Question 1

Osmotic pressure is

Accepted Answer

A) inversely proportional to mass fraction. 
B) directly proportional to lattice energy. 
C) inversely proportional to molality. 
D) inversely proportional to mole fraction. 
E) directly proportional to molarity. 
A) inversely proportional to mass fraction. 
B) directly proportional to lattice energy. 
C) inversely proportional to molality. 
D) inversely proportional to mole fraction. 
E) directly proportional to molarity.

Question 2

What is the mole fraction of urea,CH4N2O,in an aqueous solution that is 37% urea by mass?

Accepted Answer

A) 0.15 
B) 0.85 
C) 0.37 
D) 0.54 
E) 0.66 
A) 0.15 
B) 0.85 
C) 0.37 
D) 0.54 
E) 0.66

Question 3

What is the molar mass of an aromatic hydrocarbon if 0.75 g of the compound depresses the freezing point of 123 g of benzene by 0.28°C? (Kf for benzene is 5.12°C/m.)

Accepted Answer

A) 43 g/mol 
B) 150 g/mol 
C) 110.00 g/mol 110 
D) 2900 g/mol 
E) 140 g/mol 
A) 43 g/mol 
B) 150 g/mol 
C) 110.00 g/mol 110 
D) 2900 g/mol 
E) 140 g/mol

Question 4

The volume of a 24.0% (by mass)solution is 65.2 mL.The density of the solution is 1.072 g/mL.What is the mass of the solution?

Accepted Answer

A) 69.8 g 
B) 61 g 
C) 1670 g 
D) 167 g 
E) 17 g 
A) 69.8 g 
B) 61 g 
C) 1670 g 
D) 167 g 
E) 17 g

Question 5

Which way of expressing concentration is used to relate the vapor pressure of a solution to the amount of nonvolatile solute dissolved in the solution?

Accepted Answer

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

Question 6

What mass of a 29.0% by mass glucose,C6H12O6,solution contains 60.0 g of glucose?

Accepted Answer

A) 52.2 g 
B) 207 g 
C) 17.4 g 
D) 96.7 g 
E) 60.0 g 
A) 52.2 g 
B) 207 g 
C) 17.4 g 
D) 96.7 g 
E) 60.0 g

Question 7

What is the molality of ethanol,C2H5OH,in an aqueous solution that is 36.4% ethanol by mass?

Accepted Answer

A) 1 m 
B) 0 m 
C) 12 m 
D) 19 m 
E) 97 m 
A) 1 m 
B) 0 m 
C) 12 m 
D) 19 m 
E) 97 m

Question 8

Thyroxine,an important hormone that controls the rate of metabolism in the body,can be isolated from the thyroid gland.If 0.454 g of thyroxine is dissolved in 10.0 g of benzene,the freezing point of the solution could be measured as 5.144°C.Pure benzene freezes at 5.444°C and has a value for the molal freezing-point-depression constant of Kf of 5.12°C/m.What is the approximate molar mass of thyroxine?

Accepted Answer

A) 775 g/mol 
B) 7.75 g/mol 
C) 7.75 × 105 g/mol 
D) 42.7 g/mol 
E) 11.3 g/mol 
A) 775 g/mol 
B) 7.75 g/mol 
C) 7.75 × 105 g/mol 
D) 42.7 g/mol 
E) 11.3 g/mol

Question 9

A 2.2-g sample of a small protein having a molecular weight of 42,000 g/mol is dissolved in 31.2 mL of water at 28°C.What is the osmotic pressure of the solution? (R = 0.0821 L · atm/(K · mol))

Accepted Answer

A) 32 mmHg 
B) 1300 mmHg 
C) 2.9 mmHg 
D) 18,000 mmHg 
E) 0.041 mmHg 
A) 32 mmHg 
B) 1300 mmHg 
C) 2.9 mmHg 
D) 18,000 mmHg 
E) 0.041 mmHg

Question 10

Based on the formulas of the following solutes,which compound would have the smallest van't Hoff factor (i)?

Accepted Answer

A) Ca(NO3)2(aq) 
B) K2SO4(aq) 
C) Th(SO4)2(aq) 
D) Al2(SO4)3(aq) 
E) MgSO4(aq) 
A) Ca(NO3)2(aq) 
B) K2SO4(aq) 
C) Th(SO4)2(aq) 
D) Al2(SO4)3(aq) 
E) MgSO4(aq)

Question 11

As the number of solute particles in a given volume of solution increases,

Accepted Answer

A) the boiling point will increase and the vapor pressure will increase. 
B) the freezing point will decrease and the vapor pressure will decrease. 
C) the freezing point will increase and the vapor pressure will increase. 
D) the boiling point will decrease and the vapor pressure will decrease. 
E) the osmotic pressure will decrease and the lattice energy will increase. 
A) the boiling point will increase and the vapor pressure will increase. 
B) the freezing point will decrease and the vapor pressure will decrease. 
C) the freezing point will increase and the vapor pressure will increase. 
D) the boiling point will decrease and the vapor pressure will decrease. 
E) the osmotic pressure will decrease and the lattice energy will increase.

Question 12

What is the mass percent of ethylene glycol (HOCH2CH2OH)in a solution of ethylene glycol in water that has a freezing point of -17.8°C? (Kf for water is 1.858°C/m.)

Accepted Answer

A) 99.8% 
B) 37.2% 
C) 59.4% 
D) 64.7% 
E) 9.58% 
A) 99.8% 
B) 37.2% 
C) 59.4% 
D) 64.7% 
E) 9.58%

Question 13

According to _____,the partial pressure of solvent,,over a solution equals the vapor pressure of the pure solvent,   ,times the mole fraction of solvent,  
,in the solution.

Accepted Answer

A) ​Raoult's law 
B) Benford's law 
C) ​Dermott's law 
D) ​Leibniz's law 
E) ​Zipf's law 
A) ​Raoult's law 
B) Benford's law 
C) ​Dermott's law 
D) ​Leibniz's law 
E) ​Zipf's law

Question 14

What is the mass of H2SO4 in a 38.2-cm3 sample of concentrated sulfuric acid that has a density of 1.84 g/cm3 and consists of 98.3% H2SO4?

Accepted Answer

A) 37.6 g 
B) 69.1 g 
C) 4.73 g 
D) 1.81 g 
E) 20.4 g 
A) 37.6 g 
B) 69.1 g 
C) 4.73 g 
D) 1.81 g 
E) 20.4 g

Question 15

The volume of a 34.6% (by mass)solution is 129.0 mL.The density of the solution is 1.116 g/mL.What is the mass of solute in this solution?

Accepted Answer

A) 144 g 
B) 49.8 g 
C) 416 g 
D) 40.0 g 
E) 94 g 
A) 144 g 
B) 49.8 g 
C) 416 g 
D) 40.0 g 
E) 94 g

Question 16

For which of the following aqueous solutions would one expect to have the largest van't Hoff factor (i)?

Accepted Answer

A) 0.500 m K2SO4 
B) 0.500 m NaCl 
C) 0.500 m C6H12O6 (glucose) 
D) 0.050 m K2SO4 
E) 0.050 m NaCl 
A) 0.500 m K2SO4 
B) 0.500 m NaCl 
C) 0.500 m C6H12O6 (glucose) 
D) 0.050 m K2SO4 
E) 0.050 m NaCl

Question 17

Henry's Law constant is 0.034 mol/kg⋅bar and 0.0013 mol/kg⋅bar for CO2 and O2 respectively at 25°C.What pressure of O2 is required to achieve the same solubility as 0.368 bar of CO2?

Accepted Answer

A) 9.6 bar 
B) 0.0 bar 
C)    bar 
D)    bar 
E) 0.1 bar 
A) 9.6 bar 
B) 0.0 bar 
C)    bar 
D)    bar 
E) 0.1 bar

Question 18

For a solution containing only one solute dissolved in a solvent,we can calculate the mole fraction of the solvent directly,given only

Accepted Answer

A) the molar mass of the solute. 
B) the density of the solution. 
C) the molar mass of the solvent. 
D) the mole fraction of the solute. 
E) the molarity of the solution. 
A) the molar mass of the solute. 
B) the density of the solution. 
C) the molar mass of the solvent. 
D) the mole fraction of the solute. 
E) the molarity of the solution.

Question 19

Fluids that mix with or dissolve in each other in all proportions are said to be _____.

Accepted Answer

A) ​immiscible fluids 
B) ​miscible fluids 
C) ​heterogeneous fluids 
D) ​divergent fluids 
E) ​suspension fluids 
A) ​immiscible fluids 
B) ​miscible fluids 
C) ​heterogeneous fluids 
D) ​divergent fluids 
E) ​suspension fluids

Question 20

Which of the following compounds is least soluble in water?

Accepted Answer

A) CH3CH2CH2NH2 
B) CH3CH2CH2F 
C) CH3CH(OH)CH3 
D) CH3CH2COOH 
E) CH3CH2NHCH3 
A) CH3CH2CH2NH2 
B) CH3CH2CH2F 
C) CH3CH(OH)CH3 
D) CH3CH2COOH 
E) CH3CH2NHCH3

Exam 12: Solutions

Osmotic pressure is

What is the mole fraction of urea,CH4N2O,in an aqueous solution that is 37% urea by mass?

What is the molar mass of an aromatic hydrocarbon if 0.75 g of the compound depresses the freezing point of 123 g of benzene by 0.28°C? (Kf for benzene is 5.12°C/m.)

The volume of a 24.0% (by mass)solution is 65.2 mL.The density of the solution is 1.072 g/mL.What is the mass of the solution?

Which way of expressing concentration is used to relate the vapor pressure of a solution to the amount of nonvolatile solute dissolved in the solution?

What mass of a 29.0% by mass glucose,C6H12O6,solution contains 60.0 g of glucose?

What is the molality of ethanol,C2H5OH,in an aqueous solution that is 36.4% ethanol by mass?

A 2.2-g sample of a small protein having a molecular weight of 42,000 g/mol is dissolved in 31.2 mL of water at 28°C.What is the osmotic pressure of the solution? (R = 0.0821 L · atm/(K · mol))

Based on the formulas of the following solutes,which compound would have the smallest van't Hoff factor (i)?

As the number of solute particles in a given volume of solution increases,

What is the mass percent of ethylene glycol (HOCH2CH2OH)in a solution of ethylene glycol in water that has a freezing point of -17.8°C? (Kf for water is 1.858°C/m.)

According to _____,the partial pressure of solvent,,over a solution equals the vapor pressure of the pure solvent, ,times the mole fraction of solvent, ,in the solution.

What is the mass of H2SO4 in a 38.2-cm3 sample of concentrated sulfuric acid that has a density of 1.84 g/cm3 and consists of 98.3% H2SO4?

The volume of a 34.6% (by mass)solution is 129.0 mL.The density of the solution is 1.116 g/mL.What is the mass of solute in this solution?

For which of the following aqueous solutions would one expect to have the largest van't Hoff factor (i)?

Henry's Law constant is 0.034 mol/kg⋅bar and 0.0013 mol/kg⋅bar for CO2 and O2 respectively at 25°C.What pressure of O2 is required to achieve the same solubility as 0.368 bar of CO2?

For a solution containing only one solute dissolved in a solvent,we can calculate the mole fraction of the solvent directly,given only

Fluids that mix with or dissolve in each other in all proportions are said to be _____.

Which of the following compounds is least soluble in water?

Chemistry and Measurement

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Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

States of Matter; Liquids and Solids

Rates of Reaction

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

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Organic Chemistry

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Filters

What is the mole fraction of urea,CH₄N₂O,in an aqueous solution that is 37% urea by mass?

What is the molar mass of an aromatic hydrocarbon if 0.75 g of the compound depresses the freezing point of 123 g of benzene by 0.28°C? (K_f for benzene is 5.12°C/m.)

What mass of a 29.0% by mass glucose,C₆H₁₂O₆,solution contains 60.0 g of glucose?

What is the molality of ethanol,C₂H₅OH,in an aqueous solution that is 36.4% ethanol by mass?

What is the mass percent of ethylene glycol (HOCH₂CH₂OH)in a solution of ethylene glycol in water that has a freezing point of -17.8°C? (K_f for water is 1.858°C/m.)

What is the mass of H₂SO₄ in a 38.2-cm³ sample of concentrated sulfuric acid that has a density of 1.84 g/cm³ and consists of 98.3% H₂SO₄?

Henry's Law constant is 0.034 mol/kg⋅bar and 0.0013 mol/kg⋅bar for CO₂ and O₂ respectively at 25°C.What pressure of O₂ is required to achieve the same solubility as 0.368 bar of CO₂?