Question 1

Fluids used for an intravenous transfusion must be ________ with bodily fluids.

Accepted Answer

A)  isosmotic 
B)  hyperosmotic 
C)  hyposmotic 
D)  neosmotic 
E)  magnosmotic 
A)  isosmotic 
B)  hyperosmotic 
C)  hyposmotic 
D)  neosmotic 
E)  magnosmotic

Question 2

A solution containing more solute 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 3

Which of the following solutions will have the lowest freezing point?

Accepted Answer

A)  0.010 mol kg-1 K Br 
B)  0.010 mol kg-1 Na2CO3 
C)  0.035 mol kg-1 CH3CH2OH  
D)  0.015 mol kg-1 BaCl2 
A)  0.010 mol kg-1 K Br 
B)  0.010 mol kg-1 Na2CO3 
C)  0.035 mol kg-1 CH3CH2OH  
D)  0.015 mol kg-1 BaCl2

Question 4

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 5

A 150.0 mL sample of an aqueous solution at 25 °C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 Torr, what is the molar mass of the unknown compound?

Accepted Answer

A)  223 g mol-1 
B)  294 g mol-1 
C)  341 g mol-1 
D)  448 g mol-1 
E)  195 g mol-1 
A)  223 g mol-1 
B)  294 g mol-1 
C)  341 g mol-1 
D)  448 g mol-1 
E)  195 g mol-1

Question 6

Match the following.
-0.010 mol kg-1 Al(NO3)3

Accepted Answer

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

Question 7

Which of the following statements is generally TRUE?

Accepted Answer

A)  The solubility of a solid is not dependent on either temperature or pressure. 
B)  The solubility of a solid is highly dependent on pressure. 
C)  The solubility of a solid is highly dependent on both pressure and temperature. 
D)  The solubility of a solid is highly dependent on temperature. 
E)  None of the above 
A)  The solubility of a solid is not dependent on either temperature or pressure. 
B)  The solubility of a solid is highly dependent on pressure. 
C)  The solubility of a solid is highly dependent on both pressure and temperature. 
D)  The solubility of a solid is highly dependent on temperature. 
E)  None of the above

Question 8

Identify the solute with the lowest van't Hoff factor.

Accepted Answer

A)  nonelectrolyte 
B)  NaCl 
C)  MgSO4 
D)  MgCl2 
E)  FeCl3 
A)  nonelectrolyte 
B)  NaCl 
C)  MgSO4 
D)  MgCl2 
E)  FeCl3

Question 9

What volume of a 0.716 mol L-1 KBr solution is needed to provide 30.5 g of KBr?

Accepted Answer

A)  21.8 mL 
B)  42.7 mL 
C)  184 mL 
D)  357 mL 
A)  21.8 mL 
B)  42.7 mL 
C)  184 mL 
D)  357 mL

Question 10

What is the expected van't Hoff factor for MgCl2? (Assume dilute conditions)

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 11

The boiling point of an aqueous 1.83 mol kg-1 (NH4)2SO4 (molar mass = 132.15 g mol-1) solution is 102.5 °C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512 °C m-1.

Accepted Answer

A)  3.0 
B)  3.6 
C)  1.8 
D)  2.7 
E)  2.3 
A)  3.0 
B)  3.6 
C)  1.8 
D)  2.7 
E)  2.3

Question 12

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg-1 nonelectrolyte solution.

Accepted Answer

A)  CCl4, Kb = 29.9 °C m-1 
B)  C6H6, Kb = 5.12 °C m-1 
C)  CH3CH2OCH2CH3, Kb = 1.79 °C m-1 
D)  CH3CH2OH, Kb = 1.99 °C m-1 
E)  CHCl3, Kb = 4.70 °C m-1 
A)  CCl4, Kb = 29.9 °C m-1 
B)  C6H6, Kb = 5.12 °C m-1 
C)  CH3CH2OCH2CH3, Kb = 1.79 °C m-1 
D)  CH3CH2OH, Kb = 1.99 °C m-1 
E)  CHCl3, Kb = 4.70 °C m-1

Question 13

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 14

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 15

How many moles of KF are contained in 244 mL of 0.135 mol kg-1 KF solution? The density of the solution is 1.22 g mL-1.

Accepted Answer

A)  4.31 × 10-2 mol KF 
B)  4.02 × 10-2 mol KF 
C)  3.29 × 10-2 mol KF 
D)  2.32 × 10-2 mol KF 
E)  1.67 × 10-2 mol KF 
A)  4.31 × 10-2 mol KF 
B)  4.02 × 10-2 mol KF 
C)  3.29 × 10-2 mol KF 
D)  2.32 × 10-2 mol KF 
E)  1.67 × 10-2 mol KF

Question 16

A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g mL-1.

Accepted Answer

A)  52.3 ppm 
B)  13.2 ppm 
C)  12.7 ppm 
D)  25.3 ppm 
E)  36.5 ppm 
A)  52.3 ppm 
B)  13.2 ppm 
C)  12.7 ppm 
D)  25.3 ppm 
E)  36.5 ppm

Question 17

Which of the following defines dissolving?

Accepted Answer

A)  rate of dissolution = rate of deposition 
B)  rate of dissolution  rate of deposition 
D)  rate of bubbling > rate of dissolving 
E)  rate of evaporating > rate of condensing 
A)  rate of dissolution = rate of deposition 
B)  rate of dissolution  rate of deposition 
D)  rate of bubbling > rate of dissolving 
E)  rate of evaporating > rate of condensing

Question 18

A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25 °C. What is the vapour pressure of the solution if the vapour pressure of water at 25 °C is 23.76 mmHg?

Accepted Answer

A)  21.6 mmHg 
B)  22.7 mmHg 
C)  23.2 mmHg 
D)  24.9 mmHg 
A)  21.6 mmHg 
B)  22.7 mmHg 
C)  23.2 mmHg 
D)  24.9 mmHg

Question 19

What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?

Accepted Answer

A)  0. 34 
B)  0. 37 
C)  0. 25 
D)  0. 52 
A)  0. 34 
B)  0. 37 
C)  0. 25 
D)  0. 52

Question 20

A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

Accepted Answer

A)  6.04 × 10-3 
B)  1.65 × 10-2 
C)  1.40 × 10-3 
D)  1.32 × 10-2 
E)  8.84 × 10-2 
A)  6.04 × 10-3 
B)  1.65 × 10-2 
C)  1.40 × 10-3 
D)  1.32 × 10-2 
E)  8.84 × 10-2

Exam 12: Solutions

Fluids used for an intravenous transfusion must be ________ with bodily fluids.

A solution containing more solute than the equilibrium amount is called ________.

Which of the following solutions will have the lowest freezing point?

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.

A 150.0 mL sample of an aqueous solution at 25 °C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 Torr, what is the molar mass of the unknown compound?

Match the following. -0.010 mol kg-1 Al(NO3)3

Which of the following statements is generally TRUE?

Identify the solute with the lowest van't Hoff factor.

What volume of a 0.716 mol L-1 KBr solution is needed to provide 30.5 g of KBr?

What is the expected van't Hoff factor for MgCl2? (Assume dilute conditions)

The boiling point of an aqueous 1.83 mol kg-1 (NH4)2SO4 (molar mass = 132.15 g mol-1) solution is 102.5 °C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512 °C m-1.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg-1 nonelectrolyte 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.

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

How many moles of KF are contained in 244 mL of 0.135 mol kg-1 KF solution? The density of the solution is 1.22 g mL-1.

A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g mL-1.

Which of the following defines dissolving?

A KCl solution is prepared by dissolving 25.0 g KCl in 250.0 g of water at 25 °C. What is the vapour pressure of the solution if the vapour pressure of water at 25 °C is 23.76 mmHg?

What is the mole fraction of oxygen in a gas mixture that is 37% oxygen and 63% nitrogen by volume?

A solution is prepared by dissolving 76.3 g NaI in 545 g of water. Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

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Filters

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.

Match the following. -0.010 mol kg^-1 Al(NO₃)₃

What volume of a 0.716 mol L^-1 KBr solution is needed to provide 30.5 g of KBr?

What is the expected van't Hoff factor for MgCl₂? (Assume dilute conditions)

The boiling point of an aqueous 1.83 mol kg^-1 (NH₄)₂SO₄ (molar mass = 132.15 g mol^-1) solution is 102.5 °C. Determine the value of the van't Hoff factor for this solute if the K_b for water is 0.512 °C m^-1.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg^-1 nonelectrolyte 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.

How many moles of KF are contained in 244 mL of 0.135 mol kg^-1 KF solution? The density of the solution is 1.22 g mL^-1.

A 4.55 L sample of water contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g mL^-1.