AcidBase_ICETables - So How Much Do We Really Have Strong...

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So How Much Do We Really Have? Strong and Weak Acid-Base Equilibrium and ICE tables (again!)
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Today’s Topics Solve problems that involve strong acids Solve problems that involve strong bases Solve problems that involve weak acids Solve problems that involve weak bases Use ICE tables ! Use equilibrium expression.
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What is the pH of a 1.3 x 10 -4 M solution of HCl? HCl + H 2 O H 3 O + + Cl - pH = -log [H 3 O + ]= -log (1.3 x 10 -4 M) = 3.89 What is the [H 3 O + ] of a solution with a pH of 8.4? pH = -log [H 3 O + ] 10 -pH = 10 -8.4 Strong Acids in Water Strong acids dissociate completely in water (K a >> 1) = 3.98 x 10 -9 M = [H 3 O + ] What is the [OH - ] of a solution with a pH of 8.4? [OH - ] = 10 -14 / [H 3 O + ] = 10 -14 / 3.98 x 10 -9 M = 2.52 x 10 -6 M
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Weak Acids in Water: Example 1 Weak acids do not dissociate completely in water (K a << 1) These must be solved as equilibrium problems A 0.035M solution of a weak acid (HA) has pH = 4.88 What is the K a of the acid? HA(aq) + H 2 O(l) H 3 O + (aq) + A - (aq) pH = 4.88 = -log[H 3 O + ] [H 3 O + ] eq = 10 -4.88 = 1.3 x 10 -5 M = [A - ] eq x = 1.3 x 10 -5 M Molarity HA (aq) H 3 O + (aq) A - (aq) I E C 0.035 0 0 1.3 x 10 -5 -x +x +x 0.0349 1.3 x 10 -5 K a = [H 3 O + ] [A - ] [HA] = (1.3 x 10 -5 M)(1.3 x 10 -5 M) 0.0349M = 4.8 x 10 -9 M Let x = [HA] that dissociates
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Weak Acids in Water: Example 2 Hydrofluoric acid, HF, has a K a of 6.8 x 10 -4 What are the [H 3 O + ], [F -
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This note was uploaded on 01/09/2011 for the course SCIENCE 12084 taught by Professor Mrdavidbyrum during the Spring '10 term at Harrison College.

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AcidBase_ICETables - So How Much Do We Really Have Strong...

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