Question 1

Henry's Law constant is 0.0013 mol/kg⋅bar and 0.034 mol/kg⋅bar for O₂ and CO₂ respectively at 25°C.What pressure of CO₂ is required to achieve the same solubility as 0.711 bar of O₂?

Accepted Answer

The answer of Henry's Law constant is 0.0013 mol/kg⋅bar and...

Question 2

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?

Accepted Answer

According to Le Chatelier's principle, when a system at equilibrium is subjected to a change in temperature, the system will shift in the direction that opposes the change. In this case, increasing the temperature will favor the endothermic process of CO₂(g) dissolving into the liquid phase, causing the equilibrium to shift towards the left and decreasing the amount of CO₂ dissolved in the liquid.

Question 3

For the following gas-aqueous liquid equilibrium for a closed system at a constant temperature, N₂(g) D N₂(aq) What is the effect on the equilibrium composition of the liquid when the partial pressure of N₂ gas above the liquid is decreased?

Accepted Answer

According to Le Chatelier's principle, when a stress is applied to an equilibrium system, the system will shift in a way that partially counteracts the stress. In this case, decreasing the partial pressure of N₂ gas above the liquid is a decrease in the concentration of one of the reactants. Therefore, the system will shift to partially counteract this decrease by decreasing the amount of N₂ dissolved in the liquid, resulting in choice A.

Question 4

Which of the following statements is INCORRECT?

Accepted Answer

The statement "The solubility of a gas in water is inversely proportional to the molar mass of the gas" is incorrect. In reality, the solubility of a gas in water tends to decrease with increasing molar mass.

Question 5

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)

Accepted Answer

The answer of The Henry's law constant for O₂ in...

Question 6

The Henry's law constant for N₂ in water at 25 °C is 6.0 × 10^-4 mol/kg⋅bar.What is the equilibrium concentration of N₂ in water when the partial pressure of N₂ is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

Accepted Answer

The answer of The Henry's law constant for N₂ in...

Question 7

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

Accepted Answer

The answer of What mass of Zn(NO₃)₂ must be diluted...

Question 8

Which of the following compounds is not miscible with water?

Accepted Answer

CCl4 (carbon tetrachloride) is a nonpolar compound and is not miscible with water, as water is a polar solvent. The other compounds contain polar functional groups and are expected to be miscible with water.

Question 9

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.

Accepted Answer

The enthalpy of solution can be calculated as follows:
ΔHsolution = ΔHf(aq) - ΔHf(s)
ΔHsolution = (-583.8 kJ/mol) - (-557.7 kJ/mol)
ΔHsolution = -26.1 kJ/mol

The negative sign indicates that the process is exothermic, meaning that energy is released when RbF dissolves in water. This energy will be transferred to the solution, causing an increase in temperature, so the solution temperature will increase. Therefore, the correct answer is choice A.

Question 10

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 ____.

Accepted Answer

The tendency toward greater dispersal of energy is a thermodynamic function called entropy.

Question 11

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?

Accepted Answer

The solubility of gases in liquids increases with pressure according to Henry's Law. Since the pressure increases from 0.300 bar to 1.64 bar, the solubility of the gas in water will increase. The exact value cannot be determined without specific calculations or experimental data, but among the given options, an increase in solubility is expected, making option A the most plausible choice based on the information provided.

Question 12

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).

Accepted Answer

The enthalpy of hydration of LiCl can be calculated using the following equation:

ΔHhyd = ΔHsol - ΔHlattice

where ΔHhyd is the enthalpy of hydration, ΔHsol is the enthalpy of solution, and ΔHlattice is the lattice enthalpy.

Substituting the given values:

ΔHhyd = (-37 kJ/mol) - (-834 kJ/mol)
ΔHhyd = 797 kJ/mol

The answer is (C) -871.0 kJ/mol because the question is asking for the enthalpy of hydration of LiCl(s), so the answer must be negative (since energy is released during hydration).

Question 13

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?

Accepted Answer

The solubility of 1-pentanol in water is given as 2.7 g per 100 g of water. To find the amount that will dissolve in 2.1 g of water, use a proportion: (2.7 g / 100 g water) = (x g / 2.1 g water). Solving for x gives x = (2.7 * 2.1) / 100 = 0.0567 g, which rounds to 0.057 g.

Question 14

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.

Accepted Answer

To find the concentration in ppm, convert the molarity to grams per liter using the molar mass, then convert to mg/L (ppm). 7.1 × 10^-7 M × 169.9 g/mol = 1.20629 × 10^-4 g/L = 0.120629 mg/L ≈ 0.12 ppm.

Question 15

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)

Accepted Answer

The answer of According to the National Institute of Standards...

Question 16

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

Accepted Answer

The change in energy that accompanies the dissolution of a solid ionic compound in a solvent is called the enthalpy of solution.

Question 17

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

Accepted Answer

A) A small magnitude of the lattice energy of the solute: The lattice energy is the energy required to separate the ions in a solid, and if this value is small, it means the ions are not strongly attracted to each other, making it easier for them to dissolve in a liquid solvent.
B) A large magnitude of the solvation energy of the ions: The solvation energy is the energy released when ions are surrounded by solvent molecules, and if this value is large, it means the solvent molecules are strongly attracted to the ions, helping to break apart the solid and dissolve it.
C) A large polarity of the solvent: A polar solvent interacts well with polar solutes, allowing for strong ion-solvent interactions that can help dissolve the solid.

Question 18

Which of the following equations illustrates the formation of an aqueous solution of KF from its elements in their standard states?

Accepted Answer

The answer of Which of the following equations illustrates the...

Question 19

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)

Accepted Answer

The volume of the pool is 15 m x 12 m x 2.2 m = 396 m³. Converting to liters gives 396,000 L. At 0.14 ppm, the mass of silver ions is 0.14 mg/L x 396,000 L = 55,440 mg, which is 55.44 g.

Question 20

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.

Accepted Answer

The answer of What partial pressure of oxygen gas is...

Quiz 14: Solutions and Their Behavior

Henry's Law constant is 0.0013 mol/kg⋅bar and 0.034 mol/kg⋅bar for O₂ and CO₂ respectively at 25°C.What pressure of CO₂ is required to achieve the same solubility as 0.711 bar of O₂?

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?

For the following gas-aqueous liquid equilibrium for a closed system at a constant temperature, N₂(g) D N₂(aq) What is the effect on the equilibrium composition of the liquid when the partial pressure of N₂ gas above the liquid is decreased?

Which of the following statements is INCORRECT?

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)

The Henry's law constant for N₂ in water at 25 °C is 6.0 × 10^-4 mol/kg⋅bar.What is the equilibrium concentration of N₂ in water when the partial pressure of N₂ is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

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

Which of the following compounds is not miscible with water?

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.

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?

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) .

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?

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.

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)

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

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

Which of the following equations illustrates the formation of an aqueous solution of KF from its elements in their standard states?

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)

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.

Quiz 14: Solutions and Their Behavior

Henry's Law constant is 0.0013 mol/kg⋅bar and 0.034 mol/kg⋅bar for O2 and CO2 respectively at 25°C.What pressure of CO2 is required to achieve the same solubility as 0.711 bar of O2?

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?

For the following gas-aqueous liquid equilibrium for a closed system at a constant temperature, N2(g) D N2(aq) What is the effect on the equilibrium composition of the liquid when the partial pressure of N2 gas above the liquid is decreased?

Which of the following statements is INCORRECT?

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)

The Henry's law constant for N2 in water at 25 °C is 6.0 × 10-4 mol/kg⋅bar.What is the equilibrium concentration of N2 in water when the partial pressure of N2 is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

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

Which of the following compounds is not miscible with water?

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.

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?

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) .

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?

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.

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)

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

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

Which of the following equations illustrates the formation of an aqueous solution of KF from its elements in their standard states?

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)

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.

Henry's Law constant is 0.0013 mol/kg⋅bar and 0.034 mol/kg⋅bar for O₂ and CO₂ respectively at 25°C.What pressure of CO₂ is required to achieve the same solubility as 0.711 bar of O₂?

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?

For the following gas-aqueous liquid equilibrium for a closed system at a constant temperature, N₂(g) D N₂(aq) What is the effect on the equilibrium composition of the liquid when the partial pressure of N₂ gas above the liquid is decreased?

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)

The Henry's law constant for N₂ in water at 25 °C is 6.0 × 10^-4 mol/kg⋅bar.What is the equilibrium concentration of N₂ in water when the partial pressure of N₂ is 586 mm Hg? (760 mm Hg = 1 atm = 0.9869 bar)

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

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 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.

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)

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

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)

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.