What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH₂Cl) in enough water to form 2.50L of solution. The K₂ of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBro, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBrO is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H₂O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.

What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH₂Cl) in enough water to form 2.50L of solution. The K₂ of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBro, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBrO is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H₂O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.78QE

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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

**Buffer Solution Problems**

1. **Ammonia Buffer Solution**
- **Problem Statement**: What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH₃) and 20.0 g of ammonium chloride (NH₄Cl) in enough water to form 2.50 L of solution? The Kb of ammonia is 1.76 × 10⁻⁵.

2. **Sodium Hypobromite Buffer Solution**
- **Problem Statement**: How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBrO is added. Ka of HBrO is 2.50 × 10⁻⁹.

3. **Sodium Lactate Buffer Solution**
- **Problem Statement**: How many grams of sodium lactate, NaC₃H₅O₃, should be added to 1.00 L of 0.150 M lactic acid, HC₃H₅O₃, to form a buffer solution with a pH of 3.90? Assume no volume change when sodium lactate is added. Ka of lactic acid is 1.40 × 10⁻⁴.

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