**Problem Statement: Buffer Solution Preparation**How many grams of solid potassium hypochlorite should be added to 0.500 L of a 0.189 M hypochlorous acid solution to prepare a buffer with a pH of 6.684? Given:- \( K_a (\text{HClO}) = 3.50 \times 10^{-8} \)Calculation:- Mass = \(\boxed{ \ \ } \) g(Note: Please solve the equation based on the given data and buffer theory to find the required mass.) **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 = [ ] g**Explanation:**This question involves preparing a buffer solution. To solve for the mass of ammonium chloride needed, the Henderson-Hasselbalch equation can be used to relate the pH of the buffer to the concentrations of ammonia (NH₃) and ammonium chloride (NH₄Cl). The formula is as follows:\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{base}]}{[\text{acid}]} \right) \]Where:- pKa is the negative logarithm of the acid dissociation constant (Ka) for the ammonium ion.- \([\text{base}]\) is the concentration of ammonia.- \([\text{acid}]\) is the concentration of the ammonium ion provided by ammonium chloride.This problem requires understanding of buffer calculations, concentration conversion, and possibly using the molecular weight of ammonium chloride to convert moles to grams after solving for the required moles of ammonium chloride based on the desired buffer pH.

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How many grams of solid potassium hypochlorite should be added to 0.500 L of a 0.189 M hypochlorous acid solution to pre a buffer with a pH of 6.684? (K₁ (HClO) = 3.50 × 10-8) Mass= g

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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