CHEM 112 Lecture 23: CHEM112 Lecture 23
26 Mar 2016
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Chem112 lecture 24 introduction to buffers. Question: for the reaction below the k>1. Which of the components is the stronger acid: hf, because the equilibrium favors the weaker acid, and since k>1, you must realize that the equilibrium shifts, thus making for a stronger acid reactant of hf. How do buffers work: an acetic acid and acetate ion buffer solution, the buffer solution, ch3cooh + ch3coo- + h2o. If we add a strong base it reacts only with: oh- + ch3cooh ch3coo- + h2o, keq = 1. 8 x 109. If we add a strong acid it reacts only with: h3o+ + ch3coo- ch3cooh + h2o, keq = 5. 6 x 1014, the k is always going to be product favored, and limiting reactants come into play here. 0. 10 mol of sodium acetate is added: always write the reaction first, ph before: ch3cooh + h2o ch3coo- + h3o, k = 1. 8 x 10-5.
