**Buffer Preparation Using Ammonium Chloride and Ammonia****Question:** How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution to prepare a buffer with a pH of 9.850?**Answer:** Mass = 0.936 g---**Explanation:**To prepare a buffer solution with a desired pH, solid ammonium chloride is added to an ammonia solution. The precise amount required to reach a pH of 9.850 with the given volume and molarity of the ammonia solution is found to be 0.936 grams. Understanding buffer solutions:- Buffers are solutions that resist changes in pH when small amounts of acid or base are added.- The ammonia (NH₃) acts as a weak base, while the ammonium chloride (NH₄Cl) provides the conjugate acid (NH₄⁺).- This balance between NH₃ and NH₄⁺ maintains the pH close to the desired value, making it effective for buffering applications.

Given,Molarity of NH3 = 0.190 Mvolume of NH3 = 0.500 LpH = 9.850Kb of NH3 = 1.8 x 10-5

Answered: How many grams of solid ammonium…

How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution to prepare a buffer with a pH of 9.850? Mass = 0.936 g

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

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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