**Question**: What is the pH of a 0.15 M NH₄Cl (aq) solution given ammonia has a K_b of \( 1.8 \times 10^{-5} \)? **Explanation**: This problem requires the use of equilibrium calculations to find the pH of an ammonium chloride solution. Since \( \text{NH}_4^+ \) acts as a weak acid, it will donate a proton to water to form \( \text{H}^+ \) and \( \text{NH}_3 \). The given K_b value for ammonia can be used to find the K_a value for \( \text{NH}_4^+ \) by using the relationship \( K_a \times K_b = K_w \), where \( K_w \) is the ion product of water (\( 1.0 \times 10^{-14} \) at 25°C). From there, the pH can be calculated.

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What is the pH of a 0.15M NH4CI (aq) solution given ammonia has a Kp of 1.8 x 10

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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