Question 1

What is the freezing point of a 0.24 m solution of glucose,C6H12O6,in water? (Kfp for water is 1.858°C/m.)

Accepted Answer

A)  0.22°C 
B)  0.45°C 
C)  -0.45°C 
D)  -0.22°C 
E)  -0.89°C 
A)  0.22°C 
B)  0.45°C 
C)  -0.45°C 
D)  -0.22°C 
E)  -0.89°C

Question 2

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?

Accepted Answer

A)  0.124% 
B)  68.9% 
C)  1.69% 
D)  30.0% 
E)  0.322% 
A)  0.124% 
B)  68.9% 
C)  1.69% 
D)  30.0% 
E)  0.322%

Question 3

The vapor pressure of pure water at 15 S1U1P1$\circ$S1S1P0C is 12.8 mm Hg.What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH3CH2OH,molar mass = 46.07 g/mol)and 22.0 g water?

Accepted Answer

A)  2.84 mm Hg 
B)  5.61 mm Hg 
C)  7.19 mm Hg 
D)  10.0 mm Hg 
E)  12.8 mm Hg 
A)  2.84 mm Hg 
B)  5.61 mm Hg 
C)  7.19 mm Hg 
D)  10.0 mm Hg 
E)  12.8 mm Hg

Question 4

Aqueous colloidal solutions can be classified as ________ (water-fearing),or hydrophilic (water-loving).

Accepted Answer

The answer of Aqueous colloidal solutions can be classified as...

Question 5

A 12.0% sucrose solution by mass has a density of 1.05 g/cm3.What mass of sucrose is present in a 63.0-mL sample of this solution?

Accepted Answer

A)  7.94 g 
B)  7.20 g 
C)  0.126 g 
D)  551 g 
E)  7.56 g 
A)  7.94 g 
B)  7.20 g 
C)  0.126 g 
D)  551 g 
E)  7.56 g

Question 6

Calculate the molarity of a solution of magnesium chloride with a concentration of 30.3 mg/mL.

Accepted Answer

A)  0.159 M 
B)  3.14 M 
C)  0.636 M 
D)  0.507 M 
E)  0.318 M 
A)  0.159 M 
B)  3.14 M 
C)  0.636 M 
D)  0.507 M 
E)  0.318 M

Question 7

The following equation is known as ________ law:   
.

Accepted Answer

The answer of The following equation is known as ________...

Question 8

The osmotic pressure of blood is 7.65 atm at 37 S1U1P1$\circ$S1S1P0C.What mass of glucose (C6H12O6,molar mass = 180.2 g/mol)is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood.(R = 0.08206 L.atm/mol.K)

Accepted Answer

A)  0.676 g 
B)  0.698 g 
C)  5.67 g 
D)  122 g 
E)  1.02 $\times$ 103 g 
A)  0.676 g 
B)  0.698 g 
C)  5.67 g 
D)  122 g 
E)  1.02 $\times$ 103 g

Question 9

What is the definition of molality?

Accepted Answer

A)  moles of solute per kg of solvent 
B)  grams of solute per kg of solution 
C)  grams of solute per liter of solution 
D)  moles of solute per liter of solvent 
E)  moles of solute per liter of solution 
A)  moles of solute per kg of solvent 
B)  grams of solute per kg of solution 
C)  grams of solute per liter of solution 
D)  moles of solute per liter of solvent 
E)  moles of solute per liter of solution

Question 10

The volume of a 15.8% (by mass)solution is 146.4 mL.The density of the solution is 1.084 g/mL.What is the mass of solute in this solution?

Accepted Answer

A)  159 g 
B)  25.1 g 
C)  1004 g 
D)  21.3 g 
E)  134 g 
A)  159 g 
B)  25.1 g 
C)  1004 g 
D)  21.3 g 
E)  134 g

Question 11

What is the boiling-point $\underline{\text{ change }}$  for a solution containing 0.432 mol of naphthalene (a nonvolatile,nonionizing compound)in 250.g of liquid benzene? (Kbp = 2.53°C/m for benzene)

Accepted Answer

A)  4.37 °C 
B)  5.86 °C 
C)  0.273 °C 
D)  1.46 °C 
E)  1.093 °C 
A)  4.37 °C 
B)  5.86 °C 
C)  0.273 °C 
D)  1.46 °C 
E)  1.093 °C

Question 12

What mass of Zn(NO3)2 must be diluted to a mass of 1.00 kg with H2O to prepare 97 ppm Zn2+(aq)?

Accepted Answer

A)  7.8 $\times$ 10-6 g 
B)  7.8 $\times$ 10-3 g 
C)  3.3 $\times$ 10-2 g 
D)  1.3 $\times$ 10-1 g 
E)  2.8 $\times$ 10-1 g 
A)  7.8 $\times$ 10-6 g 
B)  7.8 $\times$ 10-3 g 
C)  3.3 $\times$ 10-2 g 
D)  1.3 $\times$ 10-1 g 
E)  2.8 $\times$ 10-1 g

Question 13

Which of the following statements concerning osmosis is/are CORRECT?
1)Osmosis involves the movement of ions through a semipermeable membrane until the charges on both sides of the membrane are equal.
2)Solvents move from regions of low solute concentration to regions of higher solute concentration.
3)Osmotic pressure is a colligative property.

Accepted Answer

A)  1 only 
B)  2 only 
C)  3 only 
D)  2 and 3 
E)  1,2,and 3 
A)  1 only 
B)  2 only 
C)  3 only 
D)  2 and 3 
E)  1,2,and 3

Question 14

Which of the following favor(s)the solubility of an ionic solid in a liquid solvent?

Accepted Answer

A)  a small magnitude of the lattice energy of the solute 
B)  a large magnitude of the solvation energy of the ions 
C)  a large polarity of the solvent 
D)  all of the above 
E)  none of the above 
A)  a small magnitude of the lattice energy of the solute 
B)  a large magnitude of the solvation energy of the ions 
C)  a large polarity of the solvent 
D)  all of the above 
E)  none of the above

Question 15

For the following gas-aqueous liquid equilibrium for a closed system at a constant temperature,
O2(g) $\leftrightarrows$O2(aq)
What is the effect on the equilibrium composition of the liquid when the $\underline{\text{  partial pressure }}$  of O2 gas above the liquid is decreased?

Accepted Answer

A)  The amount of O2 dissolved in the liquid decreases. 
B)  The amount of O2 dissolved in the liquid increases. 
C)  The amount of O2 dissolved in the liquid does not change. 
D)  Not enough information is provided to answer the question. 
E)  Either A or B is possible. 
A)  The amount of O2 dissolved in the liquid decreases. 
B)  The amount of O2 dissolved in the liquid increases. 
C)  The amount of O2 dissolved in the liquid does not change. 
D)  Not enough information is provided to answer the question. 
E)  Either A or B is possible.

Question 16

What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50S1U1P1$\circ$S1S1P0C? The freezing point depression constant,Kfp,of water is -1.86 S1U1P1$\circ$S1S1P0C/m.Assume the van't Hoff factor for Na2SO4 is 2.85.

Accepted Answer

A)  3.77 g 
B)  6.36 g 
C)  6.70 g 
D)  11.3 g 
E)  19.1 g 
A)  3.77 g 
B)  6.36 g 
C)  6.70 g 
D)  11.3 g 
E)  19.1 g

Question 17

What is the mole fraction of urea,CO(NH2)2, in a solution prepared by dissolving 6.8 g of urea in 33.5 g of methanol,CH3OH?

Accepted Answer

A)  0.83 
B)  0.17 
C)  0.098 
D)  0.90 
E)  0.28 
A)  0.83 
B)  0.17 
C)  0.098 
D)  0.90 
E)  0.28

Question 18

A 2.3-g sample of a small protein having a molecular weight of 62,000 g/mol is dissolved in 38.8 mL of water at 28°C.What is the osmotic pressure of the solution? (R = 0.0821 L · atm/K·mol; 1 atm = 760 mmHg)

Accepted Answer

A)  18 mmHg 
B)  1100 mmHg 
C)  1.7 mmHg 
D)  32,000 mmHg 
E)  0.024 mmHg 
A)  18 mmHg 
B)  1100 mmHg 
C)  1.7 mmHg 
D)  32,000 mmHg 
E)  0.024 mmHg

Question 19

What partial pressure of oxygen gas is required in order for 0.00392 g of the gas to dissolve in 23.7 mL of pure water? The Henry's law constant for oxygen gas is 1.3 $\times$ 10-3 M atm-1.

Accepted Answer

A)  2.2 $\times$ 10-7 atm 
B)  4.0 $\times$ 100 atm 
C)  1.6 $\times$ 10-7 atm 
D)  2.5 $\times$ 10-1 atm 
E)  4.2 $\times$ 10-2 atm 
A)  2.2 $\times$ 10-7 atm 
B)  4.0 $\times$ 100 atm 
C)  1.6 $\times$ 10-7 atm 
D)  2.5 $\times$ 10-1 atm 
E)  4.2 $\times$ 10-2 atm

Question 20

A concentrated hydrochloric acid solution has a density of 1.19 g/mL at 25°C and is 12.1 M.What is the percent by mass of HCl in the solution?

Accepted Answer

A)  37.1% HCl by mass 
B)  1.02% HCl by mass 
C)  0.980% HCl by mass 
D)  2.80% HCl by mass 
E)  30.6% HCl by mass 
A)  37.1% HCl by mass 
B)  1.02% HCl by mass 
C)  0.980% HCl by mass 
D)  2.80% HCl by mass 
E)  30.6% HCl by mass

Exam 14: Solutions and Their Behavior

What is the freezing point of a 0.24 m solution of glucose,C6H12O6,in water? (Kfp for water is 1.858°C/m.)

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?

The vapor pressure of pure water at 15 ∘\circ∘ C is 12.8 mm Hg.What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH3CH2OH,molar mass = 46.07 g/mol)and 22.0 g water?

Aqueous colloidal solutions can be classified as ________ (water-fearing),or hydrophilic (water-loving).

A 12.0% sucrose solution by mass has a density of 1.05 g/cm3.What mass of sucrose is present in a 63.0-mL sample of this solution?

Calculate the molarity of a solution of magnesium chloride with a concentration of 30.3 mg/mL.

The following equation is known as ________ law: .

The osmotic pressure of blood is 7.65 atm at 37 ∘\circ∘ C.What mass of glucose (C6H12O6,molar mass = 180.2 g/mol)is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood.(R = 0.08206 L.atm/mol.K)

What is the definition of molality?

The volume of a 15.8% (by mass)solution is 146.4 mL.The density of the solution is 1.084 g/mL.What is the mass of solute in this solution?

What is the boiling-point change ‾\underline{\text{ change }} change ​ for a solution containing 0.432 mol of naphthalene (a nonvolatile,nonionizing compound)in 250.g of liquid benzene? (Kbp = 2.53°C/m for benzene)

What mass of Zn(NO3)2 must be diluted to a mass of 1.00 kg with H2O to prepare 97 ppm Zn2+(aq)?

Which of the following favor(s)the solubility of an ionic solid in a liquid solvent?

What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing point by 2.50 ∘\circ∘ C? The freezing point depression constant,Kfp,of water is -1.86 ∘\circ∘ C/m.Assume the van't Hoff factor for Na2SO4 is 2.85.

What is the mole fraction of urea,CO(NH2)2, in a solution prepared by dissolving 6.8 g of urea in 33.5 g of methanol,CH3OH?

A 2.3-g sample of a small protein having a molecular weight of 62,000 g/mol is dissolved in 38.8 mL of water at 28°C.What is the osmotic pressure of the solution? (R = 0.0821 L · atm/K·mol; 1 atm = 760 mmHg)

What partial pressure of oxygen gas is required in order for 0.00392 g of the gas to dissolve in 23.7 mL of pure water? The Henry's law constant for oxygen gas is 1.3 ×\times× 10-3 M atm-1.

A concentrated hydrochloric acid solution has a density of 1.19 g/mL at 25°C and is 12.1 M.What is the percent by mass of HCl in the solution?

Basic Concepts of Chemistry

Mathlets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Chemistry of Solids

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

The Chemistry of Acids and Bases

Principles of Reactivity: Other Aspects of Aqueous Equilibria

Entropy and Free Energy

Principles of Reactivity: Electron Transfer Reactions

Environmental Chemistry Earths Environment,energy,and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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What is the freezing point of a 0.24 m solution of glucose,C₆H₁₂O₆,in water? (K_fp for water is 1.858°C/m.)

The vapor pressure of pure water at 15 ^$\circ$C is 12.8 mm Hg.What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH₃CH₂OH,molar mass = 46.07 g/mol)and 22.0 g water?

A 12.0% sucrose solution by mass has a density of 1.05 g/cm³.What mass of sucrose is present in a 63.0-mL sample of this solution?

The osmotic pressure of blood is 7.65 atm at 37 ^$\circ$C.What mass of glucose (C₆H₁₂O₆,molar mass = 180.2 g/mol)is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood.(R = 0.08206 L.atm/mol.K)

What is the boiling-point $\underline{\text{ change }}$ for a solution containing 0.432 mol of naphthalene (a nonvolatile,nonionizing compound)in 250.g of liquid benzene? (K_bp = 2.53°C/m for benzene)

What mass of Zn(NO₃)₂ must be diluted to a mass of 1.00 kg with H₂O to prepare 97 ppm Zn²⁺(aq)?

What mass of Na₂SO₄ must be dissolved in 100.0 grams of water to lower the freezing point by 2.50^$\circ$C? The freezing point depression constant,K_fp,of water is -1.86 ^$\circ$C/m.Assume the van't Hoff factor for Na₂SO₄ is 2.85.

What is the mole fraction of urea,CO(NH₂)₂,in a solution prepared by dissolving 6.8 g of urea in 33.5 g of methanol,CH₃OH?

What partial pressure of oxygen gas is required in order for 0.00392 g of the gas to dissolve in 23.7 mL of pure water? The Henry's law constant for oxygen gas is 1.3 $\times$ 10^-3 M atm^-1.