Which statement regarding osmotic pressure is NOT correct? Osmotic pressure

is the same for solutions with the same mass percent of solute.

increases with increasing temperature.

increases with increasing molar concentration of the solute.

is greater for 0.1 M Na2SO4 than for 0.1 M NaCl.

depends on the value of the gas constant R.

Identify the following statement as true or false and choose the correct explanation: “For solutions with the same molarity at the same temperature, the pressure needed for reverse osmosis of a sodium chloride solution will always be less than the pressure needed for a calcium chloride solution.”

False, because the van ’t Hoff factor is smaller for sodium chloride.

True, because the molar mass of sodium chloride is smaller.

True, because the van ’t Hoff factor is smaller for sodium chloride.

False, because the van ’t Hoff factor is larger for sodium chloride.

True, because the van ’t Hoff factor is larger for sodium chloride.

Which of the following statements regarding the phase diagram of water and an aqueous solution is NOT correct? Temperature is on the x-axis; pressure is on the y-axis.

The normal freezing point of the solution corresponds to point A.

The boiling point of the solution is higher than that of the solvent by an amount indicated by the difference in temperature between points E and F.

Point D corresponds to the triple point of the solvent.

The solution boils at the temperature corresponding to point F.

The freezing point of the solvent is higher than that of the solution.

Which statement below regarding vapor pressure is NOT correct?

A nonvolatile solute increases the vapor pressure of the solvent.

Vapor pressure is an intensive property.

The substance with the stronger intermolecular forces has the lower vapor pressure.

Vapor pressure increases with increasing temperature.

Pure water has a higher vapor pressure at a given temperature than seawater.

Which statement is NOT correct? Determination of the molar mass of an unknown sample by an osmotic pressure measurement requires that

the solute dissolved in the solution is pure.

the solute is a nonelectrolyte.

the molecules of the solute do not pass through the semipermeable membrane.

the mass of the solute dissolved in the solution is known in advance.

the molar concentration of the solute in the solution is known in advance.

You wish to de-ice your driveway, so you consider buying 10 lb of NaCl, 10 lb of CaCl₂, or 10 lb of MgCl₂. Which of these would de-ice your driveway most effectively? Assume that ideal dissociation of the salts occurs and that colligative properties are the only consideration.

10 lb of CaCl₂ or 10 lb of MgCl₂ will de-ice equally well.

10 lb of NaCl will de-ice best.

10 lb of CaCl₂ will de-ice best.

10 lb of MgCl₂ will de-ice best.

The three driveways will de-ice to the same extent.

Two solutions, A and B, are separated by a semipermeable membrane. Which of the following statements regarding their tonicities is NOT correct? Assume the same van 't Hoff factor for each solution.

If the molarity of B is lower than that of A, A is hypertonic relative to B.

If A and B are of equal molarities, they are isotonic.

If the molarity of A is lower than that of B, solvent will flow from B to A.

If the molarity of B is lower than that of A, B is hypotonic relative to A.

If the molarity of A is lower than that of B, the osmotic pressure of B is higher than that of A.

Which of the following statements regarding solutions and the van 't Hoff factor is NOT correct?

In dilute solutions, the experimental van 't Hoff factor for a molecule is always greater than 1.

Nonideal behavior can occur in solutions containing ions when the ions do not behave as independent particles in solution.

Theoretical van 't Hoff factors often predict colligative properties of solutions with concentrations of about 0.01 m or less.

As concentrations increase, the probability of ion pairing increases.

The deviation from ideal behavior generally increases as the charge on dissolved ions increases.

Which solution, if either, would create the higher osmotic pressure (compared to pure water): one prepared from 1.0 g of NaCl in 10 mL of water or one prepared from 1.0 g of CsBr in 10 mL of water?

CsBr would give the higher pressure.

They would have the same osmotic pressures.

NaCl would give the higher pressure.

These compounds are salts and do not produce an osmotic pressure.

Chapter 11 Practice

Authored by Zi Yang

Chemistry

University

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The normal temperature range of the liquid phase of pure water is 0°C to 100°C. Which of the following solutions will have the largest temperature range for the liquid state?

1 M aqueous ethanol solution

1 M aqueous potassium bromide solution

1 M aqueous acetic acid solution

1 M aqueous magnesium bromide solution

1 M aqueous magnesium sulfate

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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

melting point

density

boiling point

molar mass

viscosity

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Drinking seawater is dehydrating to humans because

there is a net flow of water molecules out of the cells because the solution is hypertonic.

there is a net flow of water molecules out of the cells because the solution is hypotonic.

there is a net flow of hydrated Na+, Cl-, and other ions into the cells because the solution is hypertonic.

there is a net flow of hydrated Na+, Cl-, and other ions into the cells because the solution is hypotonic.

the hydrated Na+, Cl-, and other ions block channels in the cell membrane, preventing water molecules from migrating into or out of the cells.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The normal freezing point of benzene (C6H6, 78.12 g/mol) is 5.49°C, and its Kf value is 5.12°C/m. To create a solution with a freezing point of 0.00°C, how many grams of naphthalene (C10H8, 128.2 g/mol) would need to be dissolved in 640.0 g of benzene?

5.63 g

137 g

82.0 g

187 g

88.0 g

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Determine the molal concentration of a table sugar (C12H22O11, 342.3 g/mol) solution in water that has a freezing point of –2.10°C. (Kf = 1.86°C/m for water)

1.13 m

–1.13 m

3.91 m

–3.91 m

0.113 m

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Determine the vapor pressure of n-pentane on a night when the temperature is 0.0°C. The enthalpy of vaporization of n-pentane is 27.6 kJ/mol, and its boiling point is 36.0°C.

228 torr

367 torr

185 torr

479 torr

209 torr

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Indicate which aqueous solution has the slowest evaporation rate.

0.1 M NH4Cl

0.2 M K2SO4

0.2 M NaOH

0.1 M BaCl2

0.2 M C6H12O6

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Chapter 11 Practice

The normal temperature range of the liquid phase of pure water is 0°C to 100°C. Which of the following solutions will have the largest temperature range for the liquid state?

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

Drinking seawater is dehydrating to humans because

The normal freezing point of benzene (C6H6, 78.12 g/mol) is 5.49°C, and its Kf value is 5.12°C/m. To create a solution with a freezing point of 0.00°C, how many grams of naphthalene (C10H8, 128.2 g/mol) would need to be dissolved in 640.0 g of benzene?

Determine the molal concentration of a table sugar (C12H22O11, 342.3 g/mol) solution in water that has a freezing point of –2.10°C. (Kf = 1.86°C/m for water)

Determine the vapor pressure of n-pentane on a night when the temperature is 0.0°C. The enthalpy of vaporization of n-pentane is 27.6 kJ/mol, and its boiling point is 36.0°C.

Indicate which aqueous solution has the slowest evaporation rate.

Which statement regarding osmotic pressure is NOT correct? Osmotic pressure

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°C.

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