25 mL of an aqueous solution of KCl was found to require 20 mL of 1 M solution when titrated using as an indicator. What is the depression in freezing point of KCl solution of the given concentratio

Question

25 mL of an aqueous solution of KCl was found to require 20 mL of 1 M  solution when titrated using  as an indicator. What is the depression in freezing point of KCl solution of the given concentration? (Nearest integer). (Given: ). Assume 100% ionization and density = 1 g mL⁻¹.

Canvas Classes · Accepted Answer

Strategy:
 Use the titration data to find the concentration of  and thus  in the original solution. Then calculate the freezing point depression using the van't Hoff factor.

Step 1: Calculate moles of } \ce{KCl} 	ext{
Formula: .
- Moles of .
- Moles of .

Step 2: Calculate Molality ()
Moles are in 25 mL of water. Mass of 25 mL  0.025 kg.

Step 3: Calculate } \Delta Tf 	ext{
For , . Given .

Nearest integer: 3.

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