Question 1

A solution containing 100.0 g of NaCl per liter has a density of 1.095 g/mL. What is the molality of the solution?

Accepted Answer

A)  0.5873 m 
B)  1.711 m 
C)  1.720 m 
D)  0.5844 m 
E)  none of these 
A)  0.5873 m 
B)  1.711 m 
C)  1.720 m 
D)  0.5844 m 
E)  none of these

Question 2

Pentane (C5H12) and hexane (C6H14) form an ideal solution. The vapor pressures of pentane and hexane at 25° C are 511 torr and 150 torr, respectively. The mole fraction of hexane in a pentane-hexane solution is 0.50. Calculate the mole fraction of pentane in the vapor that is in equilibrium at 25°C with this solution.

Accepted Answer

A)  0.23 
B)  0.77 
C)  0.89 
D)  0.50 
E)  none of these 
A)  0.23 
B)  0.77 
C)  0.89 
D)  0.50 
E)  none of these

Question 3

Consider that 45.0 g of a protein has been dissolved in 1.00 L of aqueous solution. The osmotic pressure of the solution at 25°C is 12.7 torr. What is the approximate molar mass of the protein?

Accepted Answer

6.59 *10<s

Question 4

When a nonvolatile solute is added to a volatile solvent, the solution vapor pressure __________, the boiling point __________, the freezing point __________, and the osmotic pressure across a semipermeable membrane __________.

Accepted Answer

A)  decreases, decreases, increases, decreases 
B)  increases, decreases, increases, decreases 
C)  decreases, increases, decreases, increases 
D)  increases, increases, decreases, increases 
E)  decreases, increases, decreases, decreases 
A)  decreases, decreases, increases, decreases 
B)  increases, decreases, increases, decreases 
C)  decreases, increases, decreases, increases 
D)  increases, increases, decreases, increases 
E)  decreases, increases, decreases, decreases

Question 5

At a given temperature, you have a mixture of benzene (vapor pressure of pure benzene = 745 torr) and toluene (vapor pressure of pure toluene = 290 torr). The mole fraction of benzene in the vapor above the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the solution.

Accepted Answer

A)  0.778 
B)  0.359 
C)  0.213 
D)  0.590 
E)  0.641 
A)  0.778 
B)  0.359 
C)  0.213 
D)  0.590 
E)  0.641

Question 6

When a 1.50-g sample of glutamic acid is dissolved in 100.0 g of H2O, the resulting solution freezes at -0.190°C. Kf for H2O is 1.86°C/m. The molar mass of glutamic acid is

Accepted Answer

A)  28.0 g/mol 
B)  147 g/mol 
C)  1.50 g/mol 
D)  189 g/mol 
E)  14.7 g/mol 
A)  28.0 g/mol 
B)  147 g/mol 
C)  1.50 g/mol 
D)  189 g/mol 
E)  14.7 g/mol

Question 7

When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L of solution, [H+] is 1.8 F1F1F1S1F1F1F1010-3 M. Calculate the freezing point of this solution. Assume that the molarity concentration is equal to the molality concentration, and assume ideal behavior. Kf (H2O) is 1.86°C kg/mol.

Accepted Answer

A)  -0.058°C 
B)  -0.029°C 
C)  -0.026°C 
D)  +0.029°C 
E)  +0.026°C 
A)  -0.058°C 
B)  -0.029°C 
C)  -0.026°C 
D)  +0.029°C 
E)  +0.026°C

Question 8

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

Accepted Answer

A)  I < II < IV < III 
B)  I < III < IV < II 
C)  I < II < III < IV 
D)  III < IV < II < I 
E)  None is correct. 
A)  I < II < IV < III 
B)  I < III < IV < II 
C)  I < II < III < IV 
D)  III < IV < II < I 
E)  None is correct.

Question 9

What is the molar mass of glucose if 22.5 g gives a freezing point of -0.930°C when dissolved in 250.0 g of water? If the empirical formula is CH2O, what is the molecular formula?

Accepted Answer

Question 10

The freezing-point depression of a 3.00 *10-3 M solution of a weak acid HA is 6.67* 10-3 °C in water. Assuming that the molarity concentration and the molality concentration are the same and assuming ideal behavior, calculate Ka for the weak acid. Kf(H2O) = 1.86 °C kg/mol.

Accepted Answer

1.4 * 10<s

Question 11

Predict the deviation from Raoult's law when two liquids are mixed and the heat of the solution is small.

Accepted Answer

A)  negative deviation 
B)  relatively ideal (small or zero deviation) 
C)  positive deviation 
A)  negative deviation 
B)  relatively ideal (small or zero deviation) 
C)  positive deviation

Question 12

When 271.0 mL of 0.828 M HCl is diluted with 161.6 mL of water, the molarity of the solution (assuming the volumes are additive) is

Accepted Answer

A)  0.519 M. 
B)  0.111 M. 
C)  0.00191 M. 
D)  0.309 M. 
E)  1.39 M. 
A)  0.519 M. 
B)  0.111 M. 
C)  0.00191 M. 
D)  0.309 M. 
E)  1.39 M.

Question 13

The molal freezing-point depression constants for benzene and water are 5.12 and 1.86, respectively. When 4.6 g of formic acid (HCOOH) is dissolved in 1.0 kg of benzene, the freezing point is depressed by 0.26°C. When the same amount of formic acid is dissolved in 1.0 kg of water, the freezing point is lowered by 0.19°C. To explain these results, we must assume that

Accepted Answer

A)  formic acid is monomeric in benzene and associated in water. 
B)  formic acid is associated in benzene and monomeric in water. 
C)  formic acid is monomeric in benzene and dissociated in water. 
D)  formic acid is dissociated in benzene and monomeric in water. 
A)  formic acid is monomeric in benzene and associated in water. 
B)  formic acid is associated in benzene and monomeric in water. 
C)  formic acid is monomeric in benzene and dissociated in water. 
D)  formic acid is dissociated in benzene and monomeric in water.

Question 14

Acetone (mw = 58.08, P   =232 mmHg) and butanone (mw = 72.11, P   =100 mmHg) have the indicated molar masses and vapor pressures. A container holds 1.00 kg of butanone. How much acetone must be added to the butanone to elevate the total vapor pressure over the mixture to 125 mmHg at 25°C?

Accepted Answer

A)  5.313 kg 
B)  290 g 
C)  188 g 
D)  More information needed 
E)  None of the above 
A)  5.313 kg 
B)  290 g 
C)  188 g 
D)  More information needed 
E)  None of the above

Question 15

Diagram and label a vapor pressure diagram for an ideal solution of two volatile liquids. Indicate the deviation predicted by an endothermic heat of solution.

Accepted Answer

positive deviation;

Question 16

How many moles of methanol, CH3OH, dissolved in 450.0 g of water are needed to make a 2.500 m solution?

Accepted Answer

Question 17

Predict the deviation from Raoult's law when two liquids are mixed and the heat of the solution is large and the reaction exothermic.

Accepted Answer

A)  positive deviation 
B)  relatively ideal (small or zero deviation) 
C)  negative deviation 
A)  positive deviation 
B)  relatively ideal (small or zero deviation) 
C)  negative deviation

Question 18

A 5.00-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 25 torr at 25°C. If it is assumed that each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of this solute?

Accepted Answer

A)  18,600 g/mol 
B)  37,200 g/mol 
C)  74,300 g/mol 
D)  1560 g/mol 
E)  none of these 
A)  18,600 g/mol 
B)  37,200 g/mol 
C)  74,300 g/mol 
D)  1560 g/mol 
E)  none of these

Question 19

A 5.96-g sample of a compound is dissolved in 222.0 g of benzene. The freezing point of this solution is 1.06°C below that of pure benzene. What is the molar mass of this compound? (Note: Kf for benzene = 5.12°C/m.)

Accepted Answer

A)  1.30 F1F1F1S1F1F1F10 102 g/mol 
B)  2.85 F1F1F1S1F1F1F10 101 g/mol 
C)  1.80 F1F1F1S1F1F1F10 102 g/mol 
D)  6.39 F1F1F1S1F1F1F10 103 g/mol 
E)  5.56 F1F1F1S1F1F1F10 102 g/mol 
A)  1.30 F1F1F1S1F1F1F10 102 g/mol 
B)  2.85 F1F1F1S1F1F1F10 101 g/mol 
C)  1.80 F1F1F1S1F1F1F10 102 g/mol 
D)  6.39 F1F1F1S1F1F1F10 103 g/mol 
E)  5.56 F1F1F1S1F1F1F10 102 g/mol

Question 20

When 100.0 g of a compound is dissolved in 1500. g of water, the freezing point of the solution is lowered to -1.35°C. Determine the molar mass of the compound.

Accepted Answer

The answer of When 100.0 g of a compound is...

A solution containing 100.0 g of NaCl per liter has a density of 1.095 g/mL. What is the molality of the solution?

Consider that 45.0 g of a protein has been dissolved in 1.00 L of aqueous solution. The osmotic pressure of the solution at 25°C is 12.7 torr. What is the approximate molar mass of the protein?

When a nonvolatile solute is added to a volatile solvent, the solution vapor pressure , the boiling point , the freezing point , and the osmotic pressure across a semipermeable membrane .

When a 1.50-g sample of glutamic acid is dissolved in 100.0 g of H₂O, the resulting solution freezes at -0.190°C. K_f for H₂O is 1.86°C/m. The molar mass of glutamic acid is

When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L of solution, [H⁺] is 1.8 10^-3 M. Calculate the freezing point of this solution. Assume that the molarity concentration is equal to the molality concentration, and assume ideal behavior. K_f (H₂O) is 1.86°C kg/mol.

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

What is the molar mass of glucose if 22.5 g gives a freezing point of -0.930°C when dissolved in 250.0 g of water? If the empirical formula is CH₂O, what is the molecular formula?

The freezing-point depression of a 3.00 10^-³ M solution of a weak acid HA is 6.67 10^-³ °C in water. Assuming that the molarity concentration and the molality concentration are the same and assuming ideal behavior, calculate K_a for the weak acid. K_f(H₂O) = 1.86 °C kg/mol.

Predict the deviation from Raoult's law when two liquids are mixed and the heat of the solution is small.

When 271.0 mL of 0.828 M HCl is diluted with 161.6 mL of water, the molarity of the solution (assuming the volumes are additive) is

Acetone (mw = 58.08, P =232 mmHg) and butanone (mw = 72.11, P =100 mmHg) have the indicated molar masses and vapor pressures. A container holds 1.00 kg of butanone. How much acetone must be added to the butanone to elevate the total vapor pressure over the mixture to 125 mmHg at 25°C?

Diagram and label a vapor pressure diagram for an ideal solution of two volatile liquids. Indicate the deviation predicted by an endothermic heat of solution.

How many moles of methanol, CH₃OH, dissolved in 450.0 g of water are needed to make a 2.500 m solution?

Predict the deviation from Raoult's law when two liquids are mixed and the heat of the solution is large and the reaction exothermic.

A 5.00-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 25 torr at 25°C. If it is assumed that each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of this solute?

A 5.96-g sample of a compound is dissolved in 222.0 g of benzene. The freezing point of this solution is 1.06°C below that of pure benzene. What is the molar mass of this compound? (Note: K_f for benzene = 5.12°C/m.)

When 100.0 g of a compound is dissolved in 1500. g of water, the freezing point of the solution is lowered to -1.35°C. Determine the molar mass of the compound.

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Exam 17: Properties of Solutions

A solution containing 100.0 g of NaCl per liter has a density of 1.095 g/mL. What is the molality of the solution?

Consider that 45.0 g of a protein has been dissolved in 1.00 L of aqueous solution. The osmotic pressure of the solution at 25°C is 12.7 torr. What is the approximate molar mass of the protein?

When a nonvolatile solute is added to a volatile solvent, the solution vapor pressure __________, the boiling point __________, the freezing point __________, and the osmotic pressure across a semipermeable membrane __________.

When a 1.50-g sample of glutamic acid is dissolved in 100.0 g of H2O, the resulting solution freezes at -0.190°C. Kf for H2O is 1.86°C/m. The molar mass of glutamic acid is

When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L of solution, [H+] is 1.8 10-3 M. Calculate the freezing point of this solution. Assume that the molarity concentration is equal to the molality concentration, and assume ideal behavior. Kf (H2O) is 1.86°C kg/mol.

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

What is the molar mass of glucose if 22.5 g gives a freezing point of -0.930°C when dissolved in 250.0 g of water? If the empirical formula is CH2O, what is the molecular formula?

The freezing-point depression of a 3.00 *10-3 M solution of a weak acid HA is 6.67* 10-3 °C in water. Assuming that the molarity concentration and the molality concentration are the same and assuming ideal behavior, calculate Ka for the weak acid. Kf(H2O) = 1.86 °C kg/mol.

Predict the deviation from Raoult's law when two liquids are mixed and the heat of the solution is small.

When 271.0 mL of 0.828 M HCl is diluted with 161.6 mL of water, the molarity of the solution (assuming the volumes are additive) is

Acetone (mw = 58.08, P =232 mmHg) and butanone (mw = 72.11, P =100 mmHg) have the indicated molar masses and vapor pressures. A container holds 1.00 kg of butanone. How much acetone must be added to the butanone to elevate the total vapor pressure over the mixture to 125 mmHg at 25°C?

Diagram and label a vapor pressure diagram for an ideal solution of two volatile liquids. Indicate the deviation predicted by an endothermic heat of solution.

How many moles of methanol, CH3OH, dissolved in 450.0 g of water are needed to make a 2.500 m solution?

Predict the deviation from Raoult's law when two liquids are mixed and the heat of the solution is large and the reaction exothermic.

A 5.00-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 25 torr at 25°C. If it is assumed that each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of this solute?

A 5.96-g sample of a compound is dissolved in 222.0 g of benzene. The freezing point of this solution is 1.06°C below that of pure benzene. What is the molar mass of this compound? (Note: Kf for benzene = 5.12°C/m.)

When 100.0 g of a compound is dissolved in 1500. g of water, the freezing point of the solution is lowered to -1.35°C. Determine the molar mass of the compound.

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Quantum Mechanics and Atomic Theory

Bonding: General Concepts

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When a nonvolatile solute is added to a volatile solvent, the solution vapor pressure , the boiling point , the freezing point , and the osmotic pressure across a semipermeable membrane .

When a 1.50-g sample of glutamic acid is dissolved in 100.0 g of H₂O, the resulting solution freezes at -0.190°C. K_f for H₂O is 1.86°C/m. The molar mass of glutamic acid is

When 0.014 mol of a weak acid HA is dissolved in enough water to make 1.0 L of solution, [H⁺] is 1.8 10^-3 M. Calculate the freezing point of this solution. Assume that the molarity concentration is equal to the molality concentration, and assume ideal behavior. K_f (H₂O) is 1.86°C kg/mol.

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

What is the molar mass of glucose if 22.5 g gives a freezing point of -0.930°C when dissolved in 250.0 g of water? If the empirical formula is CH₂O, what is the molecular formula?

The freezing-point depression of a 3.00 10^-³ M solution of a weak acid HA is 6.67 10^-³ °C in water. Assuming that the molarity concentration and the molality concentration are the same and assuming ideal behavior, calculate K_a for the weak acid. K_f(H₂O) = 1.86 °C kg/mol.

How many moles of methanol, CH₃OH, dissolved in 450.0 g of water are needed to make a 2.500 m solution?

A 5.96-g sample of a compound is dissolved in 222.0 g of benzene. The freezing point of this solution is 1.06°C below that of pure benzene. What is the molar mass of this compound? (Note: K_f for benzene = 5.12°C/m.)