### Designing a Buffer System with pH 3.76**Objective:**Design a buffer that has a pH of 3.76 using one of the weak acid/conjugate base systems shown below.#### Buffer Systems:The table shows three potential weak acid/conjugate base systems, their dissociation constants (Kₐ), and their pKₐ values:| Weak Acid | Conjugate Base | Kₐ | pKₐ || --------- | -------------- | --- | --- || HC₂O₄⁻ | C₂O₄²⁻ | 6.4 x 10⁻⁵ | 4.19 || H₂PO₄⁻ | HPO₄²⁻ | 6.2 x 10⁻⁸ | 7.21 || HCO₃⁻ | CO₃²⁻ | 4.8 x 10⁻¹¹ | 10.32 |**Problem:**How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?**Required Calculations:**- grams of potassium salt of the weak acid = ____- grams of potassium salt of the conjugate base = ____### Understanding the Table and ProblemThe table contains valuable information about different buffer systems that can potentially be used to create a buffer solution with the desired pH. Here's a breakdown of the columns:- **Weak Acid:** The chemical formula of the weak acid.- **Conjugate Base:** The chemical formula of the conjugate base that pairs with the weak acid.- **Kₐ (Acid Dissociation Constant):** A numeric value representing the strength of the weak acid in water.- **pKₐ:** The negative logarithm of the Kₐ value, giving a more intuitive measure of acid strength.### Choosing the Appropriate Buffer SystemTo choose the correct buffer system, compare the desired pH (3.76) with the pKₐ values of the acids. The most effective buffer will have a pKₐ close to the desired pH. In this case:- HC₂O₄⁻ has a pKₐ of 4.19, which is close

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Design a buffer that has a pH of 3.76 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pka HC₂04 C₂04²- 6.4 x 10-5 4.19 H₂PO4 HPO4²- 6.2 x 10-8 7.21 HCO3 CO3²- 4.8 x 10-11 10.32

Design a buffer that has a pH of 3.76 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pka HC₂04 C₂04²- 6.4 x 10-5 4.19 H₂PO4 HPO4²- 6.2 x 10-8 7.21 HCO3 CO3²- 4.8 x 10-11 10.32

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 108QRT

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Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8.
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Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8.
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