubility of an ionic solid in water?

Accepted Answer

A) a low lattice energy for the solid and a low hydration energy for its ions 
B) a low lattice energy for the solid and a high hydration energy for its ions 
C) a high lattice energy for the solid and a low hydration energy for its ions 
D) a high lattice energy for the solid and a high hydration energy for its ions 
A) a low lattice energy for the solid and a low hydration energy for its ions 
B) a low lattice energy for the solid and a high hydration energy for its ions 
C) a high lattice energy for the solid and a low hydration energy for its ions 
D) a high lattice energy for the solid and a high hydration energy for its ions

Question 15

A solution is prepared by dissolving 17.75 g sulfuric acid,H2SO4,in enough water to make exactly 100.0 mL of solution.If the density of the solution is 1.1094 g/mL,what is the weight % H2SO4 in the solution?

Accepted Answer

A) 16.00% 
B) 18.00% 
C) 19.00% 
D) 84.00% 
A) 16.00% 
B) 18.00% 
C) 19.00% 
D) 84.00%

Question 16

Which cation in each set is expected to have the larger (more negative)hydration energy? I.Li+ or Na+
II.Rb+ or Cu2+

Accepted Answer

A) Li+ in set I and Rb+ in set II 
B) Li+ in set I and Cu2+ in set II 
C) Na+ in set I and Rb+ in set II 
D) Na+ in set I and Cu2+ in set II 
A) Li+ in set I and Rb+ in set II 
B) Li+ in set I and Cu2+ in set II 
C) Na+ in set I and Rb+ in set II 
D) Na+ in set I and Cu2+ in set II

Question 17

What is the mole fraction of I2 in a solution made by dissolving 139 g of I2 in 245 g of hexane,C6H14?

Accepted Answer

A) 0.161 
B) 0.193 
C) 0.278 
D) 0.385 
A) 0.161 
B) 0.193 
C) 0.278 
D) 0.385

Question 18

When solute is added to water,the solution has a ________ freezing point than that of pure ice at 0˚C.

Accepted Answer

The answer of When solute is added to water,the solution...

Question 19

-Which drawing above represents the system with the lowest entropy?

Accepted Answer

A) drawing (a) 
B) drawing (b) 
C) drawing (c) 
D) drawing (d) 
A) drawing (a) 
B) drawing (b) 
C) drawing (c) 
D) drawing (d)

Question 20

Arrows in the energy diagram below represent enthalpy changes occurring in the exothermic formation of a solution:
ΔHS1U1B1solnS1U1B0 = enthalpy of solution
ΔHsolute-solute = enthalpy change involving solute-solute interactions
ΔHsolute-solvent = enthalpy change involving solute-solvent interactions
ΔHsolvent-solvent = enthalpy change involving solvent-solvent interactions  
-Which arrow represents ΔHsoln?

Accepted Answer

A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d) 
A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d)

Exam 12: Solutions and Their Properties

A saturated solution is defined as

Sodium hydroxide is available commercially as a 50.0% by weight aqueous solution.Calculate the molality of this sodium hydroxide solution.

Although there are exceptions,which is most likely to be true for the dissolving of a solid in a liquid?

Freezing point depression,boiling point elevation,vapor pressure lowering,and osmotic pressure are examples of ________ properties,which depend on the amount but not the chemical identity of dissolved particles.

How will the osmotic pressure of an aqueous solution change as evaporation occurs?

A solution is prepared by dissolving 171 g of CdCl2 in enough water to make 250.0 mL of solution.If the density of the solution is 1.556 g/mL,what is the molarity of the solution?

Which ion-dipole interaction results in the larger (more negative)hydration energy?

How much water must be added to 36.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?

Drawings (1)and (2)show the equilibrium vapor pressures of two pure liquids.Which drawing (3)-(6)represents the equilibrium vapor pressure of a solution made by mixing equal moles of each liquid?

-What is the approximate boiling temperature of a mixture that is 0.70 XA and 0.30 XB?

A person is considered legally intoxicated with a blood alcohol level of 80 mg/dL.Assuming that blood plasma has a density of 1.025 g/mL,what is this concentration expressed in parts per million?

Calculate the freezing point of a solution when 370 grams of Ca3(PO4)is added to 3000mL of water.(density of water is 1.00 g/mL).The Kf for water is 1.86°C/m and normal freezing point of water is 0.00°C.

Which of the following should most favor the solubility of an ionic solid in water?

A solution is prepared by dissolving 17.75 g sulfuric acid,H2SO4,in enough water to make exactly 100.0 mL of solution.If the density of the solution is 1.1094 g/mL,what is the weight % H2SO4 in the solution?

Which cation in each set is expected to have the larger (more negative)hydration energy? I.Li+ or Na+ II.Rb+ or Cu2+

What is the mole fraction of I2 in a solution made by dissolving 139 g of I2 in 245 g of hexane,C6H14?

When solute is added to water,the solution has a ________ freezing point than that of pure ice at 0˚C.

-Which drawing above represents the system with the lowest entropy?

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A solution is prepared by dissolving 171 g of CdCl₂ in enough water to make 250.0 mL of solution.If the density of the solution is 1.556 g/mL,what is the molarity of the solution?

How much water must be added to 36.0 g of CaCl₂ to produce a solution that is 35.0 wt% CaCl₂?

-What is the approximate boiling temperature of a mixture that is 0.70 X_A and 0.30 X_B?

Calculate the freezing point of a solution when 370 grams of Ca₃(PO₄)is added to 3000mL of water.(density of water is 1.00 g/mL).The K_f for water is 1.86°C/m and normal freezing point of water is 0.00°C.

A solution is prepared by dissolving 17.75 g sulfuric acid,H₂SO₄,in enough water to make exactly 100.0 mL of solution.If the density of the solution is 1.1094 g/mL,what is the weight % H₂SO₄ in the solution?

Which cation in each set is expected to have the larger (more negative)hydration energy? I.Li⁺ or Na⁺ II.Rb⁺ or Cu²⁺

What is the mole fraction of I₂ in a solution made by dissolving 139 g of I₂ in 245 g of hexane,C₆H₁₄?