**Buffer Solution Calculation****Problem Statement:**How many grams of solid **sodium fluoride** should be added to 2.00 L of a $9.37 \times 10^{-2}$ M **hydrofluoric acid** solution to prepare a buffer with a pH of **2.622**?**Calculation Required:**grams of **sodium fluoride** = \_\_\_\_ g**Explanation:**To find the amount of sodium fluoride needed, one would typically use the Henderson-Hasselbalch equation for buffer solutions:\[ pH = pK_a + \log \left( \frac{[A^-]}{[HA]} \right) \]Where:- $ [A^-] $ is the concentration of the conjugate base (sodium fluoride),- $ [HA] $ is the concentration of the weak acid (hydrofluoric acid),- $ pK_a $ is the negative log of the acid dissociation constant (Ka) of hydrofluoric acid.In this scenario, rearrange the equation to solve for the concentration of sodium fluoride needed, and convert that to grams using the molar mass $ (NaF) $.

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How many grams of solid sodium fluoride should be added to 2.00 L of a 9.37x10 M hydrofluoric acid solution to prepare a buffer with a pH of 2.622? grams sodium fluoride = |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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