Question 1

What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18°C?

Accepted Answer

A) 0.55 atm 
B) 1.10 atm 
C) 8.95 atm 
D) 17.9 atm 
E) 35.9 atm 
A) 0.55 atm 
B) 1.10 atm 
C) 8.95 atm 
D) 17.9 atm 
E) 35.9 atm E

Question 2

The solubility of gases in water usually decreases with

Accepted Answer

A) increasing pressure. 
B) increasing temperature. 
C) decreasing temperature. 
A) increasing pressure. 
B) increasing temperature. 
C) decreasing temperature. B

Question 3

Calculate the molality of a 20.0% by mass ammonium sulfate (NH4)2SO4 solution. The density of the solution is 1.117 g/mL.

Accepted Answer

A) 0.150 m 
B) 1.51 m 
C) 1.70 m 
D) 1.89 m 
E) 2.10 m 
A) 0.150 m 
B) 1.51 m 
C) 1.70 m 
D) 1.89 m 
E) 2.10 m D

Question 4

How many grams of sucrose (C12H22O11, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Accepted Answer

A) 0.57 g 
B) 6.8 g 
C) 2.0 * 102 g 
D) 4.9 * 102 g 
E) 5.8 * 103 g 
A) 0.57 g 
B) 6.8 g 
C) 2.0 * 102 g 
D) 4.9 * 102 g 
E) 5.8 * 103 g

Question 5

A solution of chloroform, CHCl3, and acetone, (CH3)2CO, exhibits a negative deviation from Raoult's law. This result implies that

Accepted Answer

A) chloroform-chloroform interactions are stronger than chloroform-acetone interactions. 
B) chloroform-chloroform interactions are weaker than chloroform-acetone interactions. 
C) acetone-acetone interactions are stronger than chloroform-acetone interactions. 
D) acetone-acetone interactions are weaker than chloroform-acetone interactions. 
E) Both B and D.
F)Both A and C. 
A) chloroform-chloroform interactions are stronger than chloroform-acetone interactions. 
B) chloroform-chloroform interactions are weaker than chloroform-acetone interactions. 
C) acetone-acetone interactions are stronger than chloroform-acetone interactions. 
D) acetone-acetone interactions are weaker than chloroform-acetone interactions. 
E) Both B and D.
F)Both A and C.

Question 6

Define solvation.

Accepted Answer

Solvation is the process in wh

Question 7

To interconvert the concentration units molarity (M)and mass percent, you must also know the density of the solution.

Accepted Answer

A) True 
 B)False

Question 8

What is the molality of a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Question 9

What is the molarity of a solution of 10% by mass cadmium sulfate, CdSO4 (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

Accepted Answer

A) 0.528 M 
B) 0.436 M 
C) 0.479 M 
D) 0.048 M 
E) 22.9 M 
A) 0.528 M 
B) 0.436 M 
C) 0.479 M 
D) 0.048 M 
E) 22.9 M

Question 10

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?

Accepted Answer

A) 769 g 
B) 36.2 g 
C) 100.g 
D) 0.157 g 
E) 157 g 
A) 769 g 
B) 36.2 g 
C) 100.g 
D) 0.157 g 
E) 157 g

Question 11

Which of the following aqueous solutions has the highest boiling point? Kb for water is 0.52°C/m.

Accepted Answer

A) 0.2 m KCl 
B) 0.2 m Na2SO4 
C) 0.2 m Ca(NO3)2 
D) A and B. 
E) B and C. 
A) 0.2 m KCl 
B) 0.2 m Na2SO4 
C) 0.2 m Ca(NO3)2 
D) A and B. 
E) B and C.

Question 12

What is the mass percent CH3OH of a 0.256 m CH3OH(aq)solution.

Accepted Answer

A) 0.814 % 
B) 0.992 % 
C) 1.23 % 
D) 1.29 % 
E) 1.51 % 
A) 0.814 % 
B) 0.992 % 
C) 1.23 % 
D) 1.29 % 
E) 1.51 %

Question 13

A saturated solution

Accepted Answer

A) contains more solute than solvent. 
B) contains more solvent than solute. 
C) contains equal moles of solute and solvent. 
D) contains the maximum amount of solute that will dissolve in that solvent at that temperature. 
E) contains a solvent with only sigma bonds and no pi bonds (i.e.only single bonds, with no double or triple bonds). 
A) contains more solute than solvent. 
B) contains more solvent than solute. 
C) contains equal moles of solute and solvent. 
D) contains the maximum amount of solute that will dissolve in that solvent at that temperature. 
E) contains a solvent with only sigma bonds and no pi bonds (i.e.only single bonds, with no double or triple bonds).

Question 14

Some KCl is dissolved in water 25°C, where it completely dissociates.The vapor pressure of pure water at 25°C is 28.3 mmHg. On the graph below, sketch the vapor pressure above the salt solution as a function of the mole fraction of H2O, assuming that Raoult's law is obeyed. Explain how you arrived at your graph.

Accepted Answer

@#IMG-DLM& Pure water has a vapor pressu

Question 15

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

Accepted Answer

The answer of A 100.-mL sample of water is taken...

Question 16

In the course of research, a chemist isolates a new compound with an empirical formula C3H3O2. Dissolving 2.51 g of the compound in 100.g of water produces a solution with a freezing point of -0.325S1U1P1$\circ$S1S1P0C. What is the molecular formula of the compound? (For water, Kf = 1.86°C/m.)

Accepted Answer

C<sub>6</s

Question 17

Which of the following gives the molarity of a 17.0% by mass solution of sodium acetate, CH3COONa (molar mass = 82.0 g/mol)in water? The density of the solution is 1.09 g/mL.

Accepted Answer

A) 2.26 * 10-6 M 
B) 0.207 M 
C) 2.07 M 
D) 2.26 M 
E) 2.72 M 
A) 2.26 * 10-6 M 
B) 0.207 M 
C) 2.07 M 
D) 2.26 M 
E) 2.72 M

Question 18

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, what is the molality, m, of aspirin in your blood? (Assume density of plasma is 1.00 g/mL.)

Accepted Answer

2.99 * 10<

Question 19

In how many grams of water should 25.31 g of potassium nitrate (KNO3)be dissolved to prepare a 0.1982 m solution?

Accepted Answer

A) 250.0 g 
B) 792.0 g 
C) 1,000.g 
D) 1,263 g 
E) 7,917 g 
A) 250.0 g 
B) 792.0 g 
C) 1,000.g 
D) 1,263 g 
E) 7,917 g

Question 20

The solubility of gases in water always decreases with increasing temperature.

Accepted Answer

A) True 
 B)False

Exam 12: Physical Properties of Solutions

What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18°C?

The solubility of gases in water usually decreases with

Calculate the molality of a 20.0% by mass ammonium sulfate (NH4)2SO4 solution. The density of the solution is 1.117 g/mL.

How many grams of sucrose (C12H22O11, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol)

A solution of chloroform, CHCl3, and acetone, (CH3)2CO, exhibits a negative deviation from Raoult's law. This result implies that

Define solvation.

To interconvert the concentration units molarity (M)and mass percent, you must also know the density of the solution.

What is the molality of a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

What is the molarity of a solution of 10% by mass cadmium sulfate, CdSO4 (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?

Which of the following aqueous solutions has the highest boiling point? Kb for water is 0.52°C/m.

What is the mass percent CH3OH of a 0.256 m CH3OH(aq)solution.

A saturated solution

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.

In the course of research, a chemist isolates a new compound with an empirical formula C3H3O2. Dissolving 2.51 g of the compound in 100.g of water produces a solution with a freezing point of -0.325 ∘\circ∘ C. What is the molecular formula of the compound? (For water, Kf = 1.86°C/m.)

Which of the following gives the molarity of a 17.0% by mass solution of sodium acetate, CH3COONa (molar mass = 82.0 g/mol)in water? The density of the solution is 1.09 g/mL.

In how many grams of water should 25.31 g of potassium nitrate (KNO3)be dissolved to prepare a 0.1982 m solution?

The solubility of gases in water always decreases with increasing temperature.

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

Calculate the molality of a 20.0% by mass ammonium sulfate (NH₄)₂SO₄ solution. The density of the solution is 1.117 g/mL.

How many grams of sucrose (C₁₂H₂₂O₁₁, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol)

A solution of chloroform, CHCl₃, and acetone, (CH₃)₂CO, exhibits a negative deviation from Raoult's law. This result implies that

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

What is the molarity of a solution of 10% by mass cadmium sulfate, CdSO₄ (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?

Which of the following aqueous solutions has the highest boiling point? K_b for water is 0.52°C/m.

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq)solution.

In the course of research, a chemist isolates a new compound with an empirical formula C₃H₃O₂. Dissolving 2.51 g of the compound in 100.g of water produces a solution with a freezing point of -0.325^$\circ$C. What is the molecular formula of the compound? (For water, K_f = 1.86°C/m.)

Which of the following gives the molarity of a 17.0% by mass solution of sodium acetate, CH₃COONa (molar mass = 82.0 g/mol)in water? The density of the solution is 1.09 g/mL.

In how many grams of water should 25.31 g of potassium nitrate (KNO₃)be dissolved to prepare a 0.1982 m solution?