If the solubility of O2 at 0.300 bar and 25°C is 12.5 g/100 g H2O, what is the solubility of O2 at a pressure of 1.64 bar and 25°C?

A) 68 g/100 g H2O B) 25.4 g/100 g H2O C) 0.4 g/100 g H2O D) 0.0 g/100 g H2O E) 2.3 g/100 g H2O A) 68 g/100 g H2O B) 25.4 g/100 g H2O C) 0.4 g/100 g H2O D) 0.0 g/100 g H2O E) 2.3 g/100 g H2O

A solution consisting of 0.278 mol of methylbenzene, C6H5CH3, in 244 g of nitrobenzene, C6H5NO2, freezes at -2.0°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?

A) 7.1°C/m B) 29°C/m C) 14.0°C/m D) 3.5°C/m E) 7.0°C/m A) 7.1°C/m B) 29°C/m C) 14.0°C/m D) 3.5°C/m E) 7.0°C/m

Exam 14: Solutions and Their Behavior

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Henry's law states that the solubility of a gas in a liquid is directly proportional to its pressure above the liquid. This law holds Right for gases such as nitrogen and oxygen. However, Henry's law does not hold Right for hydrogen chloride gas. Why?

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Question 21

The vapor pressure of pure water at 15 °C is 12.8 mm Hg. What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH₃CH₂OH, molar mass = 46.07 g/mol) and 22.0 g water?

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Question 22

What is the freezing point of an aqueous 1.38 m NaCl solution? (K_fp for water is 1.858°C/m.) Assume no ion pairing occurs.

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Question 23

What is the freezing point of a solution containing 2.80 grams benzene (molar mass = 78.11 g/mol) dissolved in 43.0 grams paradichlorobenzene (molar mass = 147.0 g/mol)? The freezing point of pure paradichlorobenzene is 53.0 °C and the freezing point depression constant, K_fp, is -7.10 °C/m.

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Question 24

Which of the following solutions has the lowest osmotic pressure?

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Question 25

The solubility of 1-pentanol in water is 2.7 g per 100 g of water at 25°C. What is the maximum amount of 1-pentanol that will dissolve in 2.1 g of water at 25°C?

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Question 26

The lattice enthalpy of LiCl is −834 kJ/mol and the enthalpy of solution of LiCl is -37 kJ/mol. Calculate the enthalpy of hydration of LiCl(s).

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Question 27

What type of colloid is formed when a liquid is dispersed in a gas?

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Question 28

A solution in which there is more dissolved solute than in a saturated solution is known as a(n) ________ solution.

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Question 29

What mass of an aqueous 18.8% glucose solution contains 85.5 g of water?

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Question 30

If an egg's shell is carefully dissolved using an acid, the egg white and yolk will remain intact inside a membrane. If the egg is then placed in distilled water, it will slowly expand until it bursts. Why?

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Question 31

If the solubility of O₂ at 0.300 bar and 25°C is 12.5 g/100 g H₂O, what is the solubility of O₂ at a pressure of 1.64 bar and 25°C?

(Multiple Choice)

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Question 32

What is the boiling-point change for a solution containing 0.251 mol of naphthalene (a nonvolatile, nonionizing compound) in 250. g of liquid benzene? (K_bp = 2.53°C/m for benzene)

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Question 33

A solution consisting of 0.278 mol of methylbenzene, C₆H₅CH₃, in 244 g of nitrobenzene, C₆H₅NO₂, freezes at -2.0°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?

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Question 34

A 15 meter by 12 meter pool of water has a depth of 2.2 meters. What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m³ = 1000 L; assume the density of the solution is 1.00 g/mL)

(Multiple Choice)

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Question 35

Because ________ particles are relatively large (say, 1000 nm in diameter) they scatter visible light, making the mixtures containing these particles appear cloudy. This scattering is known as the Tyndall effect.

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Question 36

Which of the following compounds is not miscible with water?

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Question 37

_____ are colloidal dispersions of one liquid in another.

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Question 38

A concentrated hydrochloric acid solution is 37.2% HCl by mass and has a density of 1.19 g/mL at 25°C. What is the molarity of HCl?

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Question 39

If one of the factors determining the equilibrium of a system is changed, the system adjusts to counteract that change. This is known as ________ principle.

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Question 40

Showing 21 - 40 of 80

Exam 14: Solutions and Their Behavior

Henry's law states that the solubility of a gas in a liquid is directly proportional to its pressure above the liquid. This law holds Right for gases such as nitrogen and oxygen. However, Henry's law does not hold Right for hydrogen chloride gas. Why?

The vapor pressure of pure water at 15 °C is 12.8 mm Hg. What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH3CH2OH, molar mass = 46.07 g/mol) and 22.0 g water?

What is the freezing point of an aqueous 1.38 m NaCl solution? (Kfp for water is 1.858°C/m.) Assume no ion pairing occurs.

What is the freezing point of a solution containing 2.80 grams benzene (molar mass = 78.11 g/mol) dissolved in 43.0 grams paradichlorobenzene (molar mass = 147.0 g/mol)? The freezing point of pure paradichlorobenzene is 53.0 °C and the freezing point depression constant, Kfp, is -7.10 °C/m.

Which of the following solutions has the lowest osmotic pressure?

The solubility of 1-pentanol in water is 2.7 g per 100 g of water at 25°C. What is the maximum amount of 1-pentanol that will dissolve in 2.1 g of water at 25°C?

The lattice enthalpy of LiCl is −834 kJ/mol and the enthalpy of solution of LiCl is -37 kJ/mol. Calculate the enthalpy of hydration of LiCl(s).

What type of colloid is formed when a liquid is dispersed in a gas?

A solution in which there is more dissolved solute than in a saturated solution is known as a(n) ________ solution.

What mass of an aqueous 18.8% glucose solution contains 85.5 g of water?

If an egg's shell is carefully dissolved using an acid, the egg white and yolk will remain intact inside a membrane. If the egg is then placed in distilled water, it will slowly expand until it bursts. Why?

If the solubility of O2 at 0.300 bar and 25°C is 12.5 g/100 g H2O, what is the solubility of O2 at a pressure of 1.64 bar and 25°C?

What is the boiling-point change for a solution containing 0.251 mol of naphthalene (a nonvolatile, nonionizing compound) in 250. g of liquid benzene? (Kbp = 2.53°C/m for benzene)

A solution consisting of 0.278 mol of methylbenzene, C6H5CH3, in 244 g of nitrobenzene, C6H5NO2, freezes at -2.0°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?

A 15 meter by 12 meter pool of water has a depth of 2.2 meters. What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m3 = 1000 L; assume the density of the solution is 1.00 g/mL)

Because ________ particles are relatively large (say, 1000 nm in diameter) they scatter visible light, making the mixtures containing these particles appear cloudy. This scattering is known as the Tyndall effect.

Which of the following compounds is not miscible with water?

_____ are colloidal dispersions of one liquid in another.

A concentrated hydrochloric acid solution is 37.2% HCl by mass and has a density of 1.19 g/mL at 25°C. What is the molarity of HCl?

If one of the factors determining the equilibrium of a system is changed, the system adjusts to counteract that change. This is known as ________ principle.

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

Bonding and Molecular Structure

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

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

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The vapor pressure of pure water at 15 °C is 12.8 mm Hg. What is the equilibrium vapor pressure of water above a mixture of 72.0 g ethanol (CH₃CH₂OH, molar mass = 46.07 g/mol) and 22.0 g water?

What is the freezing point of an aqueous 1.38 m NaCl solution? (K_fp for water is 1.858°C/m.) Assume no ion pairing occurs.

What is the freezing point of a solution containing 2.80 grams benzene (molar mass = 78.11 g/mol) dissolved in 43.0 grams paradichlorobenzene (molar mass = 147.0 g/mol)? The freezing point of pure paradichlorobenzene is 53.0 °C and the freezing point depression constant, K_fp, is -7.10 °C/m.

If the solubility of O₂ at 0.300 bar and 25°C is 12.5 g/100 g H₂O, what is the solubility of O₂ at a pressure of 1.64 bar and 25°C?

What is the boiling-point change for a solution containing 0.251 mol of naphthalene (a nonvolatile, nonionizing compound) in 250. g of liquid benzene? (K_bp = 2.53°C/m for benzene)

A solution consisting of 0.278 mol of methylbenzene, C₆H₅CH₃, in 244 g of nitrobenzene, C₆H₅NO₂, freezes at -2.0°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?

A 15 meter by 12 meter pool of water has a depth of 2.2 meters. What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m³ = 1000 L; assume the density of the solution is 1.00 g/mL)