Question 1

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 2

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO4 solution.

Accepted Answer

A) 0.013 
B) 1.3 
C) 1.5 
D) 2.0 
E) 76.8 
A) 0.013 
B) 1.3 
C) 1.5 
D) 2.0 
E) 76.8

Question 3

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

Question 4

Which of the following compounds should be soluble in CCl4?

Accepted Answer

A) NaCl 
B) H2O 
C) NaOH 
D) C8H18 
E) None of these 
A) NaCl 
B) H2O 
C) NaOH 
D) C8H18 
E) None of these

Question 5

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 6

Which of the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality?

Accepted Answer

Percent mass, mole f

Question 7

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 8

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 9

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 10

What is the percent CdSO4 by mass in a 1.0 molal aqueous CdSO4 solution?

Accepted Answer

A) 1.00 * 10-3 % 
B) 0.100 % 
C) 17.2 % 
D) 20.8 % 
E) 24.4 % 
A) 1.00 * 10-3 % 
B) 0.100 % 
C) 17.2 % 
D) 20.8 % 
E) 24.4 %

Question 11

Consider a 0.90 M Al(NO3)3 solution. This solution has a nitrate ion concentration of

Accepted Answer

A) 0.30 M. 
B) 0.90 M. 
C) 0.0 M. 
D) 8.1 M. 
E) 2.7 M. 
A) 0.30 M. 
B) 0.90 M. 
C) 0.0 M. 
D) 8.1 M. 
E) 2.7 M.

Question 12

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O2 from the air is 2.67 * 10-4 M at sea level and 25°C, what is the solubility of O2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O2 in air is 0.209 at both 12,000 ft and at sea level.

Accepted Answer

A) 1.75 * 10-4 M 
B) 2.67 * 10-4 M 
C) 3.66 * 10-5 M 
D) 4.06 * 10-4 M 
E) None of the above. 
A) 1.75 * 10-4 M 
B) 2.67 * 10-4 M 
C) 3.66 * 10-5 M 
D) 4.06 * 10-4 M 
E) None of the above.

Question 13

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Question 14

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 15

The concentration of nitrogen in water at 25°C was determined to be 7.2 * 10-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 * 10-4 mol/L·atm?

Accepted Answer

The answer of The concentration of nitrogen in water at...

Question 16

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 17

The vapor pressure of water at 20°C is 17.5 mmHg. What is the vapor pressure of water over a solution prepared from 2.00 * 102 g of sucrose (C12H22O11)and 3.50 * 102 g water?

Accepted Answer

A) 0.51 mmHg 
B) 16.0 mmHg 
C) 17.0 mmHg 
D) 18.0 mmHg 
E) 19.4 mmHg 
A) 0.51 mmHg 
B) 16.0 mmHg 
C) 17.0 mmHg 
D) 18.0 mmHg 
E) 19.4 mmHg

Question 18

What is the approximate Na+ ion concentration in a 0.75 M Na2CO3 solution?

Accepted Answer

A) 0.375 M 
B) 0.75 M 
C) 1.25 M 
D) 1.50 M 
E) 2.25 M 
A) 0.375 M 
B) 0.75 M 
C) 1.25 M 
D) 1.50 M 
E) 2.25 M

Question 19

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 20

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....

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.

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

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 compounds should be 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 the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality?

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.

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

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

What is the percent CdSO₄ by mass in a 1.0 molal aqueous CdSO₄solution?

Consider a 0.90 M Al(NO₃)₃ solution. This solution has a nitrate ion concentration of

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 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)

The concentration of nitrogen in water at 25°C was determined to be 7.2 * 10^-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 * 10^-4 mol/L·atm?

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

The vapor pressure of water at 20°C is 17.5 mmHg. What is the vapor pressure of water over a solution prepared from 2.00 * 10² g of sucrose (C₁₂H₂₂O₁₁)and 3.50 * 10² g water?

What is the approximate Na⁺ ion concentration in a 0.75 M Na₂CO₃ solution?

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

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 13: Physical Properties of Solutions

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.

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO4 solution.

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 compounds should be 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 the following concentration units will not change with temperature: molarity, percent mass, mole fraction, and molality?

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.

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

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

What is the percent CdSO4 by mass in a 1.0 molal aqueous CdSO4 solution?

Consider a 0.90 M Al(NO3)3 solution. This solution has a nitrate ion concentration of

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 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)

The concentration of nitrogen in water at 25°C was determined to be 7.2 * 10-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 * 10-4 mol/L·atm?

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

The vapor pressure of water at 20°C is 17.5 mmHg. What is the vapor pressure of water over a solution prepared from 2.00 * 102 g of sucrose (C12H22O11)and 3.50 * 102 g water?

What is the approximate Na+ ion concentration in a 0.75 M Na2CO3 solution?

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

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

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.

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

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 compounds should be soluble in CCl₄?

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

What is the percent CdSO₄ by mass in a 1.0 molal aqueous CdSO₄solution?

Consider a 0.90 M Al(NO₃)₃ solution. This solution has a nitrate ion concentration of

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 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)

The concentration of nitrogen in water at 25°C was determined to be 7.2 * 10^-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 * 10^-4 mol/L·atm?

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

The vapor pressure of water at 20°C is 17.5 mmHg. What is the vapor pressure of water over a solution prepared from 2.00 * 10² g of sucrose (C₁₂H₂₂O₁₁)and 3.50 * 10² g water?

What is the approximate Na⁺ ion concentration in a 0.75 M Na₂CO₃ solution?