Question 1

Explain the following, on the basis of osmosis or osmotic pressure: An effective way to kill a snail or slug in your garden is to sprinkle it with salt.

Accepted Answer

The water leaves the

Question 2

The density of a 20.3 M CH3OH (methanol)solution is 0.858 g/mL. What is the molality of this solution? H2O is the solvent.

Accepted Answer

A) 17.4 m 
B) 20.8 m 
C) 23.7 m 
D) 70.0 m 
E) 97.6 m 
A) 17.4 m 
B) 20.8 m 
C) 23.7 m 
D) 70.0 m 
E) 97.6 m

Question 3

Dissolving a solute such as KOH in a solvent such as water results in

Accepted Answer

A) an increase in the melting point of the liquid. 
B) a decrease in the boiling point of the liquid. 
C) a decrease in the vapor pressure of the liquid. 
D) no change in the boiling point of the liquid. 
A) an increase in the melting point of the liquid. 
B) a decrease in the boiling point of the liquid. 
C) a decrease in the vapor pressure of the liquid. 
D) no change in the boiling point of the liquid.

Question 4

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

Accepted Answer

A) 0.03097 M 
B) 0.4133 M 
C) 0.4646 M 
D) 1.590 M 
E) 3.097 M 
A) 0.03097 M 
B) 0.4133 M 
C) 0.4646 M 
D) 1.590 M 
E) 3.097 M

Question 5

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. The density of water is 0.997 g/mL.

Accepted Answer

A) 1.51 % 
B) 7.57 % 
C) 13.3 % 
D) 15.2 % 
E) None of these 
A) 1.51 % 
B) 7.57 % 
C) 13.3 % 
D) 15.2 % 
E) None of these

Question 6

What volume of water should be added to 600.mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, Kb = 1.22 °C/m, density = 0.789 g/cm3, boiling point = 78.4°C)

Accepted Answer

A) 186 mL 
B) 245 mL 
C) 518 mL 
D) 116 mL 
E) 322 mL 
A) 186 mL 
B) 245 mL 
C) 518 mL 
D) 116 mL 
E) 322 mL

Question 7

The solubility of CO2 gas in water

Accepted Answer

A) increases with increasing gas pressure. 
B) increases with decreasing gas pressure. 
C) decreases with increasing gas pressure. 
D) is not dependent on pressure. 
A) increases with increasing gas pressure. 
B) increases with decreasing gas pressure. 
C) decreases with increasing gas pressure. 
D) is not dependent on pressure.

Question 8

What is the molarity of a solution that is 7.00% by mass magnesium sulfate and has a density of 1.071 g/mL?

Accepted Answer

A) 0.0890 M 
B) 0.496 M 
C) 0.543 M 
D) 0.623 M 
E) 1.32 M 
A) 0.0890 M 
B) 0.496 M 
C) 0.543 M 
D) 0.623 M 
E) 1.32 M

Question 9

For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

Accepted Answer

A) True 
 B)False

Question 10

What volume of ethanol (density = 0.7893 g/cm3)should be added to 450.mL of water in order to have a solution that freezes at -15.0°C? (For water, Kf = 1.86 °C/m.)

Accepted Answer

A) 371 mL 
B) 470 mL 
C) 212 mL 
D) 132 mL 
E) 167 mL 
A) 371 mL 
B) 470 mL 
C) 212 mL 
D) 132 mL 
E) 167 mL

Question 11

In which of the following solvents would you expect KBr to be most soluble?

Accepted Answer

A) C6H14 (hexane) 
B) CH3CH2OH (ethanol) 
C) C6H6 (benzene) 
D) CCl4 (carbon tetrachloride) 
E) C6H12 (cyclohexane) 
A) C6H14 (hexane) 
B) CH3CH2OH (ethanol) 
C) C6H6 (benzene) 
D) CCl4 (carbon tetrachloride) 
E) C6H12 (cyclohexane)

Question 12

What is the freezing point of a solution that contains 10.0 g of glucose (C6H12O6)in 100.g of H2O? Kf for water is 1.86°C/m.

Accepted Answer

A) -0.186°C 
B) +0.186°C 
C) -0.10°C 
D) +0.10°C 
E) -1.03°C 
A) -0.186°C 
B) +0.186°C 
C) -0.10°C 
D) +0.10°C 
E) -1.03°C

Question 13

Which one of the following would be immiscible with water?

Accepted Answer

The answer of Which one of the following would be...

Question 14

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO3)2; 0.100 m ethanol; 0.090 m NaCl.

Accepted Answer

A) Mg(NO3)2 3)2 3)2 
D) NaCl 3)2 
E) Mg(NO3)2 < ethanol < NaCl 
A) Mg(NO3)2 3)2 3)2 
D) NaCl 3)2 
E) Mg(NO3)2 < ethanol < NaCl

Question 15

What is the molality of a solution that is 3.68 % by mass calcium chloride.

Accepted Answer

A) 0.0332 m 
B) 0.332 m 
C) 0.344 m 
D) 0.464 m 
E) 0.506 m 
A) 0.0332 m 
B) 0.332 m 
C) 0.344 m 
D) 0.464 m 
E) 0.506 m

Question 16

A 9.50 % by mass solution of acetone (C3H6O)in water has a density of 0.9849 g/mL at 20°C.What is the molarity of this solution?

Accepted Answer

A) 0.621 M 
B) 1.61 M 
C) 1.66 M 
D) 1.71 M 
E) 16.9 M 
A) 0.621 M 
B) 1.61 M 
C) 1.66 M 
D) 1.71 M 
E) 16.9 M

Question 17

Plasma is the fluid portion of blood.The concentration of acetylsalicylic acid (aspirin, C9H8O4, molar mass = 180.g/mol)in your plasma is found to be 2.99 * 10-4 M after you take two tablets of aspirin.If the volume of your plasma is 5.85 L, how many grams of aspirin are in your blood? (Assume that the density of plasma is 1.00 g/mL.)

Accepted Answer

The answer of Plasma is the fluid portion of blood.The...

Question 18

According to Raoult's law, 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 19

What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 g/mL?

Accepted Answer

A) 3.87 * 10-4 % 
B) 3.87 * 10-1 % 
C) 11.0 % 
D) 1.10 % 
E) 6.50 * 10-2  % 
A) 3.87 * 10-4 % 
B) 3.87 * 10-1 % 
C) 11.0 % 
D) 1.10 % 
E) 6.50 * 10-2  %

Question 20

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

Accepted Answer

Exam 12: Physical Properties of Solutions

Explain the following, on the basis of osmosis or osmotic pressure: An effective way to kill a snail or slug in your garden is to sprinkle it with salt.

The density of a 20.3 M CH3OH (methanol)solution is 0.858 g/mL. What is the molality of this solution? H2O is the solvent.

Dissolving a solute such as KOH in a solvent such as water results in

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. The density of water is 0.997 g/mL.

What volume of water should be added to 600.mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, Kb = 1.22 °C/m, density = 0.789 g/cm3, boiling point = 78.4°C)

The solubility of CO2 gas in water

What is the molarity of a solution that is 7.00% by mass magnesium sulfate and has a density of 1.071 g/mL?

For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

What volume of ethanol (density = 0.7893 g/cm3)should be added to 450.mL of water in order to have a solution that freezes at -15.0°C? (For water, Kf = 1.86 °C/m.)

In which of the following solvents would you expect KBr to be most soluble?

What is the freezing point of a solution that contains 10.0 g of glucose (C6H12O6)in 100.g of H2O? Kf for water is 1.86°C/m.

Which one of the following would be immiscible with water?

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO3)2; 0.100 m ethanol; 0.090 m NaCl.

What is the molality of a solution that is 3.68 % by mass calcium chloride.

A 9.50 % by mass solution of acetone (C3H6O)in water has a density of 0.9849 g/mL at 20°C.What is the molarity of this solution?

According to Raoult's law, which statement is false?

What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 g/mL?

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

Chemistry: The Study of Change

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

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Quantum Theory and the Electronic Structure of Atoms

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Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

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Acid-Base Equilibria and Solubility Equilibria

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The density of a 20.3 M CH₃OH (methanol)solution is 0.858 g/mL. What is the molality of this solution? H₂O is the solvent.

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C.What is the molarity of this solution?

Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO₃ and 295 mL of water. The density of water is 0.997 g/mL.

What volume of water should be added to 600.mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, K_b = 1.22 °C/m, density = 0.789 g/cm³, boiling point = 78.4°C)

The solubility of CO₂ gas in water

What volume of ethanol (density = 0.7893 g/cm³)should be added to 450.mL of water in order to have a solution that freezes at -15.0°C? (For water, K_f = 1.86 °C/m.)

What is the freezing point of a solution that contains 10.0 g of glucose (C₆H₁₂O₆)in 100.g of H₂O? K_f for water is 1.86°C/m.

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃)₂; 0.100 m ethanol; 0.090 m NaCl.

A 9.50 % by mass solution of acetone (C₃H₆O)in water has a density of 0.9849 g/mL at 20°C.What is the molarity of this solution?

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.