Question 1

In general,which of the following type(s)of solid(s)would exhibit the greatest solubility in a polar solvent?
A)network covalent
B)ionic or polar molecular
C)ionic
D)metallic
E)polar molecular

Accepted Answer

Ionic or polar molecular solids tend to dissolve well in polar solvents due to the strong interactions between the solute and solvent molecules, such as ion-dipole or dipole-dipole interactions.

Question 2

Which of the following gases is least soluble in water? A)CO₂ B)SO₃ C)NH₃ D)N₂ E)HCl

Accepted Answer

Nitrogen (N₂) is the least soluble in water among the options given. This is because it is a nonpolar molecule and has relatively low solubility in water compared to the other gases listed, which include compounds that are either more polar or can form hydrogen bonds with water.

Question 3

Henry's Law constant is 0.034 mol/kg⋅bar and 0.0013 mol/kg⋅bar for CO₂ and O₂ respectively at 25°C.What pressure of O₂ is required to achieve the same solubility as 0.368 bar of CO₂? A)9.6 bar B)0.0 bar C) bar D) bar E)0.1 bar

Accepted Answer

A

Question 4

Which of the following favor(s)the solubility of an ionic solid in a liquid solvent?
A)a small magnitude of the lattice energy of the solute
B)a large magnitude of the solvation energy of the ions
C)a large polarity of the solvent
D)all of the above
E)none of the above

Accepted Answer

A small magnitude of the lattice energy of the solute means that it takes less energy to break apart the ionic solid, making it easier to dissolve in the liquid solvent. A large magnitude of the solvation energy of the ions means that the ions are strongly attracted to the solvent molecules, allowing them to be dispersed evenly throughout the solution. A large polarity of the solvent can help to dissolve ionic compounds through ion-dipole interactions. Therefore, all three factors favor the solubility of an ionic solid in a liquid solvent.

Question 5

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 4.1g of water at 25°C?
A)0.11 g
B)0.65 g
C)2.7 g
D)11 g
E)0.0065 g

Accepted Answer

The solubility of 1-pentanol in water is 2.7 g per 100 g of water. To find the amount that will dissolve in 4.1 g of water, use a proportion: (2.7 g / 100 g water) = (x g / 4.1 g water). Solving for x gives x = (2.7 * 4.1) / 100 = 0.1107 g, which rounds to 0.11 g.

Question 6

Which of the following is a correct statement of Henry's law?
A)The concentration of a gas in solution is directly proportional to the mole fraction of solvent.
B)The concentration of a gas in solution is inversely proportional to temperature.
C)The concentration of a gas in solution is independent of pressure.
D)The concentration of a gas in a solution is inversely proportional to pressure.
E)none of these

Accepted Answer

Henry's law states that the concentration of a gas in a solution is directly proportional to the partial pressure of that gas above the solution, which is not listed among the provided options.

Question 7

Which of the following statements best describes what happens when a small amount of solid rubidium chloride is dissolved in water?
A)The heat from the warm water melts the solid,making it a liquid.
B)Nothing happens,because rubidium chloride is insoluble in water.
C)The solid RbCl breaks apart into separate Rb and Cl atoms by interacting with the water molecules.
D)The water molecules surround each ion in the solid RbCl,separating the Rb ions from the Cl ions.
E)The solid undergoes a chemical change by reacting with the water.

Accepted Answer

When a small amount of solid rubidium chloride is dissolved in water, the water molecules surround each ion in the solid, separating the Rb ions from the Cl ions. This is because water is a polar solvent and can form hydration shells around the ions, stabilizing them in solution. Rubidium chloride is a soluble ionic compound and therefore can dissociate in water to form free ions. No chemical reaction takes place in this process.

Question 8

Which of the following compounds is least soluble in water? A)CH₃CH₂CH₂NH₂ B)CH₃CH₂CH₂F C)CH₃CH(OH)CH₃ D)CH₃CH₂COOH E)CH₃CH₂NHCH₃

Accepted Answer

The presence of fluorine atoms in molecule B makes it less soluble in water because of the high electronegativity of fluorine. The other choices contain polar functional groups that can form hydrogen bonds with water and thus have higher solubility in water.

Question 9

According to the National Institute of Standards webbook,the Henry's Law constant for N₂ gas is 0.000639 mol/kg⋅bar at 25°C What is the Henry's law constant in units of mol/kg⋅atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg) A) × 10^-4 mol/kg⋅atm B) × 10^-7 mol/kg⋅atm C) × 10^-1 mol/kg⋅atm D) × 10³ mol/kg⋅atm E) × 10⁶ mol/kg⋅atm

Accepted Answer

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

Question 10

Consider the following gas-aqueous liquid equilibrium for a closed system at a constant temperature. O₂(g) O₂(aq) What is the effect on the equilibrium composition of the liquid when the partial pressure of O₂ gas above the liquid is decreased? A)The amount of O₂ dissolved in the liquid decreases. B)The amount of O₂ dissolved in the liquid increases. C)The amount of O₂ dissolved in the liquid does not change. D)Not enough information is provided to answer the question. E)Either A or B.

Accepted Answer

According to Le Chatelier's principle, when the partial pressure of O₂ gas is decreased, the system tries to compensate by shifting the equilibrium to the side with more gas molecules. Therefore, some of the O₂ dissolved in the liquid will evaporate to restore the equilibrium. As a result, the amount of O₂ dissolved in the liquid decreases.

Question 11

Consider the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of N₂. N₂(g) N₂(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased? A)The amount of N₂ dissolved in the liquid increases. B)The amount of N₂ dissolved in the liquid decreases. C)The amount of N₂ dissolved in the liquid does not change. D)Not enough information is provided to answer the question. E)Either A or B could occur.

Accepted Answer

The answer of Consider the following gas-liquid equilibrium for an...

Question 12

Which of the following correctly states the relationship between the solubility of a substance in water and temperature?
A)The solubility of a substance in water increases as the temperature rises,especially for gases.
B)The solubility of a substance in water decreases as the temperature lowers,especially for gases.
C)The relationship between the solubility of a substance in water and temperature cannot be accurately predicted,especially for ionic solids.
D)The solubility of a substance in water decreases as the temperature rises,especially for ionic solids.
E)Two of these are correct.

Accepted Answer

The answer of Which of the following correctly states the...

Question 13

Which of the following sets of conditions favors maximum solubility of an ionic solute in water?
A)The enthalpy of hydration of the cation should be equal to the enthalpy of hydration of the anion,regardless of the magnitude of the lattice energy.
B)The magnitude of the lattice energy should be small,and the enthalpy of hydration of the ions should be large.
C)The magnitude of the lattice energy should be small,and the enthalpy of hydration of the ions should be small.
D)The magnitude of the lattice energy should be large,and the enthalpy of hydration of the ions should be small.
E)The magnitude of the lattice energy should be large,and the enthalpy of hydration of the ions should be large.

Accepted Answer

For maximum solubility of an ionic solute in water, the lattice energy (which must be overcome to dissolve the solute) should be small, and the enthalpy of hydration (energy released when ions are solvated by water) should be large. This combination favors the dissolution process energetically.

Question 14

At a particular temperature the solubility of O₂ in water is 0.590 g/L at an oxygen pressure of around 15.2 atm.What is the Henry's law constant for O₂ (in units of L · atm/mol)? A)3.88 × 10^-2 B)8.24 × 10² C)2.80× 10^-1 D)1.21× 10^-3 E)None of the above are within 5% of the correct answer.

Accepted Answer

The answer of At a particular temperature the solubility of...

Question 15

Which of the following pure liquids is the best solvent for sodium fluoride? A)CCl₄(l) B)C₂Cl₆(l) C)HCl(l) D)BCl₃(l) E)PCl₅(l)

Accepted Answer

HCl(l) is polar and can dissolve ionic compounds like sodium fluoride due to its ability to ionize and interact with the ions.

Question 16

Which of the following sets of conditions favors maximum solubility of solute in solvent?
A)The intermolecular forces between solute and solvent molecules are much weaker than the intermolecular forces between solute molecules,but much stronger than the intermolecular forces between solvent molecules.
B)The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solute molecules or the intermolecular forces between solvent molecules.
C)The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solvent molecules,but much weaker than the intermolecular forces between solute molecules.
D)The intermolecular forces between solute and solvent molecules are much stronger than the intermolecular forces between solute molecules,but much weaker than the intermolecular forces between solvent molecules.
E)The intermolecular forces between solute and solvent molecules are much weaker than the intermolecular forces between solute molecules or the intermolecular forces between solvent molecules.

Accepted Answer

The maximum solubility of a solute in a solvent is favored when the intermolecular forces between solute and solvent molecules are much stronger than those between solute molecules alone or solvent molecules alone. This ensures that the solute molecules are effectively pulled into the solvent, overcoming their own intermolecular attractions and dispersing evenly throughout the solvent.

Question 17

Which of the following pure liquids is the best solvent for carbon disulfide? A)C₆H₆(l) B)NH₃(l) C)CH₃OH(l) D)H₂O(l) E)HBr(l)

Accepted Answer

Carbon disulfide (CS2) is a nonpolar molecule. The best solvent for a nonpolar solute is a nonpolar solvent. Among the options, carbon disulfide itself (CS2) is the only nonpolar solvent, making it the best choice for dissolving carbon disulfide.

Question 18

The solubility of a gas in a liquid can always be increased by
A)decreasing the pressure of the gas above the solvent.
B)increasing the pressure of the gas above the solvent.
C)increasing the temperature of the solvent.
D)decreasing the polarity of the solvent.
E)decreasing the temperature of the gas above the solvent.

Accepted Answer

Increasing the pressure of the gas above the solvent will increase the solubility of the gas in the liquid. This is known as Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

Question 19

The dissolution of ionic compounds in water depends only on the hydration energy of the ions.
A)1 only
B)2 only
C)3 only
D)1 and 2
E)1,2,and 3

Accepted Answer

The answer of The dissolution of ionic compounds in water...

Question 20

How does the solubility of a gas in a solvent depend on pressure and temperature?
A)Increasing the partial pressure of the gas while increasing the temperature increases the solubility of the gas.
B)Decreasing the partial pressure of the gas while decreasing the temperature increases the solubility of the gas.
C)Increasing the partial pressure of the gas while decreasing the temperature increases the solubility of the gas.
D)Decreasing the partial pressure of the gas while increasing the temperature increases the solubility of the gas.
E)Gas solubility is unaffected by pressure or temperature.

Accepted Answer

According to Henry's Law, the solubility of a gas in a solvent increases with increasing pressure of the gas. At the same time, the solubility of a gas in a solvent decreases with increasing temperature. Therefore, increasing the partial pressure of the gas while decreasing the temperature would further increase the solubility of the gas in the solvent.

Quiz 12: Solutions

In general,which of the following type(s) of solid(s) would exhibit the greatest solubility in a polar solvent?

Which of the following gases is least soluble in water?

Henry's Law constant is 0.034 mol/kg⋅bar and 0.0013 mol/kg⋅bar for CO₂ and O₂ respectively at 25°C.What pressure of O₂ is required to achieve the same solubility as 0.368 bar of CO₂?

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

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 4.1g of water at 25°C?

Which of the following is a correct statement of Henry's law?

Which of the following statements best describes what happens when a small amount of solid rubidium chloride is dissolved in water?

Which of the following compounds is least soluble in water?

According to the National Institute of Standards webbook,the Henry's Law constant for N₂ gas is 0.000639 mol/kg⋅bar at 25°C What is the Henry's law constant in units of mol/kg⋅atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

Consider the following gas-aqueous liquid equilibrium for a closed system at a constant temperature. O₂(g) O₂(aq) What is the effect on the equilibrium composition of the liquid when the partial pressure of O₂ gas above the liquid is decreased?

Consider the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of N₂. N₂(g) N₂(aq) What is the effect on the equilibrium composition of the liquid when the temperature of the liquid is increased?

Which of the following correctly states the relationship between the solubility of a substance in water and temperature?

Which of the following sets of conditions favors maximum solubility of an ionic solute in water?

At a particular temperature the solubility of O₂ in water is 0.590 g/L at an oxygen pressure of around 15.2 atm.What is the Henry's law constant for O₂ (in units of L · atm/mol) ?

Which of the following pure liquids is the best solvent for sodium fluoride?

Which of the following sets of conditions favors maximum solubility of solute in solvent?

Which of the following pure liquids is the best solvent for carbon disulfide?

The solubility of a gas in a liquid can always be increased by

The dissolution of ionic compounds in water depends only on the hydration energy of the ions.

How does the solubility of a gas in a solvent depend on pressure and temperature?