Lecture 10

Lecture 10 - Today PS 4 Assigned Finishing Chapter 7 1...

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1 Today: PS 4 Assigned, Finishing Chapter 7
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2 Water can donate or accept a proton (Amphiprotic) K w = [H 3 O + ][OH - ] = 1.00 x 10 -14 (298K) 0.25M HCl: 2H 2 O (l) H 3 O + (aq) + OH - (aq) Autoionization of Water It is both an acid and a base, even in pure water (Amphoteric) [H 3 O + ] = [OH - ] = 1.00 x 10 -7 M [H 3 O + ] = 0.25M; [OH - ] = 4.00 x 10 -14 M [H 3 O + ] = 1.34 x 10 -3 M; [OH - ] = 7.46 x 10 -12 M Pure Water: 0.10M Acetic Acid
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3 pH = -log 10 [H 3 O + ] pOH = -log 10 [OH - ] The pH and pOH Scale Pure Water: [H 3 O + ] = [OH - ] = 1.00 x 10 -7 M 0.25 M HCl: [H 3 O + ] = 0.25M [OH - ] = 4.00 x 10 -14 M 0.10 M Acetic Acid: [H 3 O + ] = 1.34 x 10 -3 M [OH - ] = 7.46 x 10 -12 M 0.25M Ammonia: [OH - ] = 2.12 x 10 -3 M [H 3 O + ] = 4.72 x 10 -12 M pH = pOH = 7.00 pH = 0.60 pOH = 13.40 pH = 2.87 pOH = 11.13 pOH = 2.67 pH = 11.33 K w = [H 3 O + ][OH - ] = 1.00 x 10 -14 (at 298 K) -log 10 K w = -log 10 [H 3 O + ] - log 10 [OH - ] = -log 10 (1.00 x 10 -14 ) pK w = pH + pOH = 14.00 (at 298 K)
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Strong Acid or Base: Fully ionized-- Percent ionization always 100. Weak Acid or Base: Percent ionization increases
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Lecture 10 - Today PS 4 Assigned Finishing Chapter 7 1...

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