LEC 18 CHAP 17 - Lecture 18 Calculating the pH of a Buffer...

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TOUPADAKIS Lecture 18 Chapter 17 Lecture 18 Calculating the pH of a Buffer Solution After the Addition of a Strong Base. Buffer Capacity. Preparing a Buffer Solution. Acid-Base Indicators.
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TOUPADAKIS Lecture 18 Chapter 17 Calculating pH Changes in Buffer Solutions
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TOUPADAKIS Lecture 18 Chapter 17 Calculating the pH of a Buffer Solution After the Addition of a Strong Base Consider the buffer solution which contains 0.040 Μ CH 3 COONa and 0.080 Μ CH 3 COOH and has pH = 4.44. Calculate the pH of the solution after the addition of 0.030 mole NaOH in 500.0 ml buffer solution. What is the % pH change of the solution? Consider that Κ a = 1.8 x 10 -5 and that there is not solution volume change after the addition of the solid NaOH. If we add the same amount of 0.030 mole NaOH in the same volume of 500.0 ml HCl solution with the same pH = 4.44, what would be the new pH of the solution. What is the % pH change of the un-buffered solution this time ?
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TOUPADAKIS Lecture 18 Chapter 17 Solution for Part 1 Τ he added base of 0.030 mole OH - will react completely with the acid CH 3 COO Η of the buffer solution, decreasing its amount by 0.030 mole and increasing the amount of the its conjugate base CH 3 COO - by 0.030 mole. Calculating the new concentration of CH
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This note was uploaded on 04/18/2010 for the course CHEM 2B 993029 taught by Professor Toupadakis during the Spring '10 term at UC Davis.

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LEC 18 CHAP 17 - Lecture 18 Calculating the pH of a Buffer...

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