Question 1

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...

Question 2

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 3

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

To convert the Henry's Law constant from mol/kg?bar to mol/kg?mmHg, multiply by the conversion factor from bar to mmHg: 0.0013 mol/kg?bar * (1 bar / 0.9869 atm) * (1 atm / 760 mmHg) = 1.7 x 10^-6 mol/kg?mmHg.

Question 4

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 5

Which of the following liquids are miscible with water in any proportion?

Accepted Answer

Ethanol and formic acid are both polar and can form hydrogen bonds with water, making them miscible with water in any proportion.

Question 6

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

Accepted Answer

The formation of an aqueous solution of KF from its elements in their standard states involves potassium (K) in its solid state and fluorine (F2) in its gaseous state reacting to form KF in an aqueous solution.

Question 7

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 8

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 change of solution is the sum of the lattice enthalpy and the enthalpy change of hydration. Therefore,
ΔHsoln = ΔHlattice + ΔHhydration
-37 kJ/mol = -834 kJ/mol + ΔHhydration
ΔHhydration = -37 kJ/mol - (-834 kJ/mol)
ΔHhydration = -37 + 834 kJ/mol
ΔHhydration = 797 kJ/mol
Therefore, the enthalpy of hydration of LiCl(s) is -797 kJ/mol, which is choice C.

Question 9

What is the Henry's law constant for O2 if the solubility of O2 in water is 0.590 g/L at a pressure of 15.5 atm?

Accepted Answer

The answer of What is the Henry's law constant for...

Question 10

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 11

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

Using the solubility value given, we can calculate the maximum amount of 1-pentanol that will dissolve in 100 g of water:

2.7 g/100 g water

We can use this value to convert the amount of water given (2.1 g) into the maximum amount of 1-pentanol that will dissolve:

(2.7 g/100 g water) x (2.1 g water) = 0.057 g 1-pentanol

Therefore, the answer is A, with a maximum of 0.057 g of 1-pentanol dissolving in 2.1 g of water at 25°C.

Question 12

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 13

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 14

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. The solubility of a gas in water is actually directly proportional to the molar mass of the gas.

Question 15

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 calculate the concentration of silver nitrate in ppm, we need to convert the molarity of AgNO3 to moles per liter first.

7.1 × 10^-7 M AgNO3 = 7.1 × 10^-7 moles of AgNO3 per liter of solution

Since the solution density is 1.0 g/mL, 1 liter of the solution equals 1000 grams of solution. We can use this information to convert the moles of AgNO3 to grams of AgNO3:

7.1 × 10^-7 moles/L × 169.9 g/mol × 1000 g/L = 0.0121 g/L

Finally, we convert grams of AgNO3 per liter to ppm:

0.0121 g/L = 12.1 ppm

Therefore, the concentration of silver nitrate in the solution is 0.12 ppm. Answer: B.

Question 16

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 17

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

Accepted Answer

A small magnitude of the lattice energy of the solute means that the ionic solid can easily break apart into individual ions in the liquid solvent. A large magnitude of the solvation energy of the ions means that the solvent can effectively surround and separate the individual ions, preventing them from re-forming the ionic solid. A large polarity of the solvent means that the solvent molecules can interact favorably with the ions, thus stabilizing them in solution. All three of these factors favor the solubility of an ionic solid in a liquid solvent.

Question 18

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 answer of A 15 meter by 12 meter pool...

Question 19

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 using the equation:
ΔH(solution) = ΔH(aq) - ΔH(s)
where ΔH(aq) is the enthalpy of formation of RbF(aq,1m) and ΔH(s) is the enthalpy of formation of RbF(s).

ΔH(solution) = -583.8 kJ/mol - (-557.7 kJ/mol) 
ΔH(solution) = -26.1 kJ/mol

Since the enthalpy of solution is negative, it means that the solution is exothermic and releases heat when RbF is dissolved in water. Thus, the solution temperature will increase.

Question 20

Which of the following compounds is not miscible with water?

Accepted Answer

CCl4 is a nonpolar compound and does not exhibit any electrostatic interactions with water molecules. Therefore, it is not miscible with water. The other compounds are polar or have functional groups that interact with water, making them miscible.

Quiz 14: Solutions and Their Behavior

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?

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 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)

Which of the following liquids are miscible with water in any proportion?

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

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

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 is the Henry's law constant for O2 if the solubility of O2 in water is 0.590 g/L at a pressure of 15.5 atm?

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 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?

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 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 statements is INCORRECT?

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.

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

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 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.

Which of the following compounds is not miscible with water?

Quiz 14: Solutions and Their Behavior

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?

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 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)

Which of the following liquids are miscible with water in any proportion?

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

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

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 is the Henry's law constant for O2 if the solubility of O2 in water is 0.590 g/L at a pressure of 15.5 atm?

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 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?

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 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 statements is INCORRECT?

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.

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

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 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.

Which of the following compounds is not miscible with water?

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?

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 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)

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

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)

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

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 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)