Question 1

Define the Tyndall effect.

Accepted Answer

The Tyndall effect i

Question 2

Which of the following statements is TRUE?

Accepted Answer

A) In general, the solubility of a solid in water decreases with increasing temperature. 
B) In general, the solubility of a gas in water decreases with increasing temperature. 
C) The solubility of a gas in water usually increases with decreasing pressure. 
D) The solubility of an ionic solid in water decreases with increasing temperature. 
E) None of the above statements is true. 
A) In general, the solubility of a solid in water decreases with increasing temperature. 
B) In general, the solubility of a gas in water decreases with increasing temperature. 
C) The solubility of a gas in water usually increases with decreasing pressure. 
D) The solubility of an ionic solid in water decreases with increasing temperature. 
E) None of the above statements is true.

Question 3

A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions. Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g mL-1.

Accepted Answer

A) 2.8 ppm 
B) 7.2 ppm 
C) 3.6 ppm 
D) 1.8 ppm 
E) 5.4 ppm 
A) 2.8 ppm 
B) 7.2 ppm 
C) 3.6 ppm 
D) 1.8 ppm 
E) 5.4 ppm

Question 4

How many moles of KF are contained in 347 g of water in a 0.175 mol kg-1 KF solution?

Accepted Answer

A) 1.65 × 10-2 mol KF 
B) 5.04 × 10-2 mol KF 
C) 6.07 × 10-2 mol KF 
D) 3.22 × 10-2 mol KF 
E) 1.98 × 10-2 mol KF 
A) 1.65 × 10-2 mol KF 
B) 5.04 × 10-2 mol KF 
C) 6.07 × 10-2 mol KF 
D) 3.22 × 10-2 mol KF 
E) 1.98 × 10-2 mol KF

Question 5

Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3 g of sucrose, C12H22O11, at a temperature of 25.0 °C. The vapour pressure of pure water at 25 °C is 31.7 mbar, the density of water is 1.00 g mL-1, and assume no change in volume occurs upon dissolution.

Accepted Answer

A) 204 mL 
B) 31.8 mL 
C) 286 mL 
D) 323 mL 
E) 516 mL 
A) 204 mL 
B) 31.8 mL 
C) 286 mL 
D) 323 mL 
E) 516 mL

Question 6

A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is ________ molal.

Accepted Answer

A) 1.61 × 10-3 
B) 622 
C) 0.622 
D) 1.27 × 103 
E) 1.61 
A) 1.61 × 10-3 
B) 622 
C) 0.622 
D) 1.27 × 103 
E) 1.61

Question 7

A solution containing less than the equilibrium amount is called

Accepted Answer

A) an unsaturated solution. 
B) a dilute solution. 
C) a supersaturated solution. 
D) a concentrated solution. 
E) a saturated solution. 
A) an unsaturated solution. 
B) a dilute solution. 
C) a supersaturated solution. 
D) a concentrated solution. 
E) a saturated solution.

Question 8

Calculate the solution temperature required to produce an osmotic pressure of 1.18 mbar using 3.72 mg of a protein with a molar mass of 4176 g mol-1 that is dissolved in enough water to create 20.9 mL of solution.

Accepted Answer

A) 333 K 
B) 298 K 
C) 316 K 
D) 351 K 
E) 288 K 
A) 333 K 
B) 298 K 
C) 316 K 
D) 351 K 
E) 288 K

Question 9

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C6H12O6, has a vapour pressure of 545.0 mbar.

Accepted Answer

A) 531 mbar 
B) 578 mbar 
C) 508 mbar 
D) 599 mbar 
E) 520 mbar 
A) 531 mbar 
B) 578 mbar 
C) 508 mbar 
D) 599 mbar 
E) 520 mbar

Question 10

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11)in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Accepted Answer

A) 4.09 × 10-3 
B) 7.80 × 10-2 
C) 1.28 × 10-3 
D) 7.23 × 10-2 
E) 2.45 × 10-3 
A) 4.09 × 10-3 
B) 7.80 × 10-2 
C) 1.28 × 10-3 
D) 7.23 × 10-2 
E) 2.45 × 10-3

Question 11

Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?

Accepted Answer

A) trimethylamine (N(CH3)3) 
B) acetone (CH3COCH3) 
C) ethylene glycol (HOCH2CH2OH) 
D) hexane (CH3CH2CH2CH2CH2CH3) 
E) None of these compounds should be soluble in ethanol. 
A) trimethylamine (N(CH3)3) 
B) acetone (CH3COCH3) 
C) ethylene glycol (HOCH2CH2OH) 
D) hexane (CH3CH2CH2CH2CH2CH3) 
E) None of these compounds should be soluble in ethanol.

Question 12

What is the term for the amount of solute in moles per litre of solution?

Accepted Answer

A) molality 
B) molarity 
C) mole fraction 
D) mole percent 
E) mass percent 
A) molality 
B) molarity 
C) mole fraction 
D) mole percent 
E) mass percent

Question 13

An aqueous solution has a normal boiling point of 103.0 °C. What is the freezing point of this solution? For water Kb = 0.51 °C m-1 and Kf = 1.86 °C m-1.

Accepted Answer

A) -0.82 °C 
B) -3.0 °C 
C) -3.6 °C 
D) -11 °C 
A) -0.82 °C 
B) -3.0 °C 
C) -3.6 °C 
D) -11 °C

Question 14

How much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?

Accepted Answer

A) 54.0 g 
B) 74.2 g 
C) 87.5 g 
D) 114 g 
A) 54.0 g 
B) 74.2 g 
C) 87.5 g 
D) 114 g

Question 15

Calculate the total solution volume required to produce an osmotic pressure of 6.39 mbar using 12.34 mg of a protein with a molar mass of 5309 g mol-1 at 25.0 °C.

Accepted Answer

A) 12.5 mL 
B) 11.8 mL 
C) 9.91 mL 
D) 8.37 mL 
E) 9.02 mL 
A) 12.5 mL 
B) 11.8 mL 
C) 9.91 mL 
D) 8.37 mL 
E) 9.02 mL

Question 16

Match the following.

-0.050 mol kg-1 NaCl

Accepted Answer

A) largest van't Hoff factor 
B) solution that is most strongly dependent upon pressure 
C) solution of ionic compound with highest freezing point. 
D) highest boiling point 
E) solution with ΔTb = 0.026 °C 
A) largest van't Hoff factor 
B) solution that is most strongly dependent upon pressure 
C) solution of ionic compound with highest freezing point. 
D) highest boiling point 
E) solution with ΔTb = 0.026 °C

Question 17

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

Accepted Answer

The vapour pressure of the solution will

Question 18

Which cation in each set is expected to have the larger (more negative)hydration energy? I Be2+ or Ca2+
II Rb+ or Zn2+

Accepted Answer

A) Be2+ in set I and Rb+ in set II 
B) Be2+ in set I and Zn2+ in set II 
C) Ca2+ in set I and Rb+ in set II 
D) Ca2+ in set I and Zn2+ in set II 
A) Be2+ in set I and Rb+ in set II 
B) Be2+ in set I and Zn2+ in set II 
C) Ca2+ in set I and Rb+ in set II 
D) Ca2+ in set I and Zn2+ in set II

Question 19

What mass of ethane (CH3CH3)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL-1.

Accepted Answer

A) 2.35 g 
B) 8.49 g 
C) 11.8 g 
D) 6.95 g 
E) 4.25 g 
A) 2.35 g 
B) 8.49 g 
C) 11.8 g 
D) 6.95 g 
E) 4.25 g

Exam 12: Solutions

Define the Tyndall effect.

Which of the following statements is TRUE?

A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions. Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g mL-1.

How many moles of KF are contained in 347 g of water in a 0.175 mol kg-1 KF solution?

Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3 g of sucrose, C12H22O11, at a temperature of 25.0 °C. The vapour pressure of pure water at 25 °C is 31.7 mbar, the density of water is 1.00 g mL-1, and assume no change in volume occurs upon dissolution.

A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is ________ molal.

A solution containing less than the equilibrium amount is called

Calculate the solution temperature required to produce an osmotic pressure of 1.18 mbar using 3.72 mg of a protein with a molar mass of 4176 g mol-1 that is dissolved in enough water to create 20.9 mL of solution.

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C6H12O6, has a vapour pressure of 545.0 mbar.

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11)in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Which of the following compounds will be most soluble in ethanol (CH3CH2OH)?

What is the term for the amount of solute in moles per litre of solution?

An aqueous solution has a normal boiling point of 103.0 °C. What is the freezing point of this solution? For water Kb = 0.51 °C m-1 and Kf = 1.86 °C m-1.

How much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?

Calculate the total solution volume required to produce an osmotic pressure of 6.39 mbar using 12.34 mg of a protein with a molar mass of 5309 g mol-1 at 25.0 °C.

Match the following. -0.050 mol kg-1 NaCl

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

Which cation in each set is expected to have the larger (more negative)hydration energy? I Be2+ or Ca2+ II Rb+ or Zn2+

What mass of ethane (CH3CH3)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL-1.

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A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions. Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g mL^-1.

How many moles of KF are contained in 347 g of water in a 0.175 mol kg^-1 KF solution?

Calculate the solution temperature required to produce an osmotic pressure of 1.18 mbar using 3.72 mg of a protein with a molar mass of 4176 g mol^-1 that is dissolved in enough water to create 20.9 mL of solution.

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C₆H₁₂O₆, has a vapour pressure of 545.0 mbar.

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁)in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Which of the following compounds will be most soluble in ethanol (CH₃CH₂OH)?

An aqueous solution has a normal boiling point of 103.0 °C. What is the freezing point of this solution? For water K_b = 0.51 °C m^-1and K_f = 1.86 °C m^-1.

How much water must be added to 40.0 g of CaCl₂ to produce a solution that is 35.0 wt% CaCl₂?

Calculate the total solution volume required to produce an osmotic pressure of 6.39 mbar using 12.34 mg of a protein with a molar mass of 5309 g mol^-1 at 25.0 °C.

Match the following. -0.050 mol kg^-1 NaCl

Which cation in each set is expected to have the larger (more negative)hydration energy? I Be²⁺ or Ca²⁺ II Rb⁺ or Zn²⁺

What mass of ethane (CH₃CH₃)is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL^-1.