Question

Match the following aqueous solutions with the appropriate letter from the column on the right. fill in the blank 1 1. 0.14 m Na2S A. Lowest freezing point fill in the blank 2 2. 0.20 m KI B. Second lowest freezing point fill in the blank 3 3. 0.15 m Na2CO3 C. Third lowest freezing point fill in the blank 4 4. 0.37 m Ethylene glycol(nonelectrolyte) D. Highest freezing point

Answer 1

1. 0.14 m Na2S - B. Second lowest freezing point
2. 0.20 m KI - C. Third lowest freezing point
3. 0.15 m Na2CO3 - A. Lowest freezing point
4. 0.37 m Ethylene glycol(nonelectrolyte) - D. Highest freezing point

The freezing point of a solution is lowered when a solute is added to a solvent. The extent of the lowering depends on the concentration of the solute particles in the solution. The more solute particles there are, the greater the lowering of the freezing point.

In this case, Na2S and KI are both ionic compounds that dissociate into multiple ions in solution, so they will have a greater effect on the freezing point than Na2CO3, which is also ionic but has fewer ions per formula unit. Ethylene glycol, on the other hand, is a nonelectrolyte, meaning it does not dissociate into ions in solution, so it will have the least effect on the freezing point.

Therefore, the order of the solutions from lowest to highest freezing point is:

1. 0.15 m Na2CO3 - A. Lowest freezing point
2. 0.20 m KI - C. Third lowest freezing point
3. 0.14 m Na2S - B. Second lowest freezing point
4. 0.37 m Ethylene glycol(nonelectrolyte) - D. Highest freezing point

Step-by-step explanation: