**Problem 1: Percent Ionization of Chloroacetic Acid**Calculate the percent ionization of 0.0065 M chloroacetic acid. Given: \( K_a = 1.36 \times 10^{-3} \).**Problem 2: pH Calculation at Physiological Temperature**The value of \( K_w \) at the physiological temperature of 37°C is \( 2.4 \times 10^{-14} \). Determine the pH at the neutral point of water at this temperature, where there are equal numbers of \( \text{H}^+ \) and \( \text{OH}^- \).

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What is percent ionization of 0.0065 M chloroacetic acid? K₁ = 1.36 × 10-3 The value of Kw at the physiological temperature 37°C is 2.4 x 10-14. What is the pH at the neutral point of water at this temperature, where there are equal number of H+ and OH-?

What is percent ionization of 0.0065 M chloroacetic acid? K₁ = 1.36 × 10-3 The value of Kw at the physiological temperature 37°C is 2.4 x 10-14. What is the pH at the neutral point of water at this temperature, where there are equal number of H+ and OH-?

Chemistry

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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

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Question

**Problem 1: Percent Ionization of Chloroacetic Acid**

Calculate the percent ionization of 0.0065 M chloroacetic acid. Given: \( K_a = 1.36 \times 10^{-3} \).

**Problem 2: pH Calculation at Physiological Temperature**

The value of \( K_w \) at the physiological temperature of 37°C is \( 2.4 \times 10^{-14} \). Determine the pH at the neutral point of water at this temperature, where there are equal numbers of \( \text{H}^+ \) and \( \text{OH}^- \).

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