**Problem:** What is the pH at the equivalence point when 65.0 mL of 0.30 M HCN is titrated with 0.25 M LiOH? Ka = 6.2 × 10⁻¹⁰**Explanation:** In this problem, you are asked to determine the pH at the equivalence point during a titration. Hydrocyanic acid (HCN) is being titrated with lithium hydroxide (LiOH). The given data includes the volume and molarity of HCN, the molarity of LiOH, and the acid dissociation constant (Ka) for HCN.

Answered: What is the pH at the equivalence point…

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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**Problem:**
What is the pH at the equivalence point when 65.0 mL of 0.30 M HCN is titrated with 0.25 M LiOH?
Ka = 6.2 × 10⁻¹⁰

**Explanation:**
In this problem, you are asked to determine the pH at the equivalence point during a titration. Hydrocyanic acid (HCN) is being titrated with lithium hydroxide (LiOH). The given data includes the volume and molarity of HCN, the molarity of LiOH, and the acid dissociation constant (Ka) for HCN.

Expert Solution

Step 1: Salt hydrolysis

Answer:

Conjugate base of weak acid gets hydrolysed in water producing OH^- ion that makes the solution weakly basic. HCN is the weak acid and LiOH is the strong base.

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