Chapter 11 concepts quiz

Calculate the mole fraction of NaCl in a solution prepared by dissolving 117 g NaCl in 1.11 kg H₂O.

• 1.57 × 10^–2

• 9.91 × 10^–1

• 6.29 × 10^–2

• 3.15 × 10^–2

• 1.12 × 10^–2

Shaving cream is an example of which colloid type?

• sol

• aerosol

• foam

• emulsion

• coagulate

A solution of hydrogen peroxide is 26.3% H₂O₂ by mass and has a density of 1.11 g/cm³. The molarity of the solution is:

• 8.95 M

• 0.292 M

• 8.06 M

• none of these

• 8.58 M

Which of the following concentration measures will change in value as the temperature of a solution changes?

• all of these

• molarity

• mole fraction

• molality

• mass percent

A liquid-liquid solution is called an ideal solution if:

I. It obeys PV = nRT.

II. It obeys Raoult's law.

III. Solute-solute, solvent-solvent, and solute-solvent interactions are very similar.

IV. Solute-solute, solvent-solvent, and solute-solvent interactions are quite different.

• I, II, IV

• II, III

• I, III, IV

• II, IV

• I, II, III

Which of the following favors the solubility of an ionic solid in a liquid solvent?

• all of these

• none of these

• a large magnitude of the solvation energy of the ions

• a small magnitude of the lattice energy of the solute

• a large polarity of the solvent

When solid Ca(CH₃COO)₂ is dissolved in a nearly saturated solution of Ca(CH₃COO)₂, the solution becomes warmer. This information indicates that if the temperature of a solution is decreased:

• The solubility of Ca(CH₃COO)₂ will increase.

• ΔH will become negative.

• The solubility of Ca(CH₃COO)₂ will decrease.

• The solubility of Ca(CH₃COO)₂ will not change.

• ΔH will become zero.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS3-4

Rank the following compounds according to increasing solubility in water.

I. CH₃–CH₂–CH₂–CH₃

II. CH₃–CH₂–O–CH₂–CH₃

III. CH₃–CH₂–OH

IV. CH₃–OH

​

• III < IV < II < I

• None of these is correct.

• I < II < III < IV

• I < II < IV < III

• I < III < IV < II

For each of the following solutions, describe the deviation with respect to Raoult's Law.

hexane (C₆H₁₄) and chloroform (CHCl₃)

• relatively ideal

• more information needed

• negative deviation

• none of these

• positive deviation

In osmosis:

• The semipermeable membrane is used to change the freezing and melting points of a solution.

• Knowing the osmotic pressure can help determine the molar mass of a solute dissolved in a solvent.

• Temperature does not affect the osmotic pressure of a solution.

• Solutions cannot have identical osmotic pressures.

• At least two of these statements are correct.