Lec10_Acid_Base

Lec10_Acid_Base - Lecture 10: Acid-Base Reactions and the...

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Lecture 10: Acid-Base Reactions and the Carbonate System CHEM/ENVS 380 March 11, 2010 Brønsted-Lowry Acids and Bases 1. Refresh memory on acid-base equilibria. 2. Get to know the species and reactions that comprise the carbonate system. 3. What is alkalinity? Carbonate alkalinity? 4. Be able to predict how lakes with low alkalinity will respond to acid deposition compared to lakes with high alkalinity. An acid is a substance that can donate H + ( proton ). HCl, HBr, H 2 SO 4 , HNO 3 H 2 CO 3 , H 3 PO 4 , CH 3 COOH A base is a substance that can accept H + . Most famous base is OH - ( hydroxide ion ). NaOH , KOH, LiOH NH 3 , CO 3 2-
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Acid-Base Equilibrium Constants Acid-base equilibria: aA + bB cC + dD K eq is the equilibrium constant. [ i ] = concentration of “i” in M (mol L -1 ) Strong acids and bases have very large K eq . Examples: HCl H + + Cl - hydrochloric acid, K a = ~10 3 CH 3 - + H 2 O CH 4 + OH - methyl anion, K b = ~10 20 [ ] [ ] [ ] [ ] b a d c eq B A D C K =
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This note was uploaded on 09/23/2011 for the course CHEM 380 taught by Professor Staff during the Spring '11 term at S.F. State.

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Lec10_Acid_Base - Lecture 10: Acid-Base Reactions and the...

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