Question 1

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water Kf = 1.86°C/m and Kb = 0.52°C/m.

Accepted Answer

A) -8.94°C 
B) -366°C 
C) -0.99°C 
D) 0.99°C 
E) 8.94°C 
A) -8.94°C 
B) -366°C 
C) -0.99°C 
D) 0.99°C 
E) 8.94°C

Question 2

When 20.0 grams of an unknown compound are dissolved in 500.grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.444°C, and the Kf for benzene is 5.12°C/m.What is the molar mass of the unknown compound?

Accepted Answer

Question 3

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

Accepted Answer

A) 2.45 * 10-4 m 
B) 5.80 * 10-4 m 
C) 2.45 * 10-1 m 
D) 103 m 
E) 5.80 m 
A) 2.45 * 10-4 m 
B) 5.80 * 10-4 m 
C) 2.45 * 10-1 m 
D) 103 m 
E) 5.80 m

Question 4

Calculate the molality of a 15.0% by mass solution of MgCl2 in H2O. The density of this solution is 1.127 g/mL.

Accepted Answer

A) 0.157 m 
B) 11.8 m 
C) 1.86 m 
D) 0.0134 m 
E) 1.58 m 
A) 0.157 m 
B) 11.8 m 
C) 1.86 m 
D) 0.0134 m 
E) 1.58 m

Question 5

A 20.0 % by mass solution of phosphoric acid (H3PO4)in water has a density of 1.114 g/mL at 20°C.What is the molarity of this solution?

Accepted Answer

A) 0.0114 M 
B) 0.0568 M 
C) 0.114 M 
D) 2.27 M 
E) 11.4 M 
A) 0.0114 M 
B) 0.0568 M 
C) 0.114 M 
D) 2.27 M 
E) 11.4 M

Question 6

Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.

Accepted Answer

The water passes into the cell

Question 7

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C8H18)and water
Pair #2: acetic acid (CH3COOH)and water
Pair #3: octane (C8H18)and carbon tetrachloride(CCl4)

Accepted Answer

A) 1, 3 
B) 1, 2 
C) 3 
D) 2 
E) 2, 3 
A) 1, 3 
B) 1, 2 
C) 3 
D) 2 
E) 2, 3

Question 8

For water Kf = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C2H5OH (ethanol)solutions are the same.

Accepted Answer

A) True 
 B)False

Question 9

What is the concentration of O2(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10-3 mol/L·atm.

Accepted Answer

5.6 * 10<s

Question 10

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH)dissolved in enough water to make 500.mL of solution at 27°C?

Accepted Answer

A) 0.014 atm 
B) 0.037 atm 
C) 0.456 atm 
D) 0.01 atm 
E) 11.2 atm 
A) 0.014 atm 
B) 0.037 atm 
C) 0.456 atm 
D) 0.01 atm 
E) 11.2 atm

Question 11

What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25°C? Kb of water is 0.52°C/m. Assume the density of the solution is the same as that of pure water.

Accepted Answer

A) 0.22°C 
B) 0.429°C 
C) 100.43°C 
D) 99.78°C 
E) 100.22°C 
A) 0.22°C 
B) 0.429°C 
C) 100.43°C 
D) 99.78°C 
E) 100.22°C

Question 12

Which of the following liquids would make a good solvent for iodine, I2?

Accepted Answer

A) HCl 
B) H2O 
C) CH3OH 
D) NH3 
E) CS2 
A) HCl 
B) H2O 
C) CH3OH 
D) NH3 
E) CS2

Question 13

What is the mole fraction of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Question 14

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4)and has a density of 1.0244 g/mL?

Accepted Answer

Question 15

Which of the following has the greater molal concentration (molality)?

Accepted Answer

A) 1.0 m KNO3 
B) 1.0 M KNO3 
C) Both have same molality. 
A) 1.0 m KNO3 
B) 1.0 M KNO3 
C) Both have same molality.

Question 16

Explain the following, on the basis of osmosis or osmotic pressure: Meat that is salted before cooking tends to dry out.

Accepted Answer

The water passes thr

Question 17

An aqueous dextrose solution having a density of 1.04 g/cm3 freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.Kf of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

Accepted Answer

A) 13.8 atm 
B) 14.1 atm 
C) 15.1 atm 
D) 12.9 atm 
E) 120 atm 
A) 13.8 atm 
B) 14.1 atm 
C) 15.1 atm 
D) 12.9 atm 
E) 120 atm

Question 18

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Question 19

A solution is prepared by adding 40.3 g of Mg(NO3)2 to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

Accepted Answer

mole fract

Question 20

A solution is 40.0% by volume benzene (C6H6)in carbon tetrachloride at 20°C. The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm3; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm3. If this solution is ideal, its total vapor pressure at 20°C is

Accepted Answer

A) 84.64 mmHg 
B) 84.30 mmHg 
C) 82.96 mmHg 
D) 81.63 mmHg 
E) 165.93 mmHg 
A) 84.64 mmHg 
B) 84.30 mmHg 
C) 82.96 mmHg 
D) 81.63 mmHg 
E) 165.93 mmHg

Exam 12: Physical Properties of Solutions

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water Kf = 1.86°C/m and Kb = 0.52°C/m.

When 20.0 grams of an unknown compound are dissolved in 500.grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.444°C, and the Kf for benzene is 5.12°C/m.What is the molar mass of the unknown compound?

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

Calculate the molality of a 15.0% by mass solution of MgCl2 in H2O. The density of this solution is 1.127 g/mL.

A 20.0 % by mass solution of phosphoric acid (H3PO4)in water has a density of 1.114 g/mL at 20°C.What is the molarity of this solution?

Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C8H18)and water Pair #2: acetic acid (CH3COOH)and water Pair #3: octane (C8H18)and carbon tetrachloride(CCl4)

For water Kf = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C2H5OH (ethanol)solutions are the same.

What is the concentration of O2(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10-3 mol/L·atm.

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH)dissolved in enough water to make 500.mL of solution at 27°C?

What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25°C? Kb of water is 0.52°C/m. Assume the density of the solution is the same as that of pure water.

Which of the following liquids would make a good solvent for iodine, I2?

What is the mole fraction of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4)and has a density of 1.0244 g/mL?

Which of the following has the greater molal concentration (molality)?

Explain the following, on the basis of osmosis or osmotic pressure: Meat that is salted before cooking tends to dry out.

An aqueous dextrose solution having a density of 1.04 g/cm3 freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.Kf of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO3)2 to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5°C? For water K_f = 1.86°C/m and K_b = 0.52°C/m.

When 20.0 grams of an unknown compound are dissolved in 500.grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.444°C, and the K_f for benzene is 5.12°C/m.What is the molar mass of the unknown compound?

Calculate the molality of a 15.0% by mass solution of MgCl₂ in H₂O. The density of this solution is 1.127 g/mL.

A 20.0 % by mass solution of phosphoric acid (H₃PO₄)in water has a density of 1.114 g/mL at 20°C.What is the molarity of this solution?

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C₈H₁₈)and water Pair #2: acetic acid (CH₃COOH)and water Pair #3: octane (C₈H₁₈)and carbon tetrachloride(CCl₄)

For water K_f = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol)solutions are the same.

What is the concentration of O₂(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-3 mol/L·atm.

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C₃H₇OH)dissolved in enough water to make 500.mL of solution at 27°C?

What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25°C? K_b of water is 0.52°C/m. Assume the density of the solution is the same as that of pure water.

Which of the following liquids would make a good solvent for iodine, I₂?

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

An aqueous dextrose solution having a density of 1.04 g/cm³ freezes at -1.15°C. Find the osmotic pressure of this solution at 25°C.K_f of water is 1.86 °C/m; molecular mass of dextrose = 180.16 g/mol.

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO₃)₂ to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.