**Designing a Buffer System****Objective:**Design a buffer that has a pH of **6.70** using one of the weak acid/conjugate base systems shown below.**Buffer Systems Table:**| Weak Acid | Conjugate Base | $ K_{\text{a}} $ | $ pK_{\text{a}} $ ||-----------|----------------|--------------------|-------------------|| $ \text{HC}_2\text{O}_4^- $ | $ \text{C}_2\text{O}_4^{2-} $ | $ 6.4 \times 10^{-5} $ | 4.19 || $ \text{H}_2\text{PO}_4^- $ | $ \text{HPO}_4^{2-} $ | $ 6.2 \times 10^{-8} $ | 7.21 || $ \text{HCO}_3^- $ | $ \text{CO}_3^{2-} $ | $ 4.8 \times 10^{-11} $ | 10.32 |**Calculation Question:**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?Variables to Solve:- Grams of potassium salt of weak acid = _____- Grams of potassium salt of conjugate base = _____

Given: Volume of buffer solution = 1.0 L concentration of weak base = 1.0 M To prepare the buffer of…

Design a buffer that has a pH of 6.70 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base K pK, HC,04 C,0,²- 6.4 x 105 4.19 H2PO4 HPO,2- 6.2 x 10-8 7.21 HCO, co,2- 4.8 × 10-1! 10.32 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? grams potassium salt of weak acid = grams potassium salt of conjugate base =

Design a buffer that has a pH of 6.70 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base K pK, HC,04 C,0,²- 6.4 x 105 4.19 H2PO4 HPO,2- 6.2 x 10-8 7.21 HCO, co,2- 4.8 × 10-1! 10.32 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? grams potassium salt of weak acid = grams potassium salt of conjugate base =

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 7CR: 7. Describe a buffered solution. Give three examples of buffered solutions. For each of your...

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Concept explainers

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.

Question

**Designing a Buffer System**

**Objective:**
Design a buffer that has a pH of **6.70** using one of the weak acid/conjugate base systems shown below.

**Buffer Systems Table:**

| Weak Acid | Conjugate Base | $ K_{\text{a}} $ | $ pK_{\text{a}} $ |
|-----------|----------------|--------------------|-------------------|
| $ \text{HC}_2\text{O}_4^- $ | $ \text{C}_2\text{O}_4^{2-} $ | $ 6.4 \times 10^{-5} $ | 4.19 |
| $ \text{H}_2\text{PO}_4^- $ | $ \text{HPO}_4^{2-} $ | $ 6.2 \times 10^{-8} $ | 7.21 |
| $ \text{HCO}_3^- $ | $ \text{CO}_3^{2-} $ | $ 4.8 \times 10^{-11} $ | 10.32 |

**Calculation Question:**
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?

Variables to Solve:
- Grams of potassium salt of weak acid = _____
- Grams of potassium salt of conjugate base = _____

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