Question 1

Which of the following is not soluble in water?

Accepted Answer

A)  Vitamin C 
B)  NaCl 
C)  CH3CH2OH 
D)  NH3 
E)  Vitamin E 
A)  Vitamin C 
B)  NaCl 
C)  CH3CH2OH 
D)  NH3 
E)  Vitamin E

Question 2

Which combination of a 36.0% (w/w) stock solution of acetic acid (d = 1.045 g/mL) and water will result in 1.00 kg of a 15.0% (w/w) acetic acid solution?

Accepted Answer

A)  417 mL of 36% acetic acid in 583 mL of distilled water 
B)  417 g of 36% acetic acid in 583 g of distilled water 
C)  360 mL of 36% acetic acid in 640 mL of distilled water 
D)  360 g of 36% acetic acid in 640 g of distilled water 
E)  150 g of 36% acetic acid in 850 g of distilled water 
A)  417 mL of 36% acetic acid in 583 mL of distilled water 
B)  417 g of 36% acetic acid in 583 g of distilled water 
C)  360 mL of 36% acetic acid in 640 mL of distilled water 
D)  360 g of 36% acetic acid in 640 g of distilled water 
E)  150 g of 36% acetic acid in 850 g of distilled water

Question 3

Which is most soluble in CCl4?

Accepted Answer

A)  NaCl 
B)  H2O 
C)  NaOH 
D)  C8H18 
E)  CH3OH 
A)  NaCl 
B)  H2O 
C)  NaOH 
D)  C8H18 
E)  CH3OH

Question 4

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 5

Which of these compounds is a strong electrolyte?

Accepted Answer

A)  H2O 
B)  N2 
C)  CH3COOH (acetic acid) 
D)  C2H6O (ethanol) 
E)  KOH 
A)  H2O 
B)  N2 
C)  CH3COOH (acetic acid) 
D)  C2H6O (ethanol) 
E)  KOH

Question 6

What is the molarity of a 17.0% by mass solution of sodium acetate, NaC2H3O2 (82.0 g/mol), in water? The density of the solution is 1.09 g/mL.

Accepted Answer

A)  0.170 M 
B)  0.207 M 
C)  2.07 M 
D)  2.26 M 
E)  1.90 M 
A)  0.170 M 
B)  0.207 M 
C)  2.07 M 
D)  2.26 M 
E)  1.90 M

Question 7

Which of these compounds is a weak electrolyte?

Accepted Answer

A)  HCl 
B)  CH3COOH (acetic acid) 
C)  C6H12O6 (glucose) 
D)  O2 
E)  NaCl 
A)  HCl 
B)  CH3COOH (acetic acid) 
C)  C6H12O6 (glucose) 
D)  O2 
E)  NaCl

Question 8

What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

Accepted Answer

A)  231 mL 
B)  1.72 L 
C)  1.10 L 
D)  440 mL 
E)  909 mL 
A)  231 mL 
B)  1.72 L 
C)  1.10 L 
D)  440 mL 
E)  909 mL

Question 9

Aqueous ammonia is commercially available in a solution that is 28% (w/w) ammonia. What is the mole fraction of ammonia in such a solution?

Accepted Answer

A)  0.017 
B)  0.023 
C)  0.012 
D)  0.24 
E)  0.29 
A)  0.017 
B)  0.023 
C)  0.012 
D)  0.24 
E)  0.29

Question 10

Which statement is false?

Accepted Answer

A)  The vapor pressure of a solvent over a solution decreases as its mole fraction increases. 
B)  The solubility of a gas increases as the temperature decreases. 
C)  The vapor pressure of a solvent over a solution is less than that of pure solvent. 
D)  The greater the pressure of a gas over a solution, the greater its solubility. 
E)  Ionic solutes dissociate in solution, causing an enhancement of all colligative properties. 
A)  The vapor pressure of a solvent over a solution decreases as its mole fraction increases. 
B)  The solubility of a gas increases as the temperature decreases. 
C)  The vapor pressure of a solvent over a solution is less than that of pure solvent. 
D)  The greater the pressure of a gas over a solution, the greater its solubility. 
E)  Ionic solutes dissociate in solution, causing an enhancement of all colligative properties.

Question 11

A solution containing 0.102 g of an unknown compound dissolved in 100. mL of water has an osmotic pressure of 28.1 mmHg at 20.°C. What is the molar mass of the compound? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg)

Accepted Answer

A)  663 g/mol 
B)  0.872 g/mol 
C)  1.15 g/mol 
D)  727 g/mol 
E)  1.10 × 102 g/mol 
A)  663 g/mol 
B)  0.872 g/mol 
C)  1.15 g/mol 
D)  727 g/mol 
E)  1.10 × 102 g/mol

Question 12

Calcium nitrite is used as a corrosion inhibitor in lubricants. What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

Accepted Answer

A)  0.181 m 
B)  0.222 m 
C)  0.596 m 
D)  1.35 m 
E)  1.68 m 
A)  0.181 m 
B)  0.222 m 
C)  0.596 m 
D)  1.35 m 
E)  1.68 m

Question 13

Colligative properties are properties that depend on the number of solvent particles in solution, but not on the nature of the solvent.

Accepted Answer

A) True 
 B)False

Question 14

What is defined as a solution that has a higher concentration of dissolved substances than plasma?

Accepted Answer

A)  Hypotonic 
B)  Hypertonic 
C)  Aplasmic 
D)  Plasmic 
E)  Colloidal 
A)  Hypotonic 
B)  Hypertonic 
C)  Aplasmic 
D)  Plasmic 
E)  Colloidal

Question 15

If the shell of a raw egg is carefully dissolved away, and the egg in its flexible membrane is then placed in distilled water, the egg's volume will expand. Explain.

Accepted Answer

The osmotic pressure of the solution ins

Question 16

Which substance is present in the smallest proportion in a solution?

Accepted Answer

A)  liquid 
B)  gas 
C)  solvent 
D)  solid 
E)  solute 
A)  liquid 
B)  gas 
C)  solvent 
D)  solid 
E)  solute

Question 17

The structure of Vitamin B1, thiamine, is shown here. Vitamin B1 is most soluble in ________.

Accepted Answer

A)  fats 
B)  water 
C)  air 
D)  carbon tetrachloride 
E)  octane 
A)  fats 
B)  water 
C)  air 
D)  carbon tetrachloride 
E)  octane

Question 18

When two pure substances are mixed to form a solution

Accepted Answer

A)  heat is released. 
B)  heat is absorbed. 
C)  there is an increase in entropy. 
D)  there is a decrease in entropy. 
E)  entropy is conserved. 
A)  heat is released. 
B)  heat is absorbed. 
C)  there is an increase in entropy. 
D)  there is a decrease in entropy. 
E)  entropy is conserved.

Question 19

What is defined as the difference between the freezing point of a pure solvent and the freezing point of the solution?

Accepted Answer

A)  Freezing point 
B)  Freezing-point elevation 
C)  Freezing-point depression 
D)  Subzero freezing 
E)  Supercooling 
A)  Freezing point 
B)  Freezing-point elevation 
C)  Freezing-point depression 
D)  Subzero freezing 
E)  Supercooling

Question 20

Which solution has the highest vapor pressure?

Accepted Answer

A)  0.75 mol of a nonvolatile compound in 750 g of ethanol 
B)  0.75 mol of a volatile compound in 750 g of ethanol 
C)  1.5 mol of a nonvolatile compound in 750 g of ethanol 
D)  Solutions A and B have the same vapor pressure and it is higher than the vapor pressure of solution C. 
E)  Not enough information is given to determine which solution has the highest vapor pressure. 
A)  0.75 mol of a nonvolatile compound in 750 g of ethanol 
B)  0.75 mol of a volatile compound in 750 g of ethanol 
C)  1.5 mol of a nonvolatile compound in 750 g of ethanol 
D)  Solutions A and B have the same vapor pressure and it is higher than the vapor pressure of solution C. 
E)  Not enough information is given to determine which solution has the highest vapor pressure.

Exam 13: Physical Properties of Solutions

Which of the following is not soluble in water?

Which combination of a 36.0% (w/w) stock solution of acetic acid (d = 1.045 g/mL) and water will result in 1.00 kg of a 15.0% (w/w) acetic acid solution?

Which is most soluble in CCl4?

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

Which of these compounds is a strong electrolyte?

What is the molarity of a 17.0% by mass solution of sodium acetate, NaC2H3O2 (82.0 g/mol), in water? The density of the solution is 1.09 g/mL.

Which of these compounds is a weak electrolyte?

What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

Aqueous ammonia is commercially available in a solution that is 28% (w/w) ammonia. What is the mole fraction of ammonia in such a solution?

Which statement is false?

A solution containing 0.102 g of an unknown compound dissolved in 100. mL of water has an osmotic pressure of 28.1 mmHg at 20.°C. What is the molar mass of the compound? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg)

Calcium nitrite is used as a corrosion inhibitor in lubricants. What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

Colligative properties are properties that depend on the number of solvent particles in solution, but not on the nature of the solvent.

What is defined as a solution that has a higher concentration of dissolved substances than plasma?

If the shell of a raw egg is carefully dissolved away, and the egg in its flexible membrane is then placed in distilled water, the egg's volume will expand. Explain.

Which substance is present in the smallest proportion in a solution?

The structure of Vitamin B1, thiamine, is shown here. Vitamin B1 is most soluble in ________.

When two pure substances are mixed to form a solution

What is defined as the difference between the freezing point of a pure solvent and the freezing point of the solution?

Which solution has the highest vapor pressure?

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

Which is most soluble in CCl₄?

What is the molarity of a 17.0% by mass solution of sodium acetate, NaC₂H₃O₂ (82.0 g/mol), in water? The density of the solution is 1.09 g/mL.