What is the expected freezing point of a 0.50 mol kg-1 solution of Li2SO4 in water? Kf for water is 1.86 °C m-1.

A) -0.93 °C B) -1.9 °C C) -2.8 °C D) -6.5 °C A) -0.93 °C B) -1.9 °C C) -2.8 °C D) -6.5 °C

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g mL-1)and 387 mL of CH3CH2CH2OH (d = 0.811 g mL-1).

A) 0.630 mol kg-1 B) 0.812 mol kg-1 C) 1.57 mol kg-1 D) 2.01 mol kg-1 E) 4.98 mol kg-1 A) 0.630 mol kg-1 B) 0.812 mol kg-1 C) 1.57 mol kg-1 D) 2.01 mol kg-1 E) 4.98 mol kg-1

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

Place the following solutions in order of increasing osmotic pressure. I.0.15 mol L-1 C2H6O2 $\quad$II.0.15 mol L-1 MgCl2 $\quad$III.0.15 mol L-1 NaCl

A) III < I < II B) II < III < I C) I < II < III D) II < I < III E) I < III < II A) III < I < II B) II < III < I C) I < II < III D) II < I < III E) I < III < II

Exam 12: Solutions

At a given temperature the vapour pressures of benzene and toluene are 183 mmHg and 59.2 mmHg,respectively.Calculate the total vapour pressure over a solution of benzene and toluene with X_benzene = 0.580.

(Multiple Choice)

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Question 21

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g mol^-1)dissolved in 722 mL of benzene (d = 0.877 g mL^-1).Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

(Multiple Choice)

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Question 22

Choose the aqueous solution with the lowest vapour pressure.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 23

Which of the following defines dissolving?

(Multiple Choice)

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Question 24

What is the expected freezing point of a 0.50 mol kg^-1 solution of Li₂SO₄ in water? K_f for water is 1.86 °C m^-1.

(Multiple Choice)

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Question 25

Choose the aqueous solution below with the highest freezing 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 26

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g mL^-1)and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g mL^-1).

(Multiple Choice)

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Question 27

Which of the following ions should have the most exothermic Δ_hydrationH?

(Multiple Choice)

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Question 28

Define the Tyndall effect.

(Short Answer)

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Question 29

A nonelectrolyte compound with a molar mass of 862 g mol^-1 was dissolved in enough water to make 100 mL of solution at 25 °C and produced an osmotic pressure of 38.4 mbar.Calculate the mass of the compound,in mg,used to make this solution.

(Multiple Choice)

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Question 30

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 31

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C.What mass of sucrose (molar mass = 342.30 g mol^-1)would be needed to dissolve in 500.0 g of water? K_b (water)= 0.512 °C m^-1.

(Multiple Choice)

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Question 32

Place the following aqueous solutions of nonvolatile,nonionic compounds in order of decreasing osmotic pressure. I.0.011 mol L^-1 sucrose II.0.00095 mol L^-1 glucose III.0.0060 mol L^-1 glycerin

(Multiple Choice)

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Question 33

A 125.0 mL sample of an aqueous solution at 25 °C contains 29.4 mg of an unknown nonelectrolyte compound.If the solution has an osmotic pressure of 24.4 mbar,what is the molar mass of the unknown compound?

(Multiple Choice)

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Question 34

Calculate the solution temperature required to produce an osmotic pressure of 1.18 mbar using 3.72 mg of a protein with a molar mass of 4176 g mol^-1 that is dissolved in enough water to create 20.9 mL of solution.

(Multiple Choice)

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Question 35

Identify the major force between acetone and chloroform.

(Multiple Choice)

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Question 36

Place the following solutions in order of increasing osmotic pressure. I.0.15 mol L^-1 C₂H₆O₂ $\quad$ II.0.15 mol L^-1 MgCl₂ $\quad$ III.0.15 mol L^-1 NaCl

(Multiple Choice)

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Question 37

What volume of a 0.716 mol L^-1 KBr solution is needed to provide 30.5 g of KBr?

(Multiple Choice)

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Question 38

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C₆H₈O₆,in 55.0 g of water?

(Multiple Choice)

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Question 39

A small amount,6.78 g,of pentane (C₅H₁₂)is mixed with 100.00 g hexane (C₆H₁₄).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 40

Showing 21 - 40 of 153

Exam 12: Solutions

At a given temperature the vapour pressures of benzene and toluene are 183 mmHg and 59.2 mmHg,respectively.Calculate the total vapour pressure over a solution of benzene and toluene with Xbenzene = 0.580.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8,molar mass = 128.16 g mol-1)dissolved in 722 mL of benzene (d = 0.877 g mL-1).Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m-1.

Choose the aqueous solution with the lowest vapour pressure.These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

Which of the following defines dissolving?

What is the expected freezing point of a 0.50 mol kg-1 solution of Li2SO4 in water? Kf for water is 1.86 °C m-1.

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

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g mL-1)and 387 mL of CH3CH2CH2OH (d = 0.811 g mL-1).

Which of the following ions should have the most exothermic ΔhydrationH?

Define the Tyndall effect.

A nonelectrolyte compound with a molar mass of 862 g mol-1 was dissolved in enough water to make 100 mL of solution at 25 °C and produced an osmotic pressure of 38.4 mbar.Calculate the mass of the compound,in mg,used to make this solution.

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

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C.What mass of sucrose (molar mass = 342.30 g mol-1)would be needed to dissolve in 500.0 g of water? Kb (water)= 0.512 °C m-1.

Place the following aqueous solutions of nonvolatile,nonionic compounds in order of decreasing osmotic pressure. I.0.011 mol L-1 sucrose II.0.00095 mol L-1 glucose III.0.0060 mol L-1 glycerin

A 125.0 mL sample of an aqueous solution at 25 °C contains 29.4 mg of an unknown nonelectrolyte compound.If the solution has an osmotic pressure of 24.4 mbar,what is the molar mass of the unknown compound?

Calculate the solution temperature required to produce an osmotic pressure of 1.18 mbar using 3.72 mg of a protein with a molar mass of 4176 g mol-1 that is dissolved in enough water to create 20.9 mL of solution.

Identify the major force between acetone and chloroform.

Place the following solutions in order of increasing osmotic pressure. I.0.15 mol L-1 C2H6O2 \quad II.0.15 mol L-1 MgCl2 \quad III.0.15 mol L-1 NaCl

What volume of a 0.716 mol L-1 KBr solution is needed to provide 30.5 g of KBr?

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C6H8O6,in 55.0 g of water?

A small amount,6.78 g,of pentane (C5H12)is mixed with 100.00 g hexane (C6H14).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.

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At a given temperature the vapour pressures of benzene and toluene are 183 mmHg and 59.2 mmHg,respectively.Calculate the total vapour pressure over a solution of benzene and toluene with X_benzene = 0.580.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g mol^-1)dissolved in 722 mL of benzene (d = 0.877 g mL^-1).Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

What is the expected freezing point of a 0.50 mol kg^-1 solution of Li₂SO₄ in water? K_f for water is 1.86 °C m^-1.

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g mL^-1)and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g mL^-1).

Which of the following ions should have the most exothermic Δ_hydrationH?

A nonelectrolyte compound with a molar mass of 862 g mol^-1 was dissolved in enough water to make 100 mL of solution at 25 °C and produced an osmotic pressure of 38.4 mbar.Calculate the mass of the compound,in mg,used to make this solution.

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

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C.What mass of sucrose (molar mass = 342.30 g mol^-1)would be needed to dissolve in 500.0 g of water? K_b (water)= 0.512 °C m^-1.

Place the following aqueous solutions of nonvolatile,nonionic compounds in order of decreasing osmotic pressure. I.0.011 mol L^-1 sucrose II.0.00095 mol L^-1 glucose III.0.0060 mol L^-1 glycerin

Calculate the solution temperature required to produce an osmotic pressure of 1.18 mbar using 3.72 mg of a protein with a molar mass of 4176 g mol^-1 that is dissolved in enough water to create 20.9 mL of solution.

Place the following solutions in order of increasing osmotic pressure. I.0.15 mol L^-1 C₂H₆O₂ $\quad$ II.0.15 mol L^-1 MgCl₂ $\quad$ III.0.15 mol L^-1 NaCl

What volume of a 0.716 mol L^-1 KBr solution is needed to provide 30.5 g of KBr?

What is the weight percent of vitamin C in a solution made by dissolving 6.50 g of vitamin C,C₆H₈O₆,in 55.0 g of water?

A small amount,6.78 g,of pentane (C₅H₁₂)is mixed with 100.00 g hexane (C₆H₁₄).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.