If 27.9 g LiCl is dissolved in 175 g H2O, what is the weight percent of LiCl in the solution?

A) 0.376% B) 6.78% C) 13.8% D) 15.9% E) 19.0% A) 0.376% B) 6.78% C) 13.8% D) 15.9% E) 19.0%

What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 49% urea by mass?

A) 0.22 B) 0.78 C) 0.49 D) 0.42 E) 0.76 A) 0.22 B) 0.78 C) 0.49 D) 0.42 E) 0.76

What is the molality of ethanol (C2H5OH) in an aqueous solution that is 39.8% ethanol by mass?

A) 1 m.. B) 0 m C) 14 m D) 1 m E) 84.0 m A) 1 m.. B) 0 m C) 14 m D) 1 m E) 84.0 m

According to the National Institute of Standards webbook, the Henry's Law constant for O2 gas is 0.0013 mol/kg?bar at 25°C What is the Henry's law constant in units of mol/kg?mmHg? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

A) \(1.7 \times 10^ {- 6}\) mol/kg?mmHg B) \(1.3 \times 10 ^ { - 3 }\) mol/kg?mmHg C) \(9.9 \times 10 ^ { - 1 }\) mol/kg?mmHg D) \(5.8 \times 10 ^ { 5 }\) mol/kg?mmHg E) \(7.6 \times 10 ^ { 2 }\) mol/kg?mmHg A) \(1.7 \times 10^ {- 6}\) mol/kg?mmHg B) \(1.3 \times 10 ^ { - 3 }\) mol/kg?mmHg C) \(9.9 \times 10 ^ { - 1 }\) mol/kg?mmHg D) \(5.8 \times 10 ^ { 5 }\) mol/kg?mmHg E) \(7.6 \times 10 ^ { 2 }\) mol/kg?mmHg

What concentration of silver nitrate (in ppm) is present in 7.1 × 10-7 M AgNO3(aq)? For very dilute aqueous solutions, you can assume the solution's density is 1.0 g/mL. The molar mass of AgNO3 is 169.9 g/mol.

A) 0.0071 ppm B) 0.12 ppm C) 0.71 ppm D) 1.7 ppm E) 8.3 ppm A) 0.0071 ppm B) 0.12 ppm C) 0.71 ppm D) 1.7 ppm E) 8.3 ppm

How many milliliters of 11.7 M H2SO4 are needed to prepare 600.0 mL of 0.10 M H2SO4?

A) 0.19 mL B) 70 mL C) 5.1 mL D) 2.6 mL E) 6.1 mL A) 0.19 mL B) 70 mL C) 5.1 mL D) 2.6 mL E) 6.1 mL

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.50 g of the nonvolatile solute urea, CO(NH2)2, to 22.7 g of methanol, CH3OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

A) 8.51 mmHg B) 64.9 mmHg C) 74.3 mmHg D) 80.5 mmHg E) 24.1 mmHg A) 8.51 mmHg B) 64.9 mmHg C) 74.3 mmHg D) 80.5 mmHg E) 24.1 mmHg

Exam 14: Solutions and Their Behavior

The standard enthalpy of formation of RbF(s) is -557.7kJ/mol and the standard enthalpy of formation of RbF(aq, 1 m) is -583.8 kJ/mol. Determine the enthalpy of solution of RbF and indicate whether the solution temperature will increase or decrease when RbF is dissolved in water.

(Multiple Choice)

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Question 61

What is the mass of H₂SO₄ in a 38.2-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H₂SO₄?

(Multiple Choice)

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Question 62

A concentrated nitric acid solution has a density of 1.41 g/mL at 25°C and is 15.8 M. What is the percent by mass of HNO_{3 in the solution?}

(Multiple Choice)

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Question 63

If 27.9 g LiCl is dissolved in 175 g H₂O, what is the weight percent of LiCl in the solution?

(Multiple Choice)

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Question 64

What is the mole fraction of urea, CH₄N₂O, in an aqueous solution that is 49% urea by mass?

(Multiple Choice)

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Question 65

What is the molality of ethanol (C₂H₅OH) in an aqueous solution that is 39.8% ethanol by mass?

(Multiple Choice)

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Question 66

Assuming ideal behavior, which of the following aqueous solutions would be expected to exhibit the smallest freezing-point lowering?

(Multiple Choice)

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Question 67

The osmotic pressure of blood is 7.65 atm at 37 °C. What mass of glucose (C₆H₁₂O₆, molar mass = 180.2 g/mol) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (R = 0.08206 L⋅atm/mol⋅K)

(Multiple Choice)

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Question 68

Which of the following favor(s) the solubility of an ionic solid in a liquid solvent?

(Multiple Choice)

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Question 69

According to the National Institute of Standards webbook, the Henry's Law constant for O₂ gas is 0.0013 mol/kg?bar at 25°C What is the Henry's law constant in units of mol/kg?mmHg? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

(Multiple Choice)

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Question 70

A surfactant used for cleaning is called a(n) ________.

(Short Answer)

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Question 71

A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at 27 °C. What is the molar mass of the solute? (R = 0.08206 L⋅atm/mol⋅K)

(Multiple Choice)

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Question 72

What concentration of silver nitrate (in ppm) is present in 7.1 × 10^-7 M AgNO₃(aq)? For very dilute aqueous solutions, you can assume the solution's density is 1.0 g/mL. The molar mass of AgNO₃ is 169.9 g/mol.

(Multiple Choice)

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Question 73

The vapor pressure of water at 90°C is 0.692 atm. What is the vapor pressure (in atm) of a solution made by dissolving 2.91 mole(s) of CsF(s) in 1.00 kg of water? Assume that Raoult's law applies.

(Multiple Choice)

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Question 74

A 3.0 g sample of a small protein having a molecular weight of 42,000 g/mol is dissolved in 52.8 mL of water at 21°C. What is the osmotic pressure of the solution? (R = 0.0821 L · atm/K·mol, 1 atm = 760 mmHg)

(Multiple Choice)

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Question 75

What partial pressure of oxygen gas is required in order for 0.00284 g of the gas to dissolve in 15.9 mL of pure water? The Henry's law constant for oxygen gas is 1.3 × 10^-3 M atm^-1.

(Multiple Choice)

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Question 76

How many milliliters of 11.7 M H₂SO₄ are needed to prepare 600.0 mL of 0.10 M H₂SO₄?

(Multiple Choice)

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Question 77

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.50 g of the nonvolatile solute urea, CO(NH₂)₂, to 22.7 g of methanol, CH₃OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

(Multiple Choice)

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Question 78

The change in energy accompanying the equation below is the _____ of MX. MX(s) → M⁺(aq) + X−(aq)

(Multiple Choice)

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Question 79

Which of the following is a colligative property?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 80

Exam 14: Solutions and Their Behavior

The standard enthalpy of formation of RbF(s) is -557.7kJ/mol and the standard enthalpy of formation of RbF(aq, 1 m) is -583.8 kJ/mol. Determine the enthalpy of solution of RbF and indicate whether the solution temperature will increase or decrease when RbF is dissolved in water.

What is the mass of H2SO4 in a 38.2-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H2SO4?

A concentrated nitric acid solution has a density of 1.41 g/mL at 25°C and is 15.8 M. What is the percent by mass of HNO3 in the solution?

If 27.9 g LiCl is dissolved in 175 g H2O, what is the weight percent of LiCl in the solution?

What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 49% urea by mass?

What is the molality of ethanol (C2H5OH) in an aqueous solution that is 39.8% ethanol by mass?

Assuming ideal behavior, which of the following aqueous solutions would be expected to exhibit the smallest freezing-point lowering?

The osmotic pressure of blood is 7.65 atm at 37 °C. What mass of glucose (C6H12O6, molar mass = 180.2 g/mol) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (R = 0.08206 L⋅atm/mol⋅K)

Which of the following favor(s) the solubility of an ionic solid in a liquid solvent?

According to the National Institute of Standards webbook, the Henry's Law constant for O2 gas is 0.0013 mol/kg?bar at 25°C What is the Henry's law constant in units of mol/kg?mmHg? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

A surfactant used for cleaning is called a(n) ________.

A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at 27 °C. What is the molar mass of the solute? (R = 0.08206 L⋅atm/mol⋅K)

What concentration of silver nitrate (in ppm) is present in 7.1 × 10-7 M AgNO3(aq)? For very dilute aqueous solutions, you can assume the solution's density is 1.0 g/mL. The molar mass of AgNO3 is 169.9 g/mol.

The vapor pressure of water at 90°C is 0.692 atm. What is the vapor pressure (in atm) of a solution made by dissolving 2.91 mole(s) of CsF(s) in 1.00 kg of water? Assume that Raoult's law applies.

A 3.0 g sample of a small protein having a molecular weight of 42,000 g/mol is dissolved in 52.8 mL of water at 21°C. What is the osmotic pressure of the solution? (R = 0.0821 L · atm/K·mol, 1 atm = 760 mmHg)

What partial pressure of oxygen gas is required in order for 0.00284 g of the gas to dissolve in 15.9 mL of pure water? The Henry's law constant for oxygen gas is 1.3 × 10-3 M atm-1.

How many milliliters of 11.7 M H2SO4 are needed to prepare 600.0 mL of 0.10 M H2SO4?

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.50 g of the nonvolatile solute urea, CO(NH2)2, to 22.7 g of methanol, CH3OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

The change in energy accompanying the equation below is the _____ of MX. MX(s) → M+(aq) + X−(aq)

Which of the following is a colligative property?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

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Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

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Carbon: Not Just Another Element

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What is the mass of H₂SO₄ in a 38.2-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H₂SO₄?

A concentrated nitric acid solution has a density of 1.41 g/mL at 25°C and is 15.8 M. What is the percent by mass of HNO_{3 in the solution?}

If 27.9 g LiCl is dissolved in 175 g H₂O, what is the weight percent of LiCl in the solution?

What is the mole fraction of urea, CH₄N₂O, in an aqueous solution that is 49% urea by mass?

What is the molality of ethanol (C₂H₅OH) in an aqueous solution that is 39.8% ethanol by mass?

According to the National Institute of Standards webbook, the Henry's Law constant for O₂ gas is 0.0013 mol/kg?bar at 25°C What is the Henry's law constant in units of mol/kg?mmHg? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

What concentration of silver nitrate (in ppm) is present in 7.1 × 10^-7 M AgNO₃(aq)? For very dilute aqueous solutions, you can assume the solution's density is 1.0 g/mL. The molar mass of AgNO₃ is 169.9 g/mol.

What partial pressure of oxygen gas is required in order for 0.00284 g of the gas to dissolve in 15.9 mL of pure water? The Henry's law constant for oxygen gas is 1.3 × 10^-3 M atm^-1.

How many milliliters of 11.7 M H₂SO₄ are needed to prepare 600.0 mL of 0.10 M H₂SO₄?

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.50 g of the nonvolatile solute urea, CO(NH₂)₂, to 22.7 g of methanol, CH₃OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

The change in energy accompanying the equation below is the _____ of MX. MX(s) → M⁺(aq) + X−(aq)