Chapter%2013_Acids%20and%20Bases_post2

Chapter%2013_Acids%20and%20Bases_post2 - Ion-Product...

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Ion-Product Constant of Water K w = [H 3 O + ][OH ] = 1.0 x 10 −14 K eq = [H 3 O + ][OH ] 2 H 2 O ( l ) H 3 O + (aq) + OH (aq) K w K w is very small so the equilibrium lies very far to the left.
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Ion-Product Constant of Water [H 3 O + ] = [OH ] = 1.0 x 10 −7 M 2 H 2 O ( l ) H 3 O + (aq) + OH (aq) In pure water, H 3 O + and OH are produced in equal amounts since pure water is neutral. • K w is a constant when an acid or base is added to water, the concentrations of both H 3 O + and OH change – but their product is always equal to K w
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Neutral, Acidic and Basic Solutions
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Example 4 (End of Chapter 13.54) Identify each of the following conditions as acidic, basic or neutral. (a) [OH ] = 1.0 x 10 −11 M (c) [H 3 O + ] > [OH ]
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Example 5 (End of Chapter 13.58) What is the concentration of OH in each of the following solutions? (a) 0.0010 M KOH (c) 0.0010 M HCl
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Concentrations of [H 3 O + ] in solution can vary from about 1 x 10 −14 M to greater than 1 M. It’s more convenient to express this widely varying
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This note was uploaded on 02/27/2012 for the course CHEM 112 taught by Professor Harwood during the Spring '11 term at Purdue University-West Lafayette.

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Chapter%2013_Acids%20and%20Bases_post2 - Ion-Product...

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