Chapter 8 Study Guide

Chapter 8 Study Guide - Chapter 8 Study Guide Common ion...

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Chapter 8 Study Guide Common ion effect: Buffered solution: a solution that resists a change in its pH when either hydroxide ions or protons are added The most important buffering system in the blood involves HCO 3 - and H 2 CO 3 In a buffered solution the pH is governed by the ratio [HA]/[A - ] [H + ] = K a [HA] [A - ] Henderson-Hasselbalch Equation: an equation giving the relationship between the pH of an acid-base system and the concentrations of base and acid pH = p K a + log ( [base] / [acid] ) For a particular buffering system (acid-conjugate base pair), all solutions that have the same ratio of [A - ]/[HA] have the same pH Characteristics of Buffered Solutions 1) Buffered solutions contain relatively large concentrations of a weak acid and its corresponding weak base. They can involve a weak acid HA and the conjugate base A - or a weak base B and the conjugate acid BH + 2) When H + is added to a buffered solution, it reacts essentially to completion with the weak acid present: H + + A
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This note was uploaded on 09/19/2011 for the course CHEM 43L taught by Professor Therien during the Fall '09 term at Duke.

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Chapter 8 Study Guide - Chapter 8 Study Guide Common ion...

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