week 9 Acid-Base Chemistry

week 9 Acid-Base Chemistry - Acid-Base Equilibria...

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Acid-Base Equilibria Classifications of Acids and Bases I. Bronsted-Lowry Acids and Bases a. BL Acid: can donate a hydrogen ion (acetic acid) b. BL base: can accept a hydrogen ion (water) c. i.e.: CH 3 COOH (aq) + H 2 O (aq)  H 3 O + (aq) + CH 3 COO - (aq) d. conjugate acid/base i. the product that the acid turns into is the conjugate base (acetate ion) ii. the product that the base turns into is the conjugate acid (hydronium ion) e. Note: water can be both an acid or a base i. H 2 O(l) + NH 3 (aq)  NH 4 + (aq) + OH - (aq) ii. Name the acid, base, conjugate acid, and conjugate base II. Lewis Acids and Lewis Bases a. Lewis acid: any species that accepts electron pairs b. Lewis base: any species that donates electron pairs i. BF 3 + NH 3  BF 3 NH 3 ii. Draw the lewis dot structure for each of these molecules. You will notice that ammonia has a lone pair that it donates to the bond between BF3 and itself. BF3 is a lewis acid, and NH3 is a lewis base. c. Lewis definition systematizes the chemistry of many binary oxides, which can be considered as either anhydrides of acids or bases. i. Acid Anhydrides are oxides of most non metals 1. CO 2 is the acid anyhydride of H 2 CO 3 (remove one molecule of H 2 O) ii. Base Anhydrides: oxides of group I or II metals obtained by removing water from the corresponding hydroxides
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This note was uploaded on 10/26/2011 for the course CHEM 20B taught by Professor Felker during the Spring '08 term at UCLA.

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week 9 Acid-Base Chemistry - Acid-Base Equilibria...

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