Exam 11: Properties of Solutions Their Concentrations and Colligative Properties

A physiological saline solution is 0.92% NaCl by mass.What is the osmotic pressure of such a solution at a body temperature of 37 $\degree$ C? Assume the density of the solution is 1.0 g/mL.

Indicate which aqueous solution has the highest vapor pressure.

Suppose a particular salt is composed of +1 cations and -2 anions.When 125 grams of this salt is dissolved in 1.00 kg water (K_b = 0.512 $\degree$ C/m), the boiling point changes by 1.10 $\degree$ C.What is the approximate molar mass of the salt?

What is the molarity of a sucrose (C₁₂H₂₂O₁₁) solution that produces an osmotic pressure of 2.65 atm at 25.0 $\degree$ C?

What is the boiling point of a solution prepared by dissolving 157.0 g of urea (CH₄N₂O, 60.06 g/mol) in 750.0 g of water? (K_b = 0.512 $\degree$ C/m for water)

Which statement regarding the fractional distillation of two liquids is NOT correct?

The vapor pressure of acetone (C₃H₆O, 58.08 g/mol) at 30.0 $\degree$ C is approximately 0.3270 atm.Approximately how many grams of benzophenone, a nonvolatile solute C₁₃H₁₀O, 182.21 g/mol), are dissolved in 150 g of acetone when the vapor pressure of the solution is 0.3169 atm at 30.0 $\degree$ C?

Carbonated beverages are manufactured to dissolve carbon dioxide gas at high pressure that is released when the can is opened so that the beverage is more refreshing to the consumer.How many grams of dissolved carbon dioxide are in a 355 mL can of soda pop at 20 $\degree$ C if the manufacturer used a pressure of 2.4 atm of CO₂ to carbonate the soda pop? The Henry's law constant for carbon dioxide dissolving in water is 3.5 *10^-2 mol/L .atm at 20 $\degree$ C.

Which statement regarding nonideal solutions is NOT correct?

A solution is prepared by mixing 75 g of methanol (CH₃OH, 32.04 g/mol) with 25 g of ethanol (CH₃CH₂OH, 46.07 g/mol).What is the partial pressure of methanol in the vapor phase at 20 $\degree$ C?

At 25 $\degree$ C, the vapor pressure of pure water is 25.756 mmHg.What is the vapor pressure of water in a solution that contains 2.922 g of sodium chloride for every 100.0 g of water?

Describe how you would use data obtained from the following three experiments to determine the molar mass of a compound: 1) measurements of the freezing point of the solution, 2) measurements of the boiling point of the solution, and 3) measurements of the conductivity of the solution.

Describe the effect of increasing temperature, increasing surface area, and increasing intermolecular forces on the evaporation rate of a liquid.Explain your answers.

Which has the higher vapor pressure at a given temperature, pure water or salty seawater? Explain.

Henry's law constant for carbon dioxide dissolving in water is 3.5 * 10^-2 mol/L . atm at 20 $\degree$ C.What is the maximum molar concentration of carbon dioxide in a pond at this temperature? The mole fraction of CO₂ in air is 3.14 * 10^-4.

A solution is prepared by mixing 75 g of methanol (CH₃OH, 32.04 g/mol) with 25 g of ethanol (CH₃CH₂OH, 46.07 g/mol).Use the following data to determine the vapor pressure of this solution at 20 $\degree$ C.

Identify the following statement as true or false and choose the correct explanation: "For solutions requiring the same external pressure to cause reverse osmosis at the same temperature, the molarity of a sodium chloride solution will always be less than the molarity of a calcium chloride solution."

Which of the following aqueous solutions will have the lowest freezing point?

What physical property is used to separate the hydrocarbon components in petroleum (crude oil)?

Gasoline is primarily a mixture of hydrocarbons and is sold with an octane rating that is based on a comparison with the combustion properties of isooctane.Gasoline usually contains an isomer of isooctane called tetramethylbutane (C₈H₁₈), which has an enthalpy of vaporization of 43.3 kJ/mol and a boiling point of 106.5 $\degree$ C.Determine the vapor pressure of tetramethylbutane on a very hot day when the temperature is 38.0 $\degree$ C.