Question 1

Which of the following combinations of solid and liquid would not be likely to form a solution?

Accepted Answer

Ionic solids typically dissolve in polar liquids due to the interaction between the ionic charges and the polar molecules. Non-polar liquids lack the necessary polarity to effectively solvate ionic compounds, making them unlikely to form a solution.

Question 2

Which of the substances listed below is more soluble in hexane (C₆H₁₄) than in water?

Accepted Answer

CS2H5Cl (choice C) is more soluble in hexane than in water because it is a nonpolar compound, and hexane is a nonpolar solvent. Nonpolar solutes tend to dissolve better in nonpolar solvents due to similar intermolecular forces.

Question 3

Propylene glycol, C₃H₆(OH)₂, is sometimes used in automobile antifreeze solutions. If an aqueous solution has a mole fraction of c _C3H6(OH)2= 0.100, what is the molality of the propylene glycol in this solution?

Accepted Answer

To find the molality of the solution, we need to first determine the moles of propylene glycol in the solution. We can use the mole fraction of propylene glycol to do this:

moles of propylene glycol = mole fraction of propylene glycol x total moles of solution

The total moles of solution can be calculated as:

total moles of solution = moles of water + moles of propylene glycol

Since water is the solvent, we can assume that its moles are equal to its mass in grams divided by its molar mass:

moles of water = mass of water / molar mass of water

Assuming 1 L of solution, with a density of 1 g/mL, and a mole fraction of propylene glycol of 0.100, we can calculate:

mass of propylene glycol = 0.100 x 1 L x 1.04 g/mL x 76.10 g/mol = 7.82 g
mass of water = (1 – 0.100) x 1 L x 1000 g/L = 900 g

moles of propylene glycol = 7.82 g / 76.10 g/mol = 0.103 mol
moles of water = 900 g / 18.015 g/mol = 49.97 mol
total moles of solution = 0.103 mol + 49.97 mol = 50.07 mol

Now we can calculate the molality of the solution:

molality = moles of propylene glycol / mass of water in kg

mass of water in kg = 900 g / 1000 g/kg = 0.900 kg

molality = 0.103 mol / 0.900 kg = 0.1144 mol/kg ≈ 6.17 m

Therefore, the answer is choice D, 6.17 m.

Question 4

The solubility limit for Sodium Chloride at 50 ° C is 37.0 grams of NaCl per 100 grams of water. What type of solution exists if 9.25 grams of NaCl is dissolved in 25 grams of water at 50 ° C?

Accepted Answer

The answer of The solubility limit for Sodium Chloride at...

Question 5

Consider the three statements and pick the best answer.
I. An increase in disorder favors dissolution.
II. A negative enthalpy of solution favors dissolution.
III. The solubility of substances can be accurately predicted from mathematical models.

Accepted Answer

I and II are true because an increase in disorder (entropy) generally favors dissolution, and a negative enthalpy of solution (indicating an exothermic process) also favors dissolution. However, III is false because while mathematical models can provide estimates, they cannot always accurately predict the solubility of substances due to the complex nature of interactions in solution.

Question 6

What is the strongest type of intermolecular force between solute and solvent in a solution of hexane dissolved in benzene?

Accepted Answer

Hexane and benzene are both nonpolar molecules and the strongest type of intermolecular force between nonpolar molecules is dispersion forces. While dipole-dipole forces and hydrogen bonding can occur between polar molecules, they are not relevant in this case because hexane and benzene are nonpolar. Similarly, ion-dipole forces require the presence of an ion and are not applicable here. Dipole-induced dipole forces can occur between a polar molecule and a nonpolar molecule, but the strength of these forces is generally weaker than dispersion forces, so C is still the best answer.

Question 7

Which substance listed below would be most likely to dissolve in H₂O?

Accepted Answer

BaCl₂ is an ionic compound, and ionic compounds generally dissolve well in water due to the polar nature of water molecules.

Question 8

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO₃)₂ exists in an aqueous solution?

Accepted Answer

The answer of After carefully noting the orientation in which...

Question 9

Which set(s) of materials listed below will all readily dissolve in water? I. KCl, NH₃, CH₃OH II. CaBr₂, CH₂Br₂, NH₃ III. CH₃Cl, MgCl₂,CH₃OH

Accepted Answer

The materials in set I (KCl, NH3, CH3OH) will all readily dissolve in water because they are either ionic compounds or polar molecules, which are known to be soluble in water. Sets II and III contain compounds that are not all readily soluble in water.

Question 10

What type of solute-solvent interaction is most important in a solution that contains Na₂SO₄ dissolved in water?

Accepted Answer

Na₂SO₄ contains ions, specifically Na+ and SO42-. Water molecules contain partial positive and negative charges due to their polar covalent bonds. Ion-dipole interactions occur between the charged ions in the solute and the partially charged ends of the water molecules, making them the most important solute-solvent interaction in this solution.

Question 11

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl₂ exists in aqueous solution?

Accepted Answer

The answer of After carefully noting the orientation in which...

Question 12

Which of the following would be least soluble in water?

Accepted Answer

The answer of Which of the following would be least...

Question 13

Which of the following is soluble in H₂O?

Accepted Answer

H₂O is likely a chemical formula or abbreviation for a solvent or solution, but it is not recognizable. Therefore, we cannot predict whether a compound will be soluble or insoluble in it. However, we can use our knowledge of solubility rules to determine that NaCl is soluble in water, which is a common solvent, and therefore likely to be soluble in the unknown solvent as well. The other compounds, Fe(OH)₃, AgI, and PbSO₄, are insoluble in water, which is a common solvent, and therefore likely to be insoluble in the unknown solvent as well. Therefore, the best choice is D, NaCl.

Question 14

Generally a process is considered favorably spontaneous if the process releases heat to the surroundings. The following three processes are necessary to dissolve a solute such as NaCl in a solvent such as water. Which of these is considered an exothermic process?
I. Solute-Solute interactions must be broken.
II. Solvent-Solvent interactions must be broken.
III. Solute-Solvent interactions are formed.

Accepted Answer

III. Solute-Solvent interactions are formed is considered an exothermic process because energy is released when new attractions between the solute and solvent molecules are formed, leading to a release of heat to the surroundings.

Question 15

Which of the following would be expected to be more soluble in water than in hexane (C₆H₁₄)?

Accepted Answer

Ethylene glycol contains a hydroxyl (-OH) group, which allows for hydrogen bonding with water molecules, increasing its solubility in water. Napthalene and benzene are nonpolar and therefore more soluble in hexane. Chlorobenzene is polar but also contains a bulky chloro group that reduces its solubility in water. Insufficient information is given for any other substance.

Question 16

An aqueous solution of Ag₂SO₄ contains 0.28 g of Ag₂SO₄ dissolved in 25.0 grams of water at 50 ° C. How would this solution be described qualitatively if the solubility limit for this compound at 50 ° C is 1.08 g Ag₂SO₄/100 g of water?

Accepted Answer

The answer of An aqueous solution of Ag₂SO₄ contains 0.28...

Question 17

In general, a process that is exothermic is favorably spontaneous. When ammonium nitrate, NH₄NO₃, is dissolved in water, the process is endothermic yet still spontaneous. Why is this process spontaneous? Recall that there are three steps in the dissolution process. Step 1: Solute-Solute interactions must be broken. Step 2: Solvent-Solvent interactions must be broken. Step 3: Solute-Solvent interactions are formed.

Accepted Answer

The process of dissolving ammonium nitrate in water is endothermic but still spontaneous because the overall solution upon mixing is more disordered than the pure substances (NH₄NO₃ and water) due to the increase in entropy factor. In other words, the increase in disorder (entropy) of the system is favored even though it requires the input of energy to break solute-solvent and solvent-solvent interactions.

Question 18

Which of the following molecular compounds would be highly soluble in hexane, C₆H₁₄? I. CH₃OH II. C₆H₆ III. H₂O

Accepted Answer

Hexane is a nonpolar solvent, so it will dissolve nonpolar compounds better than polar compounds. Compound II is a nonpolar compound because it consists of only carbon and hydrogen atoms. Compounds I and III are polar compounds because they contain oxygen atoms, which are more electronegative than carbon and hydrogen atoms. Therefore, only compound II (C₆H₆) would be highly soluble in hexane.

Question 19

In which solvent would the solubility of potassium chloride be greatest?

Accepted Answer

Potassium chloride is an ionic compound and will dissolve in polar solvents due to its ability to dissociate into its constituent ions. Water is a highly polar solvent and thus will have the highest solubility for potassium chloride among the choices given.

Question 20

After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na₂SO₄ exists in an aqueous solution?

Accepted Answer

The answer of After carefully noting the orientation in which...

Quiz 12: Solutions

Which of the following combinations of solid and liquid would not be likely to form a solution?

Which of the substances listed below is more soluble in hexane (C₆H₁₄) than in water?

Propylene glycol, C₃H₆(OH) ₂, is sometimes used in automobile antifreeze solutions. If an aqueous solution has a mole fraction of c _{C3H6(OH) 2}= 0.100, what is the molality of the propylene glycol in this solution?

The solubility limit for Sodium Chloride at 50 ° C is 37.0 grams of NaCl per 100 grams of water. What type of solution exists if 9.25 grams of NaCl is dissolved in 25 grams of water at 50 ° C?

Consider the three statements and pick the best answer. I. An increase in disorder favors dissolution. II. A negative enthalpy of solution favors dissolution. III. The solubility of substances can be accurately predicted from mathematical models.

What is the strongest type of intermolecular force between solute and solvent in a solution of hexane dissolved in benzene?

Which substance listed below would be most likely to dissolve in H₂O?

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO₃) ₂ exists in an aqueous solution?

Which set(s) of materials listed below will all readily dissolve in water? I. KCl, NH₃, CH₃OH II. CaBr₂, CH₂Br₂, NH₃ III. CH₃Cl, MgCl₂,CH₃OH

What type of solute-solvent interaction is most important in a solution that contains Na₂SO₄ dissolved in water?

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl₂ exists in aqueous solution?

Which of the following would be least soluble in water?

Which of the following is soluble in H₂O?

Which of the following would be expected to be more soluble in water than in hexane (C₆H₁₄) ?

An aqueous solution of Ag₂SO₄ contains 0.28 g of Ag₂SO₄ dissolved in 25.0 grams of water at 50 ° C. How would this solution be described qualitatively if the solubility limit for this compound at 50 ° C is 1.08 g Ag₂SO₄/100 g of water?

Which of the following molecular compounds would be highly soluble in hexane, C₆H₁₄? I. CH₃OH II. C₆H₆ III. H₂O

In which solvent would the solubility of potassium chloride be greatest?

After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na₂SO₄ exists in an aqueous solution?

Quiz 12: Solutions

Which of the following combinations of solid and liquid would not be likely to form a solution?

Which of the substances listed below is more soluble in hexane (C6H14) than in water?

Propylene glycol, C3H6(OH) 2, is sometimes used in automobile antifreeze solutions. If an aqueous solution has a mole fraction of c C3H6(OH) 2 = 0.100, what is the molality of the propylene glycol in this solution?

The solubility limit for Sodium Chloride at 50 ° C is 37.0 grams of NaCl per 100 grams of water. What type of solution exists if 9.25 grams of NaCl is dissolved in 25 grams of water at 50 ° C?

Consider the three statements and pick the best answer. I. An increase in disorder favors dissolution. II. A negative enthalpy of solution favors dissolution. III. The solubility of substances can be accurately predicted from mathematical models.

What is the strongest type of intermolecular force between solute and solvent in a solution of hexane dissolved in benzene?

Which substance listed below would be most likely to dissolve in H2O?

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO3) 2 exists in an aqueous solution?

Which set(s) of materials listed below will all readily dissolve in water? I. KCl, NH3, CH3OH II. CaBr2, CH2Br2, NH3 III. CH3Cl, MgCl2,CH3OH

What type of solute-solvent interaction is most important in a solution that contains Na2SO4 dissolved in water?

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl2 exists in aqueous solution?

Which of the following would be least soluble in water?

Which of the following is soluble in H2O?

Which of the following would be expected to be more soluble in water than in hexane (C6H14) ?

An aqueous solution of Ag2SO4 contains 0.28 g of Ag2SO4 dissolved in 25.0 grams of water at 50 ° C. How would this solution be described qualitatively if the solubility limit for this compound at 50 ° C is 1.08 g Ag2SO4/100 g of water?

Which of the following molecular compounds would be highly soluble in hexane, C6H14? I. CH3OH II. C6H6 III. H2O

In which solvent would the solubility of potassium chloride be greatest?

After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na2SO4 exists in an aqueous solution?

Which of the substances listed below is more soluble in hexane (C₆H₁₄) than in water?

Propylene glycol, C₃H₆(OH) ₂, is sometimes used in automobile antifreeze solutions. If an aqueous solution has a mole fraction of c _{C3H6(OH) 2}= 0.100, what is the molality of the propylene glycol in this solution?

Which substance listed below would be most likely to dissolve in H₂O?

After carefully noting the orientation in which the dipoles of water molecules surround the solute particles, which choice below best represents the true nature of how Mg(NO₃) ₂ exists in an aqueous solution?

Which set(s) of materials listed below will all readily dissolve in water? I. KCl, NH₃, CH₃OH II. CaBr₂, CH₂Br₂, NH₃ III. CH₃Cl, MgCl₂,CH₃OH

What type of solute-solvent interaction is most important in a solution that contains Na₂SO₄ dissolved in water?

After carefully noting the orientation in which water surrounds each solute particle, which choice below best represents the true nature of how CaCl₂ exists in aqueous solution?

Which of the following is soluble in H₂O?

Which of the following would be expected to be more soluble in water than in hexane (C₆H₁₄) ?

An aqueous solution of Ag₂SO₄ contains 0.28 g of Ag₂SO₄ dissolved in 25.0 grams of water at 50 ° C. How would this solution be described qualitatively if the solubility limit for this compound at 50 ° C is 1.08 g Ag₂SO₄/100 g of water?

Which of the following molecular compounds would be highly soluble in hexane, C₆H₁₄? I. CH₃OH II. C₆H₆ III. H₂O

After carefully noting the orientation in which water molecules surround each solute particle, which choice below best represents the true nature of how Na₂SO₄ exists in an aqueous solution?