The Henry's law constant for O2 in water at 25 °C is 1.3 × 10-3 mol/kg⋅bar.What partial pressure of O2 (in atm)is necessary to achieve an equilibrium concentration of 2.9 × 10-3 mol/kg O2? (1 atm = 0.9869 bar)

A) 0.44 atm B) 0.45 atm C) 2.1 atm D) 2.3 atm E) 3.8 atm A) 0.44 atm B) 0.45 atm C) 2.1 atm D) 2.3 atm E) 3.8 atm

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

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO2, CO2(g) D CO2(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

A) The amount of CO2 dissolved in the liquid increases. B) The amount of CO2 dissolved in the liquid decreases. C) The amount of CO2 dissolved in the liquid does not change. D) Not enough information is provided to answer the question. E) Either A or B could occur. A) The amount of CO2 dissolved in the liquid increases. B) The amount of CO2 dissolved in the liquid decreases. C) The amount of CO2 dissolved in the liquid does not change. D) Not enough information is provided to answer the question. E) Either A or B could occur.

What is the mole fraction of urea,CO(NH2)2,in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol,CH3OH?

A) 0.86 B) 0.14 C) 0.078 D) 0.92 E) 0.23 A) 0.86 B) 0.14 C) 0.078 D) 0.92 E) 0.23

What mass of Zn(NO3)2 must be diluted to a mass of 1.00 kg with H2O to prepare 97 ppm Zn2+(aq)?

A) 7.8 × 10-6 g B) 7.8 × 10-3 g C) 3.3 × 10-2 g D) 1.3 × 10-1 g E) 2.8 × 10-1 g A) 7.8 × 10-6 g B) 7.8 × 10-3 g C) 3.3 × 10-2 g D) 1.3 × 10-1 g E) 2.8 × 10-1 g

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

A 12.0% sucrose solution by mass has a density of 1.05 g/cm3.What mass of sucrose is present in a 53.0-mL sample of this solution?

A) 6.68 g B) 6.06 g C) 0.126 g D) 464 g E) 6.36 g A) 6.68 g B) 6.06 g C) 0.126 g D) 464 g E) 6.36 g

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

A) 0.000866 B) 0.0569 C) 0.271 D) 37.2 E) 59.2 A) 0.000866 B) 0.0569 C) 0.271 D) 37.2 E) 59.2

Exam 14: Solutions and Their Behavior

The Henry's law constant for O₂ in water at 25 °C is 1.3 × 10^-3 mol/kg⋅bar.What partial pressure of O₂ (in atm)is necessary to achieve an equilibrium concentration of 2.9 × 10^-3 mol/kg O₂? (1 atm = 0.9869 bar)

(Multiple Choice)

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Question 41

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?

(Multiple Choice)

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Question 42

What is the osmotic pressure of an aqueous solution that is 0.46% NaCl by weight at 36°C.Assume the density of the solution is 1.0 g/mL.Assume no ion pairing.(R = 0.0821 L · atm/K·mol)

(Multiple Choice)

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Question 43

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.

(Multiple Choice)

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Question 44

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 45

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.

(Short Answer)

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Question 46

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO₂, CO₂(g) D CO₂(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

(Multiple Choice)

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Question 47

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 48

What is the mole fraction of urea,CO(NH₂)₂,in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol,CH₃OH?

(Multiple Choice)

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Question 49

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 50

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

(Short Answer)

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Question 51

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?

(Multiple Choice)

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Question 52

What mass of Zn(NO₃)₂ must be diluted to a mass of 1.00 kg with H₂O to prepare 97 ppm Zn²⁺(aq)?

(Multiple Choice)

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Question 53

Two nonpolar solvents,such as hexane and carbon tetrachloride,may be miscible even though the enthalpy of mixing of these liquids might be small.A reason that mixing occurs is that mixtures have a greater dispersal of energy relative to pure solvents.The tendency toward greater dispersal of energy is a thermodynamic function called ____.

(Multiple Choice)

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Question 54

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 55

A 12.0% sucrose solution by mass has a density of 1.05 g/cm³.What mass of sucrose is present in a 53.0-mL sample of this solution?

(Multiple Choice)

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Question 56

What is the mole fraction of calcium chloride in 3.35 m CaCl₂(aq)? The molar mass of CaCl₂ is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

(Multiple Choice)

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Question 57

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

(Short Answer)

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Question 58

The following equation is known as ________ law: .

(Short Answer)

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Question 59

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

(Multiple Choice)

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Question 60

Showing 41 - 60 of 79

Exam 14: Solutions and Their Behavior

The Henry's law constant for O2 in water at 25 °C is 1.3 × 10-3 mol/kg⋅bar.What partial pressure of O2 (in atm)is necessary to achieve an equilibrium concentration of 2.9 × 10-3 mol/kg O2? (1 atm = 0.9869 bar)

What is the mass percent of an aqueous sodium hydroxide solution in which the molality of NaOH is 10.7 m?

What is the osmotic pressure of an aqueous solution that is 0.46% NaCl by weight at 36°C.Assume the density of the solution is 1.0 g/mL.Assume no ion pairing.(R = 0.0821 L · atm/K·mol)

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.

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?

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.

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO2, CO2(g) D CO2(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

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 mole fraction of urea,CO(NH2)2,in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol,CH3OH?

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)

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

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 mass of Zn(NO3)2 must be diluted to a mass of 1.00 kg with H2O to prepare 97 ppm Zn2+(aq)?

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

A 12.0% sucrose solution by mass has a density of 1.05 g/cm3.What mass of sucrose is present in a 53.0-mL sample of this solution?

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

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

The following equation is known as ________ law: .

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

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The Henry's law constant for O₂ in water at 25 °C is 1.3 × 10^-3 mol/kg⋅bar.What partial pressure of O₂ (in atm)is necessary to achieve an equilibrium concentration of 2.9 × 10^-3 mol/kg O₂? (1 atm = 0.9869 bar)

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?

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of CO₂, CO₂(g) D CO₂(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

What is the mole fraction of urea,CO(NH₂)₂,in a solution prepared by dissolving 4.8 g of urea in 30.3 g of methanol,CH₃OH?

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)

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 mass of Zn(NO₃)₂ must be diluted to a mass of 1.00 kg with H₂O to prepare 97 ppm Zn²⁺(aq)?

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

A 12.0% sucrose solution by mass has a density of 1.05 g/cm³.What mass of sucrose is present in a 53.0-mL sample of this solution?

What is the mole fraction of calcium chloride in 3.35 m CaCl₂(aq)? The molar mass of CaCl₂ is 111.0 g/mol and the molar mass of water is 18.02 g/mol.