Solutions: Solubility and Intermolecular Forces

Indicate the most important type of intermolecular attraction responsible for solvation in the following solution:

Methanol, CH₃OH, dissolved in ethanol, CH₃CH₂OH

Which of the following solutes will most readily dissolve in H₂O?

Two pure chemical substance are likely to mix and form a solution if:

Which of the following statements is/are true?

I. The hydrocarbon methane (CH₄) will dissolve completely in acetone (CH₃COCH₃).

II. Ammonia (NH₃) will form a heterogeneous mixture with carbon tetrachloride (CCl₄).

III. Pentane (C₅H₁₂) will form a homogeneous mixture with carbon tetrabromide (CBr₄).

IV. Methanethiol (CH₃SH) is miscible in fluoromethane (CH₃F).

A solution is prepared by dissolving 43.0 g potassium chlorate, KClO₃, in enough water to make 100.0 mL of solution. If the density of the solution is 1.760 g/mL, what is the molality of KClO₃ in the solution?

The density of a 15.7 M methanol (CH₃OH) solution is 0.858 g/mL. If H₂O is the solvent, what is the molality of the solution?

What is the ionic molality of sodium ions in a solution of 25.7 g NaNO₃ dissolved in enough water to make a 150.0 mL of solution? Density of the solution is 1.02 g/mL.

A 5.12 L sample of solution contains 0.230 g of potassium sulfate, K₂SO₄. Determine the concentration of K₂SO₄ in ppm if the density of the solution is 1.30 g/mL.

Calculate the concentration in parts per billion of the following aqueous solution:0.91 mg of caffeine in a total volume of 131 mL.

Glucose makes up about 0.102% by mass of human blood. Calculate this concentration in ppm.

The average human body contains about 5,000 grams of blood. What mass of arsenic is present in the body if the amount in blood is 0.86 ppb?

A water sample contains the pollutant chlorobenzene with a concentration of 16 ppm (by volume). What volume of this water contains 5.01×10² mL of chlorobenzene?

Calculate mole fraction of a 2.4 m aqueous solution of citric acid (C₆H₈O₇).

If mole fraction of urea is 4.55 × 10^–1, what is the mass of urea needed to prepare 38.0 g of solution in water?

Calculate the amount of water (in kilograms) that must be added to 12.0 g of urea, (NH₂)₂CO, in the preparation of a 18.3 percent by mass solution. The molar mass of urea, (NH₂)₂CO, is 60.055 g/mol.

A solution was prepared by dissolving 51.0 g of KBr in 310 mL of water. Calculate the mass percent of KBr in the solution.

An aqueous LiNO₂ solution is made using 90.3 g LiNO₂ and diluting it to a total volume of 1.72 L. If the density of the solution is 1.20 g/mL, what is the mass percent of the solution?

Determine the percent sulfuric acid by mass of a 1.37 m aqueous solution of H₂SO₄.

The solubility of KClO₃ in water at 30ºC is 10 g per 100 mL of water. A 0.95 M solution of KClO₃ in water at 30ºC is:

Which of the following is true for the solubility of NaCl(s) and CH₄(g) in water?  

Henry’s Law Constant for nitrogen in water is 1.67 × 10^-4 M • atm^–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?

At 0°C and 1.00 atm, as much as 0.84 g of O₂ can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O₂ dissolve in 1.0 L of water?

The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry’s Law Constant for oxygen in water at this temperature is 5.3 × 10^–5 M/atm.

Which of the following compounds will have the highest boiling point?

Which of the following compound will have the highest vapor pressure?

An ethylene glycol solution contains 25.2 g of ethylene glycol (C₂H₆O₂) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.

Pure water boils at 100°C. What is the new boiling point of water after the addition of 13.12 g aluminum chloride, AlCl₃, to 615 g water?  

What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15°C?

Carbon dioxide is dissolved in 722 mL of benzene with a density of 1.59 g/mL. What mass of carbon dioxide would you add to make the boiling point of the solution 104.7°C?

How many moles of ethylene glycol, C₂H₆O₂, must be added to 1,000 g of water to form a solution that has a freezing point of –10ºC?