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It's the question "calculate the pH of a 0.10M hypochlorite acid,HClO solution."  Ka=2.9 x 10-8

It's the question "calculate the pH of a 0.10M hypochlorite acid,HClO solution."  Ka=2.9 x 10-8

Chemistry
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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Please explain how to exactly get pH. I have looked up practice questions and tried punching them into the calculator but doesn't match up. I got up to this point so please explain how to get the answer for pH. 

It's the question "calculate the pH of a 0.10M hypochlorite acid,HClO solution." 
Ka=2.9 x 10-8

**Acids, Bases, Salts and pH** 1. **Calculate the pH of a 0.25 M hypochlorous acid, HClO, solution** Given: \( K_a = 2.9 \times 10^{-8} \) \[ K_a = \frac{[H^+][ClO^-]}{[HClO]} \] \[ K_a = \frac{[H^+]^2}{[HClO] - [H^+]} \] \[ [H^+] = \sqrt{K_a \times [HClO]} = \sqrt{2.9 \times 10^{-8} \times 0.25} \] \[ [H^+] = 4.257 \times 10^{-5} \] \[ pH = -\log[H^+] = -\log(4.257 \times 10^{-5}) \] \[ pH \approx 4.37 \] 2. **Calculate the pH of a 0.10 M hypochlorous acid, HClO, solution** 1. Given: \( K_a = 2.9 \times 10^{-8} \) \[ K_a = \frac{[H^+][ClO^-]}{[HClO]} \] \[ 2.9 \times 10^{-8} = \frac{[x]^2}{0.10 - x} \] \[ x^2 + 2.9 \times 10^{-9} = 0 \] \[ x \approx 5.38 \times 10^{-5} \] \[ pH = -\log[H^+] = -\log(5.38 \times 10^{-5}) \] 3. **Calculate the pH of a 0.25 M perchloric, HClO₄, solution** (No calculations given; handle with similar logic to the above if needed as HClO₄ is a strong acid.) 4. **Calculate the pH of a 0.10 M perchloric, HClO₄, solution**
Transcribed Image Text:**Acids, Bases, Salts and pH** 1. **Calculate the pH of a 0.25 M hypochlorous acid, HClO, solution** Given: \( K_a = 2.9 \times 10^{-8} \) \[ K_a = \frac{[H^+][ClO^-]}{[HClO]} \] \[ K_a = \frac{[H^+]^2}{[HClO] - [H^+]} \] \[ [H^+] = \sqrt{K_a \times [HClO]} = \sqrt{2.9 \times 10^{-8} \times 0.25} \] \[ [H^+] = 4.257 \times 10^{-5} \] \[ pH = -\log[H^+] = -\log(4.257 \times 10^{-5}) \] \[ pH \approx 4.37 \] 2. **Calculate the pH of a 0.10 M hypochlorous acid, HClO, solution** 1. Given: \( K_a = 2.9 \times 10^{-8} \) \[ K_a = \frac{[H^+][ClO^-]}{[HClO]} \] \[ 2.9 \times 10^{-8} = \frac{[x]^2}{0.10 - x} \] \[ x^2 + 2.9 \times 10^{-9} = 0 \] \[ x \approx 5.38 \times 10^{-5} \] \[ pH = -\log[H^+] = -\log(5.38 \times 10^{-5}) \] 3. **Calculate the pH of a 0.25 M perchloric, HClO₄, solution** (No calculations given; handle with similar logic to the above if needed as HClO₄ is a strong acid.) 4. **Calculate the pH of a 0.10 M perchloric, HClO₄, solution**
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