Question 1

If the density of a solution is less than 1.0 g/mL, its molarity will be greater than its molality.

Accepted Answer

A) True 
 B)False

Question 2

Consider the expression below, showing the terms which contribute to the heat of solution, ΔHsoln: ΔHsoln = ΔHsolute + ΔHsolvent + ΔHmix
Which of the following sets correctly shows the signs (positive or negative) of the three terms on the right hand side of the equation?

Accepted Answer

A) Δ H solute > 0; Δ H solvent > 0; Δ H mix > 0 B) Δ H solute solvent mix solute > 0; Δ H solvent > 0; Δ H mix solute solvent mix > 0 E) Δ H solute solvent > 0; Δ H mix < 0 A) Δ H solute > 0; Δ H solvent > 0; Δ H mix > 0 B) Δ H solute solvent mix solute > 0; Δ H solvent > 0; Δ H mix solute solvent mix > 0 E) Δ H solute solvent > 0; Δ H mix < 0

Question 3

Calculate the freezing point of a solution made by dissolving 3.50 g of potassium chloride (ℳ = 74.55 g/mol) in 100.0 g of water. Assume ideal behavior for the solution; Kf = 1.86°C/m.

Accepted Answer

A) −1.7°C 
B) −0.9°C 
C) 0.0°C 
D) 0.9°C 
E) 1.7°C 
A) −1.7°C 
B) −0.9°C 
C) 0.0°C 
D) 0.9°C 
E) 1.7°C

Question 4

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li2SO4?

Accepted Answer

A) 0.5 mol 
B) 1.0 mol 
C) 1.5 mol 
D) 2.0 mol 
E) 3.0 mol 
A) 0.5 mol 
B) 1.0 mol 
C) 1.5 mol 
D) 2.0 mol 
E) 3.0 mol

Question 5

For a given solution, which of the following concentration values will change as temperature changes?

Accepted Answer

A) Mass percent 
B) Molality 
C) Mole fraction 
D) Molarity 
E) None of these choices are correct. 
A) Mass percent 
B) Molality 
C) Mole fraction 
D) Molarity 
E) None of these choices are correct.

Question 6

Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C

Accepted Answer

A) 44.1 g/mol 
B) 65.8 g/mol 
C) 117 g/mol 
D) 131.6 g/mol 
E) 553 g/mol 
A) 44.1 g/mol 
B) 65.8 g/mol 
C) 117 g/mol 
D) 131.6 g/mol 
E) 553 g/mol

Question 7

Which of the following pairs of ions is arranged so that the ion with the smaller charge density is listed first?

Accepted Answer

A) K +, Rb + 
B) Cl −, K + 
C) Cl −, Br − 
D) Ca 2+, Ba 2+ 
E) None of these choices are correct. 
A) K +, Rb + 
B) Cl −, K + 
C) Cl −, Br − 
D) Ca 2+, Ba 2+ 
E) None of these choices are correct.

Question 8

What concentration of aqueous FeCl3 would have the same osmotic pressure as a 0.20 M solution of CaCl2 at the same temperature, assuming ideal behavior?

Accepted Answer

A) 0.60 M 
B) 0.40 M 
C) 0.30 M 
D) 0.15 M 
E) 0.10 M 
A) 0.60 M 
B) 0.40 M 
C) 0.30 M 
D) 0.15 M 
E) 0.10 M

Question 9

Heats of hydration may be either positive or negative.

Accepted Answer

A) True 
 B)False

Question 10

The heat of solution is the total enthalpy change when a solution is formed from the separated solute and solvent.

Accepted Answer

A) True 
 B)False

Question 11

Electrolyte solutions generally behave less ideally as the solute concentration increases.

Accepted Answer

A) True 
 B)False

Question 12

Colligative properties depend on

Accepted Answer

A) the chemical properties of the solute. 
B) the chemical properties of the solvent. 
C) the masses of the individual ions. 
D) the molar mass of the solute. 
E) the number of particles dissolved. 
A) the chemical properties of the solute. 
B) the chemical properties of the solvent. 
C) the masses of the individual ions. 
D) the molar mass of the solute. 
E) the number of particles dissolved.

Question 13

Gases with high boiling points tend to be more soluble in water than ones with low boiling points.

Accepted Answer

A) True 
 B)False

Question 14

Based only on the relative lattice energies of the compounds below, which one would be expected to have the lowest solubility in water?

Accepted Answer

A) NaBr 
B) CaS 
C) NaOH 
D) KI 
E) CsCl 
A) NaBr 
B) CaS 
C) NaOH 
D) KI 
E) CsCl

Question 15

The backbone of a protein chain consists of carbon, nitrogen, and oxygen atoms.

Accepted Answer

A) True 
 B)False

Question 16

A 2.0% (w/v) solution of sodium hydrogen citrate, Na2C6H6O7, which also contains 2.5% (w/v) of dextrose, C6H12O6, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution?

Accepted Answer

A) 0.085 M 
B) 0.19 M 
C) 0.53 M 
D) 1.2 M 
E) 1.3 M 
A) 0.085 M 
B) 0.19 M 
C) 0.53 M 
D) 1.2 M 
E) 1.3 M

Question 17

Which, if any, of the following features is common to soaps, detergents, phospholipids, and channel-forming antibiotics?

Accepted Answer

A) They all contain fatty acids. 
B) They all contain phosphate groups. 
C) They all contain polypeptide chains. 
D) Their function depends on the dual polarity of their molecules. 
E) None of these choices are correct. 
A) They all contain fatty acids. 
B) They all contain phosphate groups. 
C) They all contain polypeptide chains. 
D) Their function depends on the dual polarity of their molecules. 
E) None of these choices are correct.

Question 18

Isoamyl salicylate (ℳ = 208.25 g/mol) has a pleasant aroma and is used in perfumes and soaps. Which of the following combinations gives a 0.75 m solution of isoamyl salicylate in ethyl alcohol (d = 0.7893 g/mL)?

Accepted Answer

A) 117.2 g isoamyl salicylate in 950.0 mL of ethyl alcohol 
B) 117.2 g isoamyl salicylate in 750.0 mL of ethyl alcohol 
C) 117.2 g isoamyl salicylate in 750.0 mL of solution 
D) 117.2 g isoamyl salicylate in 592.0 g of ethyl alcohol 
E) None of these choices are correct. 
A) 117.2 g isoamyl salicylate in 950.0 mL of ethyl alcohol 
B) 117.2 g isoamyl salicylate in 750.0 mL of ethyl alcohol 
C) 117.2 g isoamyl salicylate in 750.0 mL of solution 
D) 117.2 g isoamyl salicylate in 592.0 g of ethyl alcohol 
E) None of these choices are correct.

Question 19

The larger the ion, the greater in magnitude will be its heat of hydration.

Accepted Answer

A) True 
 B)False

Question 20

Two aqueous solutions are prepared: 2.0 m Cu(NO3)2 and 2.0 m NaBr. Which of the following statements is true?

Accepted Answer

A) The Cu(NO 3)2 solution has a higher vapor pressure and lower freezing point than the NaBr solution. 
B) The Cu(NO 3)2 solution has a higher vapor pressure and higher freezing point than the NaBr solution. 
C) The Cu(NO 3)2 solution has a lower vapor pressure and lower freezing point than the NaBr solution. 
D) The Cu(NO 3)2 solution has a lower vapor pressure and higher freezing point than the NaBr solution. 
E) None of these choices are correct. 
A) The Cu(NO 3)2 solution has a higher vapor pressure and lower freezing point than the NaBr solution. 
B) The Cu(NO 3)2 solution has a higher vapor pressure and higher freezing point than the NaBr solution. 
C) The Cu(NO 3)2 solution has a lower vapor pressure and lower freezing point than the NaBr solution. 
D) The Cu(NO 3)2 solution has a lower vapor pressure and higher freezing point than the NaBr solution. 
E) None of these choices are correct.

Exam 13: The Properties of Mixtures: Solutions and Colloids

If the density of a solution is less than 1.0 g/mL, its molarity will be greater than its molality.

Consider the expression below, showing the terms which contribute to the heat of solution, ΔHsoln: ΔHsoln = ΔHsolute + ΔHsolvent + ΔHmix Which of the following sets correctly shows the signs (positive or negative) of the three terms on the right hand side of the equation?

Calculate the freezing point of a solution made by dissolving 3.50 g of potassium chloride (ℳ = 74.55 g/mol) in 100.0 g of water. Assume ideal behavior for the solution; Kf = 1.86°C/m.

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li2SO4?

For a given solution, which of the following concentration values will change as temperature changes?

Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? Kb = 1.22°C/m, boiling point of pure ethanol = 78.5°C

Which of the following pairs of ions is arranged so that the ion with the smaller charge density is listed first?

What concentration of aqueous FeCl3 would have the same osmotic pressure as a 0.20 M solution of CaCl2 at the same temperature, assuming ideal behavior?

Heats of hydration may be either positive or negative.

The heat of solution is the total enthalpy change when a solution is formed from the separated solute and solvent.

Electrolyte solutions generally behave less ideally as the solute concentration increases.

Colligative properties depend on

Gases with high boiling points tend to be more soluble in water than ones with low boiling points.

Based only on the relative lattice energies of the compounds below, which one would be expected to have the lowest solubility in water?

The backbone of a protein chain consists of carbon, nitrogen, and oxygen atoms.

A 2.0% (w/v) solution of sodium hydrogen citrate, Na2C6H6O7, which also contains 2.5% (w/v) of dextrose, C6H12O6, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution?

Which, if any, of the following features is common to soaps, detergents, phospholipids, and channel-forming antibiotics?

Isoamyl salicylate (ℳ = 208.25 g/mol) has a pleasant aroma and is used in perfumes and soaps. Which of the following combinations gives a 0.75 m solution of isoamyl salicylate in ethyl alcohol (d = 0.7893 g/mL)?

The larger the ion, the greater in magnitude will be its heat of hydration.

Two aqueous solutions are prepared: 2.0 m Cu(NO3)2 and 2.0 m NaBr. Which of the following statements is true?

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Consider the expression below, showing the terms which contribute to the heat of solution, ΔH_soln: ΔH_soln = ΔH_solute + ΔH_solvent + ΔH_mix Which of the following sets correctly shows the signs (positive or negative) of the three terms on the right hand side of the equation?

Calculate the freezing point of a solution made by dissolving 3.50 g of potassium chloride (ℳ = 74.55 g/mol) in 100.0 g of water. Assume ideal behavior for the solution; K_f = 1.86°C/m.

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li₂SO₄?

Dimethylglyoxime, DMG, is an organic compound used to test for aqueous nickel(II) ions. A solution prepared by dissolving 65.0 g of DMG in 375 g of ethanol boils at 80.3°C. What is the molar mass of DMG? K_b = 1.22°C/m, boiling point of pure ethanol = 78.5°C

What concentration of aqueous FeCl₃ would have the same osmotic pressure as a 0.20 M solution of CaCl₂ at the same temperature, assuming ideal behavior?

A 2.0% (w/v) solution of sodium hydrogen citrate, Na₂C₆H₆O₇, which also contains 2.5% (w/v) of dextrose, C₆H₁₂O₆, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution?

Two aqueous solutions are prepared: 2.0 m Cu(NO₃)₂and 2.0 m NaBr. Which of the following statements is true?