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Exam 14: Solutions

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Question 31

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Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL) .Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m.

A) 2.2°C
B) 2.5°C
C) 82.3°C
D) 80.4°C
E) 82.6°C

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Question 32

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Determine the partial pressure of oxygen necessary to form an aqueous solution that is 6.5 × 10^-4 M O₂ at 25°C.The Henry's law constant for oxygen in water at 25°C is 1.3 × 10^-3 M/atm.

A) 1.2 atm
B) 0.85 atm
C) 0.78 atm
D) 2.0 atm
E) 0.50 atm

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Question 33

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A solution is prepared by dissolving 7.00 g of glycerin (C₃H₈O₃) in 201 g of ethanol (C₂H₅OH) .The freezing point of the solution is ________°C.The freezing point of pure ethanol is -114.6°C at 1 atm.The molal-freezing-point-depression constant (K_f) for ethanol is 1.99°C/m.The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol,respectively.

A compound is found to have a molar mass of 598 g/mol.If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C,what is the osmotic pressure of the resulting solution?

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄) in enough water to make 0.250 L of solution at 25°C is ________ atm.

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

A 1.00 L sample of water contains 0.0044 g of Cl⁻ ions.Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g/mL.

Calculate the osmotic pressure,in torr,of a solution containing 3.00 mg of a sugar (342 g/mole)in enough water to make 15.0 mL of solution at 25°C.

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.

A solution containing more than the equilibrium amount is called

What mass of CuCl₂ is contained in 90.85 g of a 22.4% by mass solution of CuCl₂ in water?

Choose the situation below that would result in a ΔH_solution near 0.

Give the preparation of rock candy.

A solution is prepared by dissolving 16.2 g of benzene (C₆H₆) in 282 g of carbon tetrachloride (CCl₄) .The concentration of benzene in this solution is ________ molal.The molar masses of C₆H₆ and CCl₄ are 78.1 g/mol and 154 g/mol,respectively.

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

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C₂H₅OH,in 53.6 g of water?

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g/mL.

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.

Choose the aqueous solution with the highest vapor pressure.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) and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g/mL) .