Calculate the number of moles of solute present in each of the following aqueous solutions: (c) 124.0 g of a solution that is 6.45% glucose (C₆H₁₂O₆) by mass.

Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO₃(aq),

Calculate the number of moles of solute present in each of the following solutions: (b) 50.0 mg of an aqueous solution that is 1.50 m NaCl, (c) 75.0 g of an aqueous solution that is 1.50% sucrose (C₁₂H₂₂O₁₁) by mass.

Describe how you would prepare each of the following aqueous solutions from water and solid KBr: b. 125 g of 0.180 m KBr.

Describe how you would prepare each of the following aqueous solutions from water and the solid solute: a. 1.50 L of 0.110 M (NH₄)₂SO₄ solution;

Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNO₃ by mass in the solution.

Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 80.0 % Cu and 20.0 % Zn by mass has a density of 8750 kg/m³. (a) What is the molality of Zn in the solid solution?

Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 80.0 % Cu and 20.0 % Zn by mass has a density of 8750 kg/m³. (b) What is the molarity of Zn in the solution?

Caffeine (C₈H₁₀N₄O₂) is a stimulant found in coffee and tea. If a solution of caffeine in the solvent chloroform (CHCl₃) has a concentration of 0.0500 m, calculate (b) the mole fraction of caffeine in the solution.

Assume that a portable reverse-osmosis apparatus operates on seawater, whose effective concentration (the concentration of dissolved ions) is 1.12 M, and that the desalinated water output has an effective molarity of about 0.02 M. What minimum pressure must be applied by hand pumping at 297 K to cause reverse osmosis to occur?

You make a solution of a nonvolatile solute with a liquid solvent. Indicate if each of the following statements is true or false.

a. The solid that forms as the solution freezes is nearly pure solute.

You make a solution of a nonvolatile solute with a liquid solvent. Indicate if each of the following statements is true or false.

b. The freezing point of the solution is independent of the concentration of the solute.

a. The vapor pressure of pure water at 60°C is 149 torr. What vapor pressure is predicted by Raoult’s law for a solution at 60°C that is 50 mol % water and 50 mol % ethylene glycol (a nonvolatile solute)?

At 63.5 °C, the vapor pressure of H₂O is 175 torr, and that of ethanol (C₂H₅OH) is 400 torr. A solution is made by mixing equal masses of H₂O and C₂H₅OH. (a) What is the mole fraction of ethanol in the solution?

At 63.5 °C, the vapor pressure of H₂O is 175 torr, and that of ethanol (C₂H₅OH) is 400 torr. A solution is made by mixing equal masses of H₂O and C₂H₅OH. (b) Assuming ideal solution behavior, what is the vapor pressure of the solution at 63.5 °C?

At 63.5 °C, the vapor pressure of H₂O is 175 torr, and that of ethanol (C₂H₅OH) is 400 torr. A solution is made by mixing equal masses of H₂O and C₂H₅OH. (a) What is the composition in mole fraction of a solution that has a vapor pressure of 35 torr at 20 °C?

At 20 °C, the vapor pressure of benzene (C₆H₆) is 75 torr, and that of toluene (C₇H₈) is 22 torr. Assume that benzene and toluene form an ideal solution. (a) What is the composition in mole fraction of a solution that has a vapor pressure of 35 torr at 20 °C?

At 20 °C, the vapor pressure of benzene (C₆H₆) is 75 torr, and that of toluene (C₇H₈) is 22 torr. Assume that benzene and toluene form an ideal solution. (b) What is the mole fraction of benzene in the vapor above the solution described in part (a)?

List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.050 m LiBr, 0.050 m Zn(NO₃)₂.

Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.22 m glycerol (C₃H₈O₃) in ethanol, (b) 0.240 mol of naphthalene (C₁₀H₈) in 2.45 mol of chloroform, (c) 1.50 g NaCl in 0.250 kg of water, (d) 2.04 g KBr and 4.82 g of glucose (C₆H₁₂O₆) in 188 g of water.

Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.25 m glucose in ethanol; (b) 20.0 g of decane, C₁₀H₂₂, in 50.0 g CHCl₃; (c) 3.50 g NaOH in 175 g of water, (d) 0.45 mol ethylene glycol and 0.15 mol KBr in 150 g H₂O.

What is the freezing point of an aqueous solution that boils at 105.0 °C?