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Exam 13: Physical Properties of Solutions

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Question 21

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Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. On the graph below, sketch the vapor pressure above the salt solution as a function of the mole fraction of H₂O, assuming that Raoult's law is obeyed. Explain how you arrived at your graph.

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Pure water has a vapor pressu...

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Question 22

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Explain the following, on the basis of osmosis or osmotic pressure: When sprinkled with sugar, a dish of sliced fruit will form its own juice.

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The water inside the fruit cel...

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Question 23

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What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Which of the following liquids would make a good solvent for iodine, I₂?

What is the molarity of a solution of 10 % by mass cadmium sulfate, CdSO₄ (molar mass = 208.46 g/mol) by mass? The density of the solution is 1.10 g/mL.

What is the molarity of a solution that is 7.00 % by mass magnesium sulfate and has a density of 1.071 g/mL?

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C₈H₁₈) and water Pair #2: acetic acid (CH₃COOH) and water Pair #3: octane (C₈H₁₈) and carbon tetrachloride (CCl₄)

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq) solution?

A 100. mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate. The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

What mass of ethanol, C₂H₅OH a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at -10.0°C? Assume the density of water is 1.0 g/mL. K_f of water is 1.86°C/m.

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

In the course of research, a chemist isolates a new compound with an empirical formula C₃H₃O₂. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325°C. What is the molecular formula of the compound? (For water, K_f = 1.86°C/m.)

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution?

Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.

To interconvert the concentration units molality (m)and mass percent, you must also know the density of the solution.

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

A solution of carbon tetrachloride in benzene, C₆H₆, at 20°C has a total vapor pressure of 78.50 mmHg. (Assume that this solution is ideal.) The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm³; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm³. What percentage of the volume of this solution is due to carbon tetrachloride? (Hint: assume that you have 1.000 L of solution.)

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. Estimate the mass in grams of KCl needed per liter of pure water to reduce the vapor pressure of water at 25°C by 5%.