Question 1

Why isn't pentanol (CH3CH2CH2CH2CH2OH)very soluble in water?

Accepted Answer

Even though the pentanol molecule contai

Question 2

To make a 2.00 mol kg-1 solution,one could take 2.00 moles of solute and add

Accepted Answer

A) 1.00 L of solvent. 
B) 1.00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution. 
A) 1.00 L of solvent. 
B) 1.00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution.

Question 3

Which of the following compounds will be most soluble in pentane (C5H12)?

Accepted Answer

A) pentanol (CH3CH2CH2CH2CH2OH) 
B) benzene (C6H6) 
C) acetic acid (CH3CO2H) 
D) ethyl methyl ketone (CH3CH2COCH3) 
E) None of these compounds should be soluble in pentane. 
A) pentanol (CH3CH2CH2CH2CH2OH) 
B) benzene (C6H6) 
C) acetic acid (CH3CO2H) 
D) ethyl methyl ketone (CH3CH2COCH3) 
E) None of these compounds should be soluble in pentane.

Question 4

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol-1 that is dissolved in enough water to create 20.0 mL of solution.

Accepted Answer

A) 288 K 
B) 293 K 
C) 278 K 
D) 314 K 
E) 299 K 
A) 288 K 
B) 293 K 
C) 278 K 
D) 314 K 
E) 299 K

Question 5

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl if the solution has a density of 1.20 g mL-1.

Accepted Answer

A) 7.79 mol L-1 
B) 10.7 mol L-1 
C) 12.8 mol L-1 
D) 9.35 mol L-1 
E) 13.9 mol L-1 
A) 7.79 mol L-1 
B) 10.7 mol L-1 
C) 12.8 mol L-1 
D) 9.35 mol L-1 
E) 13.9 mol L-1

Question 6

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 7

A solution of methanol and water has a vapour pressure of 213 Torr.What would you predict as the mole fractions of each component,assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr,respectively.

Accepted Answer

A)  $\chi \text { methanol }$ = 0.214,$\chi \text { water }$ = 0.786 
B)  $\chi \text { methanol }$ = 0.786,$\chi \text { water }$ = 0.214 
C)  $\chi \text { methanol }$ = 0.885,$\chi \text { water }$ = 0.115 
D)  $\chi _ { \text {methanol } } = 0.900 , \chi \text { water } = 0.100$ 
E)  $\chi \text { methanol }$ = 0.115,$\chi \text { water }$ = 0.885 
A)  $\chi \text { methanol }$ = 0.214,$\chi \text { water }$ = 0.786 
B)  $\chi \text { methanol }$ = 0.786,$\chi \text { water }$ = 0.214 
C)  $\chi \text { methanol }$ = 0.885,$\chi \text { water }$ = 0.115 
D)  $\chi _ { \text {methanol } } = 0.900 , \chi \text { water } = 0.100$ 
E)  $\chi \text { methanol }$ = 0.115,$\chi \text { water }$ = 0.885

Question 8

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.Use 100 °C as the boiling point of water.

Accepted Answer

A) 108 °C 
B) 92 °C 
C) 130 °C 
D) 70 °C 
E) 8.3 °C 
A) 108 °C 
B) 92 °C 
C) 130 °C 
D) 70 °C 
E) 8.3 °C

Question 9

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

Accepted Answer

A) 30.0 °C 
B) -30.0 °C 
C) 8.32 °C 
D) -8.32 °C 
E) 70.2 °C 
A) 30.0 °C 
B) -30.0 °C 
C) 8.32 °C 
D) -8.32 °C 
E) 70.2 °C

Question 10

Twice as much pentane (C5H12)is mixed with hexane (C6H14)by mass.Calculate the vapour pressure of the resulting solution.The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr,respectively.Assume ideal behaviour.

Accepted Answer

A) 386 Torr 
B) 300 Torr 
C) 311 Torr 
D) 253 Torr 
E) 344 Torr 
A) 386 Torr 
B) 300 Torr 
C) 311 Torr 
D) 253 Torr 
E) 344 Torr

Question 11

Which of the following should have the largest Henry's law constant (kH)in water?

Accepted Answer

A) Ar 
B) CO 
C) Xe 
D) CH3CH3 
E) CO2 
A) Ar 
B) CO 
C) Xe 
D) CH3CH3 
E) CO2

Question 12

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

Question 13

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

Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH)very soluble in water?

To make a 2.00 mol kg^-1 solution,one could take 2.00 moles of solute and add

Which of the following compounds will be most soluble in pentane (C₅H₁₂)?

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol^-1 that is dissolved in enough water to create 20.0 mL of solution.

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl if the solution has a density of 1.20 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.

A solution of methanol and water has a vapour pressure of 213 Torr.What would you predict as the mole fractions of each component,assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr,respectively.

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.Use 100 °C as the boiling point of water.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Twice as much pentane (C₅H₁₂)is mixed with hexane (C₆H₁₄)by mass.Calculate the vapour pressure of the resulting solution.The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr,respectively.Assume ideal behaviour.

Which of the following should have the largest Henry's law constant (k_H)in water?

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.

Which of the following statements is generally TRUE?

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Exam 12: Solutions

Why isn't pentanol (CH3CH2CH2CH2CH2OH)very soluble in water?

To make a 2.00 mol kg-1 solution,one could take 2.00 moles of solute and add

Which of the following compounds will be most soluble in pentane (C5H12)?

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol-1 that is dissolved in enough water to create 20.0 mL of solution.

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl if the solution has a density of 1.20 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.

A solution of methanol and water has a vapour pressure of 213 Torr.What would you predict as the mole fractions of each component,assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr,respectively.

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.Use 100 °C as the boiling point of water.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2)dissolved in 500.0 g of water.Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

Twice as much pentane (C5H12)is mixed with hexane (C6H14)by mass.Calculate the vapour pressure of the resulting solution.The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr,respectively.Assume ideal behaviour.

Which of the following should have the largest Henry's law constant (kH)in water?

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.

Which of the following statements is generally TRUE?

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH)very soluble in water?

To make a 2.00 mol kg^-1 solution,one could take 2.00 moles of solute and add

Which of the following compounds will be most soluble in pentane (C₅H₁₂)?

Calculate the solution temperature required to produce an osmotic pressure of 1.10 mbar using 3.85 mg of a protein with a molar mass of 4183 g mol^-1 that is dissolved in enough water to create 20.0 mL of solution.

Commercial grade HCl solutions are typically 39.0% (by mass)HCl in water.Determine the molarity of the HCl if the solution has a density of 1.20 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.

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.Use 100 °C as the boiling point of water.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂)dissolved in 500.0 g of water.K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Twice as much pentane (C₅H₁₂)is mixed with hexane (C₆H₁₄)by mass.Calculate the vapour pressure of the resulting solution.The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr,respectively.Assume ideal behaviour.

Which of the following should have the largest Henry's law constant (k_H)in water?

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.