**Question 13:**Calculate \( K_b \) of the solvent given the normal boiling point of the 2.7 m solution is 35.6°C. The normal boiling point of the solvent is 32.1°C. The solute is potassium iodide in a polar solvent.---In this problem, we are asked to calculate the boiling point elevation constant (\( K_b \)) for a solution. The boiling point elevation can be determined using the formula:\[\Delta T_b = K_b \cdot m\]Where:- \(\Delta T_b\) is the boiling point elevation.- \( K_b \) is the ebullioscopic constant.- \( m \) is the molality of the solution.**Given:**- Normal boiling point of the solvent = 32.1°C- Boiling point of the solution = 35.6°C- Molality (\( m \)) = 2.7 m**Steps to Solve:**1. Calculate \(\Delta T_b\) by finding the difference between the boiling point of the solution and the normal boiling point of the solvent: \[ \Delta T_b = 35.6°C - 32.1°C = 3.5°C \]2. Rearrange the formula to solve for \( K_b \): \[ K_b = \frac{\Delta T_b}{m} = \frac{3.5°C}{2.7 \, \text{m}} \]3. Calculate \( K_b \).This calculation will give you the ebullioscopic constant \( K_b \) for the solvent, which describes how much the boiling point increases per molal concentration of the solute.

Given: Molality of solution = 2.7 m. The boiling point of solution = 35.6 oC The boiling point of…

Answered: Calculate Kb of the solvent given the…

Calculate Kb of the solvent given the normal boiling point of the 2.7m solution is 35.6 C. The normal boiling point of the solvent is 32.1°C. The solute is potassium iodide in a polar sOvene

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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