Question 1

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 2

What is the boiling point of a solution of 12.0 g of urea (CH4N2O)in 165.0 g of water? (Kb (H2O)= 0.52 °C/m)

Accepted Answer

A) 99.4°C 
B) 100.0 °C 
C) 100.6°C 
D) 106.2°C 
E) 108.4°C 
A) 99.4°C 
B) 100.0 °C 
C) 100.6°C 
D) 106.2°C 
E) 108.4°C

Question 3

Calculate the molality of 6.0 M H2SO4 solution.The density of the solution is 1.34 g/mL.

Accepted Answer

A) 4.48 m 
B) 7.98 m 
C) 8.10 m 
D) 8.43 m 
E) 10.2 m 
A) 4.48 m 
B) 7.98 m 
C) 8.10 m 
D) 8.43 m 
E) 10.2 m

Question 4

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10-4 mol/L.What is the value of the Henry's Law constant in mol/L·atm?

Accepted Answer

A) 9.0 × 10-7 mol/L·atm 
B) 3.2 × 10-4 mol/L·atm 
C) 4.7 × 10-4 mol/L·atm 
D) 6.8 × 10-4 mol/L·atm 
E) 1.5 × 103 mol/L·atm 
A) 9.0 × 10-7 mol/L·atm 
B) 3.2 × 10-4 mol/L·atm 
C) 4.7 × 10-4 mol/L·atm 
D) 6.8 × 10-4 mol/L·atm 
E) 1.5 × 103 mol/L·atm

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

Arrange the following aqueous solutions in order of increasing boiling points: 0.050m Mg(NO3)2; 0.100m ethanol; 0.090m 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 7

During osmosis

Accepted Answer

A) pure solvent diffuses through a membrane but solutes do not. 
B) pure solutes diffuse through a membrane but solvent does not. 
C) pure solvent and a solution both diffuse at the same time through a membrane. 
D) gases diffuse through a membrane into a solution and build up pressure. 
A) pure solvent diffuses through a membrane but solutes do not. 
B) pure solutes diffuse through a membrane but solvent does not. 
C) pure solvent and a solution both diffuse at the same time through a membrane. 
D) gases diffuse through a membrane into a solution and build up pressure.

Question 8

The solubility of a solid always increases with increasing solvent temperature.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following solutions has the largest molality of HCl?

Accepted Answer

A) 4.5 m HCl 
B) mole fraction, X = 0.110 HCl 
C) 15.0 mass % HCl 
D) 10.5 g HCl in 750 g of H2O 
E) 3.6 moles HCl in 45.0 moles of H2O 
A) 4.5 m HCl 
B) mole fraction, X = 0.110 HCl 
C) 15.0 mass % HCl 
D) 10.5 g HCl in 750 g of H2O 
E) 3.6 moles HCl in 45.0 moles of H2O

Question 10

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 11

Which of the following aqueous solutions has the largest molality of benzoic acid (C6H5COOH)?

Accepted Answer

A) 3.5 m C6H5COOH 
B) mole fraction, X = 0.050 C6H5COOH 
C) 2.50 mass % C6H5COOH 
D) 3.2 g C6H5COOH in 650.g of H2O 
E) 1.5 moles C6H5COOH in 65.0 moles of H2O 
A) 3.5 m C6H5COOH 
B) mole fraction, X = 0.050 C6H5COOH 
C) 2.50 mass % C6H5COOH 
D) 3.2 g C6H5COOH in 650.g of H2O 
E) 1.5 moles C6H5COOH in 65.0 moles of H2O

Question 12

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 13

Using your knowledge of osmosis or osmotic pressure explain the following statement: When sprinkled with sugar, a dish of sliced fruit will form its own juice.

Accepted Answer

The water inside the fruit cel

Question 14

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

Question 15

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

Question 16

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 17

A 23.0% by mass LiCl solution is prepared in water.What is the mole fraction of the water?

Accepted Answer

A) 0.113 
B) 0.127 
C) 0.873 
D) 0.887 
E) 0.911 
A) 0.113 
B) 0.127 
C) 0.873 
D) 0.887 
E) 0.911

Question 18

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

Accepted Answer

A) True 
 B)False

Question 19

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2)and 85.0 g H2O? Kf of water is 1.86°C/m.

Accepted Answer

A) 17.6°C 
B) 1.50°C 
C) -1.50°C 
D) -17.6°C 
E) -176°C 
A) 17.6°C 
B) 1.50°C 
C) -1.50°C 
D) -17.6°C 
E) -176°C

Question 20

Using your knowledge of osmosis or osmotic pressure explain the following statement: In trees and plants water is drawn from the soil up into the branches and leaves.

Accepted Answer

The water passes into the cell

Exam 12: Physical Properties of Solutions

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?

What is the boiling point of a solution of 12.0 g of urea (CH4N2O)in 165.0 g of water? (Kb (H2O)= 0.52 °C/m)

Calculate the molality of 6.0 M H2SO4 solution.The density of the solution is 1.34 g/mL.

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10-4 mol/L.What is the value of the Henry's Law constant in mol/L·atm?

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?

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

During osmosis

The solubility of a solid always increases with increasing solvent temperature.

Which of the following solutions has the largest molality of HCl?

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?

Which of the following aqueous solutions has the largest molality of benzoic acid (C6H5COOH)?

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

Using your knowledge of osmosis or osmotic pressure explain the following statement: When sprinkled with sugar, a dish of sliced fruit will form its own juice.

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.

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.

A 23.0% by mass LiCl solution is prepared in water.What is the mole fraction of the water?

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

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2)and 85.0 g H2O? Kf of water is 1.86°C/m.

Using your knowledge of osmosis or osmotic pressure explain the following statement: In trees and plants water is drawn from the soil up into the branches and leaves.

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

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

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

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?

What is the boiling point of a solution of 12.0 g of urea (CH₄N₂O)in 165.0 g of water? (K_b (H₂O)= 0.52 °C/m)

Calculate the molality of 6.0 M H₂SO₄ solution.The density of the solution is 1.34 g/mL.

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10^-4 mol/L.What is the value of the Henry's Law constant in mol/L·atm?

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?

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

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?

Which of the following aqueous solutions has the largest molality of benzoic acid (C₆H₅COOH)?

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.

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.

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.