Question 1

Colligative properties depend on

Accepted Answer

Colligative properties depend on the number of particles dissolved, not on their chemical properties or molar mass. Therefore, choice E is the best answer. The more particles dissolved, the greater the effect on colligative properties such as boiling point elevation or freezing point depression. The masses of individual ions are only relevant in solutions containing electrolytes, but their chemical properties are not important. The chemical properties of both the solvent and the solute do play a role in determining the nature of the solution, but not in affecting colligative properties like osmotic pressure or vapor pressure lowering.

Question 2

Two aqueous are prepared: 1.00 m Na₂CO₃and 1.00 m LiCl. Which of the following statements is true?

Accepted Answer

Na₂CO₃ dissociates into 3 ions (2 Na⁺ and 1 CO₃²⁻), while LiCl dissociates into 2 ions (1 Li⁺ and 1 Cl⁻). More ions result in higher osmotic pressure and boiling point elevation.

Question 3

What concentration of aqueous FeCl₃ would have the same osmotic pressure as a 0.20 M solution of CaCl₂ at the same temperature, assuming ideal behavior?

Accepted Answer

The answer of What concentration of aqueous FeCl₃ would have...

Question 4

From the following list of aqueous solutions and water, select the one with the highest boiling point.

Accepted Answer

The answer of From the following list of aqueous solutions...

Question 5

Select the strongest electrolyte from the following set.

Accepted Answer

Strong electrolytes dissociate completely in solution, producing a high concentration of ions. B, LiNO3, is a strong electrolyte because it dissociates completely into Li+ and NO3- ions in solution. A, ethanol, is a weak electrolyte because it only partially dissociates into ions. C, glucose, does not dissociate at all in solution because it is a non-electrolyte. D, CCl4, is a non-electrolyte because it does not dissociate into ions. E, HF, is a weak electrolyte because it only partially dissociates into H+ and F- ions in solution.

Question 6

Which of the following aqueous solutions will have the lowest osmotic pressure?

Accepted Answer

Osmotic pressure depends on the total concentration of solute particles in solution. KOH, RbCl, and K2SO4 dissociate into ions in solution, increasing the number of particles. CaSO4 and BaCl2 also dissociate, but the concentration of CaSO4 (0.05 m) is lower than the others, resulting in fewer particles and thus the lowest osmotic pressure.

Question 7

The concentration of iodine in sea water is 60. parts per billion by mass. If one assumes that the iodine exists in the form of iodide anions, what is the molarity of iodide in sea water? (The density of sea water is 1.025 g/mL.)

Accepted Answer

The answer of The concentration of iodine in sea water...

Question 8

Procaine hydrochloride (  = 272.77 g/mol) is used as a local anesthetic. Calculate the molarity of a 4.666 m solution which has a density of 1.1066 g/mL.

Accepted Answer

The answer of Procaine hydrochloride (  = 272.77 g/mol)...

Question 9

Raoult's Law relates the vapor pressure of the solvent above the solution to its mole fraction in the solution. Which of the following is an accurate statement?

Accepted Answer

Raoult's Law works best when applied to dilute solutions of non-reacting solutes in which the interactions between the solute and solvent molecules are negligible. It is an approximation and only applies to ideal solutions, in which there is no chemical interaction between the solute and solvent molecules.

Question 10

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li₂SO₄?

Accepted Answer

The answer of How many moles of sulfate ions are...

Question 11

Which of the following aqueous solutions should demonstrate the most non-ideal behavior?

Accepted Answer

Non-ideal behavior in aqueous solutions is often related to ion-ion interactions, and in particular, interactions between ions of similar charge. The copper ions in CuCl2 are both positively charged, leading to significant ion-ion interactions that can cause non-ideal behavior.

Question 12

How many moles of solute particles are present in 100.0 mL of 2.50 M (NH₄)₃PO₄?

Accepted Answer

The answer of How many moles of solute particles are...

Question 13

Which of the following aqueous solutions should demonstrate the most ideal behavior?

Accepted Answer

NaCl is a simple ionic compound that dissociates completely upon dissolution, yielding Na+ and Cl- ions. This makes it an ideal electrolyte and allows it to demonstrate the most ideal behavior.

Question 14

Children under the age of six with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead?

Accepted Answer

To convert parts per million (ppm) to molality (m), we need to use the following formula:

m = (mass of solute in moles) / (mass of solvent in kg)

Assuming the solvent is pure water, we can use the density of water (1 g/mL) to convert the mass of solvent (i.e., volume of solution) to kg.

The molar mass of Pb is approximately 207.2 g/mol. Therefore, to find the mass of Pb in 0.10 ppm of blood, we need to know the mass of blood. Let's assume a small child has a blood volume of about 1 L (1000 mL) and a density of 1.06 g/mL. This would give a mass of blood of 1060 g (1.06 kg).

Now, we can calculate the mass of Pb in 0.10 ppm of blood:

mass of Pb = (0.10 ppm) x (1 g / 10^6 ppm) x (1060 g) = 0.106 g

Finally, we can use the formula to calculate the molality:

m = (0.106 g / 207.2 g/mol) / 1 kg = 5.12 x 10^-8 mol/kg

This is closest to option B.

Question 15

From the following list of aqueous solutions and water, select the one with the lowest freezing point.

Accepted Answer

The answer of From the following list of aqueous solutions...

Question 16

Select the weakest electrolyte from the following set.

Accepted Answer

CH3COOH (propionic acid) is a weak electrolyte due to its partial ionization in water. The other compounds listed are all strong electrolytes, fully dissociating into ions in water.

Question 17

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of the non-volatile solute in the solution?

Accepted Answer

The mole fraction of the non-volatile solute in the solution can be calculated using Raoult's law, which states that the vapor pressure of a solvent above a solution (P_solution) is equal to the vapor pressure of the pure solvent (P_pure) multiplied by the mole fraction of the solvent (X_solvent). The decrease in vapor pressure is due to the presence of the non-volatile solute, so we can find the mole fraction of the solute by understanding the change in vapor pressure.Given:- Vapor pressure of pure acetone (P_pure) = 266 torr- Vapor pressure of acetone with non-volatile solute (P_solution) = 232 torrFirst, calculate the mole fraction of acetone (solvent) in the solution:$$X_{solvent} = \frac{P_{solution}}{P_{pure}} = \frac{232}{266} \approx 0.87$$Since the mole fraction of the solvent plus the mole fraction of the solute must equal 1 (because they make up the whole solution), we can find the mole fraction of the solute by subtracting the mole fraction of the solvent from 1:$$X_{solute} = 1 - X_{solvent} = 1 - 0.87 = 0.13$$Therefore, the mole fraction of the non-volatile solute in the solution is 0.13.

Question 18

How many moles of bromide ions are present in 750.0 mL of 1.35 M MgBr₂?

Accepted Answer

Firstly, we need to determine how many moles of MgBr₂ are present in 750.0 mL of 1.35 M solution: moles of MgBr₂ = (volume of solution in liters) x (molarity) moles of MgBr₂ = 0.750 L x 1.35 mol/L moles of MgBr₂ = 1.01 mol Next, we need to determine the number of bromide ions present for every one formula unit of MgBr₂. From the formula, we can see that there is one Mg2+ ion and two Br- ions per formula unit. Therefore: moles of Br- ions = (moles of MgBr₂) x 2 moles of Br- ions = 1.01 mol x 2 moles of Br- ions = 2.03 mol Therefore, the answer is C) 2.03 mol.

Question 19

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of acetone in the solution?

Accepted Answer

The mole fraction of acetone in the solution can be calculated using Raoult's law, which states that the vapor pressure of a solvent in a solution is equal to the vapor pressure of the pure solvent multiplied by the mole fraction of the solvent in the solution. Thus, $ \frac{232 \, \text{torr}}{266 \, \text{torr}} = 0.87 $, indicating the mole fraction of acetone is 0.87.

Question 20

Two aqueous solutions are prepared: 2.0 m Cu(NO₃)₂and 2.0 m NaBr. Which of the following statements is true?

Accepted Answer

The Cu(NO3)2 solution has a lower vapor pressure and lower freezing point than the NaBr solution because it dissociates into more ions (3 ions: Cu^2+ and 2 NO3^-) compared to NaBr (2 ions: Na^+ and Br^-), leading to a greater colligative effect.

Quiz 13: The Properties of Mixtures: Solutions and Colloids

Colligative properties depend on

Two aqueous are prepared: 1.00 m Na₂CO₃and 1.00 m LiCl. Which of the following statements is true?

What concentration of aqueous FeCl₃ would have the same osmotic pressure as a 0.20 M solution of CaCl₂ at the same temperature, assuming ideal behavior?

From the following list of aqueous solutions and water, select the one with the highest boiling point.

Select the strongest electrolyte from the following set.

Which of the following aqueous solutions will have the lowest osmotic pressure?

The concentration of iodine in sea water is 60. parts per billion by mass. If one assumes that the iodine exists in the form of iodide anions, what is the molarity of iodide in sea water? (The density of sea water is 1.025 g/mL.)

Procaine hydrochloride ( = 272.77 g/mol) is used as a local anesthetic. Calculate the molarity of a 4.666 m solution which has a density of 1.1066 g/mL.

Raoult's Law relates the vapor pressure of the solvent above the solution to its mole fraction in the solution. Which of the following is an accurate statement?

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li₂SO₄?

Which of the following aqueous solutions should demonstrate the most non-ideal behavior?

How many moles of solute particles are present in 100.0 mL of 2.50 M (NH₄) ₃PO₄?

Which of the following aqueous solutions should demonstrate the most ideal behavior?

Children under the age of six with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead?

From the following list of aqueous solutions and water, select the one with the lowest freezing point.

Select the weakest electrolyte from the following set.

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of the non-volatile solute in the solution?

How many moles of bromide ions are present in 750.0 mL of 1.35 M MgBr₂?

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of acetone in the solution?

Two aqueous solutions are prepared: 2.0 m Cu(NO₃) ₂and 2.0 m NaBr. Which of the following statements is true?

Quiz 13: The Properties of Mixtures: Solutions and Colloids

Colligative properties depend on

Two aqueous are prepared: 1.00 m Na2CO3 and 1.00 m LiCl. Which of the following statements is true?

What concentration of aqueous FeCl3 would have the same osmotic pressure as a 0.20 M solution of CaCl2 at the same temperature, assuming ideal behavior?

From the following list of aqueous solutions and water, select the one with the highest boiling point.

Select the strongest electrolyte from the following set.

Which of the following aqueous solutions will have the lowest osmotic pressure?

The concentration of iodine in sea water is 60. parts per billion by mass. If one assumes that the iodine exists in the form of iodide anions, what is the molarity of iodide in sea water? (The density of sea water is 1.025 g/mL.)

Procaine hydrochloride ( = 272.77 g/mol) is used as a local anesthetic. Calculate the molarity of a 4.666 m solution which has a density of 1.1066 g/mL.

Raoult's Law relates the vapor pressure of the solvent above the solution to its mole fraction in the solution. Which of the following is an accurate statement?

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li2SO4?

Which of the following aqueous solutions should demonstrate the most non-ideal behavior?

How many moles of solute particles are present in 100.0 mL of 2.50 M (NH4) 3PO4?

Which of the following aqueous solutions should demonstrate the most ideal behavior?

Children under the age of six with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead?

From the following list of aqueous solutions and water, select the one with the lowest freezing point.

Select the weakest electrolyte from the following set.

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of the non-volatile solute in the solution?

How many moles of bromide ions are present in 750.0 mL of 1.35 M MgBr2?

The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of acetone in the solution?

Two aqueous solutions are prepared: 2.0 m Cu(NO3) 2 and 2.0 m NaBr. Which of the following statements is true?

Two aqueous are prepared: 1.00 m Na₂CO₃and 1.00 m LiCl. Which of the following statements is true?

What concentration of aqueous FeCl₃ would have the same osmotic pressure as a 0.20 M solution of CaCl₂ at the same temperature, assuming ideal behavior?

How many moles of sulfate ions are present in 1.0 L of 0.5 M Li₂SO₄?

How many moles of solute particles are present in 100.0 mL of 2.50 M (NH₄) ₃PO₄?

How many moles of bromide ions are present in 750.0 mL of 1.35 M MgBr₂?

Two aqueous solutions are prepared: 2.0 m Cu(NO₃) ₂and 2.0 m NaBr. Which of the following statements is true?