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

A solution is 2.25% by weight NaHCO3.How many grams of NaHCO3 are in 150.0 g of solution?

A) 1.50 g B) 3.38 g C) 66.7 g D) 225 g A) 1.50 g B) 3.38 g C) 66.7 g D) 225 g

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3,molar mass = 92.09 g mol-1)in 376 mL of water.Some possibly useful constants for water are Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

A) 0.887 °C B) 1.65 °C C) 2.54 °C D) 3.33 °C E) 0.654 °C A) 0.887 °C B) 1.65 °C C) 2.54 °C D) 3.33 °C E) 0.654 °C

Exam 12: Solutions

A solution is prepared by dissolving 21.0 g of glycerin ( $\mathrm { C } _ { 3 }$ $\mathrm { Hg }$ $\mathrm { O } _ { 3 }$ )in 201 g of ethanol $\left( \mathrm { C } _ { 2 } \mathrm { H } _ { 5 } \mathrm { OH } \right)$ The freezing point of the solution is ________°C.The freezing point of pure ethanol is $- 114.6 ^ { \circ } \mathrm { C }$ .The molal freezing point depression constant ( $K_f$ )for ethanol is $1.99 ^ { \circ } \mathrm { Cm } ^ { - 1 }$ The molar masses of glycerin and of ethanol are 92.1 g mol^-1 and 46.1 g mol^-1,respectively.

(Multiple Choice)

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Question 61

Determine the Henry's law constant for ammonia in water at 25 °C if an ammonia pressure of 0.022 bar produces a solution with a concentration of 1.3 mol L^-1.

(Multiple Choice)

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Question 62

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF₂ in 11.5 moles H₂O.

(Multiple Choice)

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Question 63

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 64

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

(Essay)

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Question 65

The Henry's law constant for helium gas in water at 30 °C is 3.70 × $10 ^ { - 4 }$ mol L^-1 bar^-1.When the partial pressure of helium above a sample of water is 0.450 bar,the concentration of helium in the water is ________ mol L^-1.

(Multiple Choice)

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Question 66

Identify the major force between ethanol and water.

(Multiple Choice)

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Question 67

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

(Multiple Choice)

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Question 68

A solution of methanol and water has a vapour pressure of 248 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.

(Multiple Choice)

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Question 69

Equal masses,5.00 g,of pentane (C₅H₁₂)and hexane (C₆H₁₄)are mixed.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.

(Multiple Choice)

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Question 70

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.

(Multiple Choice)

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Question 71

A solution is 2.25% by weight NaHCO₃.How many grams of NaHCO₃ are in 150.0 g of solution?

(Multiple Choice)

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Question 72

Explain why water does not dissolve in gasoline.

(Short Answer)

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Question 73

Calculate the volume of solution that has a vapour pressure of 25.8 mbar and contains 200.3 g of galactose,C₆H₁₂O₆,at a temperature of 22.0 °C.The vapour pressure of pure water at 22 °C is 26.40 mbar,the density of water is 1.00 g mL^-1,and assume no change in volume occurs upon dissolution.

(Multiple Choice)

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Question 74

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

(Multiple Choice)

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Question 75

A nonelectrolyte compound with a molar mass of 648 g mol^-1 was dissolved in enough water to make 250 mL of solution at 25 °C and produced an osmotic pressure of 27.4 mbar.Calculate the mass of the compound,in g,used to make this solution.

(Multiple Choice)

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Question 76

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

(Multiple Choice)

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Question 77

Identify the compound whose solubility decreases with increasing temperature.

(Multiple Choice)

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Question 78

A solution is prepared by dissolving 16.4 g of benzene ( $\mathrm { C } _ { 6 }$ $\mathrm { H } _ { 6 }$ )in 282 g of carbon tetrachloride $\left( \mathrm { CCl } _ { 4 } \right)$ The concentration of benzene in this solution is ________ molal.The molar masses of $\mathrm { C } _ { 6 } \mathrm { H } _ { 6 }$ and $\mathrm { CCl } _ { 4 }$ are $78.1 \mathrm {~g} \mathrm {~mol} ^ { - 1 }$ and $154 \mathrm {~g} \mathrm {~mol} ^ { - 1 }$ respectively.

(Multiple Choice)

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Question 79

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃,molar mass = 92.09 g mol^-1)in 376 mL of water.Some possibly useful constants for water are K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 153

Exam 12: Solutions

Determine the Henry's law constant for ammonia in water at 25 °C if an ammonia pressure of 0.022 bar produces a solution with a concentration of 1.3 mol L-1.

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.

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

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

The Henry's law constant for helium gas in water at 30 °C is 3.70 × 10−410 ^ { - 4 }10−4 mol L-1 bar-1.When the partial pressure of helium above a sample of water is 0.450 bar,the concentration of helium in the water is ________ mol L-1.

Identify the major force between ethanol and water.

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

A solution of methanol and water has a vapour pressure of 248 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.

Equal masses,5.00 g,of pentane (C5H12)and hexane (C6H14)are mixed.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.

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 solution is 2.25% by weight NaHCO3.How many grams of NaHCO3 are in 150.0 g of solution?

Explain why water does not dissolve in gasoline.

Calculate the volume of solution that has a vapour pressure of 25.8 mbar and contains 200.3 g of galactose,C6H12O6,at a temperature of 22.0 °C.The vapour pressure of pure water at 22 °C is 26.40 mbar,the density of water is 1.00 g mL-1,and assume no change in volume occurs upon dissolution.

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

A nonelectrolyte compound with a molar mass of 648 g mol-1 was dissolved in enough water to make 250 mL of solution at 25 °C and produced an osmotic pressure of 27.4 mbar.Calculate the mass of the compound,in g,used to make this solution.

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Identify the compound whose solubility decreases with increasing temperature.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3,molar mass = 92.09 g mol-1)in 376 mL of water.Some possibly useful constants for water are Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

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Determine the Henry's law constant for ammonia in water at 25 °C if an ammonia pressure of 0.022 bar produces a solution with a concentration of 1.3 mol L^-1.

Determine the molality of a solution prepared by dissolving 0.500 moles of CaF₂ in 11.5 moles H₂O.

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

The Henry's law constant for helium gas in water at 30 °C is 3.70 × $10 ^ { - 4 }$ mol L^-1 bar^-1.When the partial pressure of helium above a sample of water is 0.450 bar,the concentration of helium in the water is ________ mol L^-1.

Equal masses,5.00 g,of pentane (C₅H₁₂)and hexane (C₆H₁₄)are mixed.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.

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 solution is 2.25% by weight NaHCO₃.How many grams of NaHCO₃ are in 150.0 g of solution?

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

A nonelectrolyte compound with a molar mass of 648 g mol^-1 was dissolved in enough water to make 250 mL of solution at 25 °C and produced an osmotic pressure of 27.4 mbar.Calculate the mass of the compound,in g,used to make this solution.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃,molar mass = 92.09 g mol^-1)in 376 mL of water.Some possibly useful constants for water are K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.