Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 mol L-1 O2 at 25 °C. The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10-3 mol L-1 bar-1.

A) 1.9 bar B) 0.53 bar C) 0.24 bar D) 0.77 bar E) 0.32 bar A) 1.9 bar B) 0.53 bar C) 0.24 bar D) 0.77 bar E) 0.32 bar

What mass of CuCl2 is contained in 75.85 g of a 22.4% by mass solution of CuCl2 in water?

A) 17.0 g B) 5.89 g C) 29.5 g D) 33.9 g E) 11.2 g A) 17.0 g B) 5.89 g C) 29.5 g D) 33.9 g E) 11.2 g

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C6H12O6)in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

A) 0.360 bar B) 0.318 bar C) 0.0308 bar D) 0.0387 bar E) 0.00567 bar A) 0.360 bar B) 0.318 bar C) 0.0308 bar D) 0.0387 bar E) 0.00567 bar

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.

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

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.

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

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C5H10O5, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

A) 264 mbar B) 239 mbar C) 309 mbar D) 363 mbar E) 255 mbar A) 264 mbar B) 239 mbar C) 309 mbar D) 363 mbar E) 255 mbar

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C6H12O6)in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

A) 27.8 Torr B) 16.9 Torr C) 28.8 Torr D) 36.9 Torr E) 24.9 Torr A) 27.8 Torr B) 16.9 Torr C) 28.8 Torr D) 36.9 Torr E) 24.9 Torr

Determine the solubility of CO2 in soda water at 25 °C if the pressure of CO2 is 5.2 bar. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 mol L-1 bar-1.

A) 0.15 mol L-1 B) 0.57 mol L-1 C) 0.65 mol L-1 D) 0.18 mol L-1 E) 0.29 mol L-1 A) 0.15 mol L-1 B) 0.57 mol L-1 C) 0.65 mol L-1 D) 0.18 mol L-1 E) 0.29 mol L-1

What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14?

A) 0.058 mol kg-1 B) 0.068 mol kg-1 C) 0.85 mol kg-1 D) 61 mol kg-1 A) 0.058 mol kg-1 B) 0.068 mol kg-1 C) 0.85 mol kg-1 D) 61 mol kg-1

Exam 12: Solutions

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4mol L^-1 O₂ at 25 °C. The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10^-3 mol L^-1 bar^-1.

(Multiple Choice)

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Question 121

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 bar of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10^-3 mol L^-1 bar^-1.

(Multiple Choice)

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Question 122

What mass of CuCl₂ is contained in 75.85 g of a 22.4% by mass solution of CuCl₂ in water?

(Multiple Choice)

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Question 123

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C₆H₁₂O₆)in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

(Multiple Choice)

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Question 124

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.

(Multiple Choice)

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Question 125

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.

(Multiple Choice)

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Question 126

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C₅H₁₀O₅, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

(Multiple Choice)

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Question 127

Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving 0.400 moles of MgCl₂ in 850.0 g of water.

(Multiple Choice)

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Question 128

Determine the solubility of N₂ in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 mol L^-1bar^-1.

(Multiple Choice)

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Question 129

A solution is prepared by dissolving 40.0 g of sucrose, C₁₂H₂₂O₁₁, in 250. 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?

(Multiple Choice)

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Question 130

A solid can be purified through which technique?

(Multiple Choice)

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Question 131

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

(Multiple Choice)

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Question 132

Determine the vapour pressure of a solution at 55 °C that contains 34.2 g NaCl in 375 mL of water. The vapour pressure of pure water at 55 °C is 0.1574 bar.

(Multiple Choice)

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Question 133

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.

(Multiple Choice)

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Question 134

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆)in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

(Multiple Choice)

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Question 135

What mass (in g)of NH₃ must be dissolved in 475 g of methanol to make a 0.250 mol kg^-1 solution?

(Multiple Choice)

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Question 136

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?

(Multiple Choice)

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Question 137

At 20 °C, a 0.376 mol L^-1 aqueous solution of ammonium chloride has a density of 1.0045 g mL^-1. What is the mass % of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g mol^-1.

(Multiple Choice)

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Question 138

Determine the solubility of CO₂ in soda water at 25 °C if the pressure of CO₂ is 5.2 bar. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 mol L^-1 bar^-1.

(Multiple Choice)

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Question 139

What molality of pentane is obtained by dissolving 15 g pentane, C₅H₁₂, in 245.0 g hexane, C₆H₁₄?

(Multiple Choice)

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Question 140

Showing 121 - 140 of 159

Exam 12: Solutions

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 mol L-1 O2 at 25 °C. The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10-3 mol L-1 bar-1.

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 bar of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 mol L-1 bar-1.

What mass of CuCl2 is contained in 75.85 g of a 22.4% by mass solution of CuCl2 in water?

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C6H12O6)in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

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.

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C5H10O5, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.

Determine the solubility of N2 in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 mol L-1 bar-1.

A solution is prepared by dissolving 40.0 g of sucrose, C12H22O11, in 250. 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?

A solid can be purified through which technique?

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

Determine the vapour pressure of a solution at 55 °C that contains 34.2 g NaCl in 375 mL of water. The vapour pressure of pure water at 55 °C is 0.1574 bar.

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.

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C6H12O6)in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

What mass (in g)of NH3 must be dissolved in 475 g of methanol to make a 0.250 mol kg-1 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?

At 20 °C, a 0.376 mol L-1 aqueous solution of ammonium chloride has a density of 1.0045 g mL-1. What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g mol-1.

Determine the solubility of CO2 in soda water at 25 °C if the pressure of CO2 is 5.2 bar. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 mol L-1 bar-1.

What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14?

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Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4mol L^-1 O₂ at 25 °C. The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10^-3 mol L^-1 bar^-1.

Calculate the mass of oxygen (in mg)dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 bar of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10^-3 mol L^-1 bar^-1.

What mass of CuCl₂ is contained in 75.85 g of a 22.4% by mass solution of CuCl₂ in water?

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C₆H₁₂O₆)in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

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.

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C₅H₁₀O₅, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

Calculate the mole fraction of total ions in an aqueous solution prepared by dissolving 0.400 moles of MgCl₂ in 850.0 g of water.

Determine the solubility of N₂ in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 mol L^-1bar^-1.

A solution is prepared by dissolving 40.0 g of sucrose, C₁₂H₂₂O₁₁, in 250. 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?

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆)in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

What mass (in g)of NH₃ must be dissolved in 475 g of methanol to make a 0.250 mol kg^-1 solution?

At 20 °C, a 0.376 mol L^-1 aqueous solution of ammonium chloride has a density of 1.0045 g mL^-1. What is the mass % of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g mol^-1.

Determine the solubility of CO₂ in soda water at 25 °C if the pressure of CO₂ is 5.2 bar. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 mol L^-1 bar^-1.

What molality of pentane is obtained by dissolving 15 g pentane, C₅H₁₂, in 245.0 g hexane, C₆H₁₄?