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Ch. 19 Acids & Bases II. pH
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H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0 10-14
A. Ionization of Water H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0 10-14
![H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0 10-14](http://slideplayer.com./slide/14077406/86/images/2/H2O+%2B+H2O+H3O%2B+%2B+OH-+Kw+%3D+%5BH3O%2B%5D%5BOH-%5D+%3D+1.0+%EF%82%B4+10-14.jpg "A. Ionization of Water. H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0 ")
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A. Ionization of Water Find the hydroxide ion concentration of 3.0 10-2 M HCl. [H3O+][OH-] = 1.0 10-14 [3.0 10-2][OH-] = 1.0 10-14 [OH-] = 3.3 M Acidic or basic? Acidic
![A. Ionization of Water Find the hydroxide ion concentration of 3.0 10-2 M HCl. [H3O+][OH-] = 1.0 ](http://slideplayer.com./slide/14077406/86/images/3/A.+Ionization+of+Water+Find+the+hydroxide+ion+concentration+of+3.0+%EF%82%B4+10-2+M+HCl.+%5BH3O%2B%5D%5BOH-%5D+%3D+1.0+%EF%82%B4.jpg "[3.0 10-2][OH-] = 1.0 [OH-] = 3.3 M. Acidic or basic Acidic.")
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pouvoir hydrogène (Fr.)
B. pH Scale 14 7 INCREASING ACIDITY INCREASING BASICITY NEUTRAL pH = -log[H3O+] pouvoir hydrogène (Fr.) “hydrogen power”
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pH of Common Substances
B. pH Scale pH of Common Substances
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pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14
B. pH Scale - Formulas pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14
![pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14](http://slideplayer.com./slide/14077406/86/images/6/pH+%3D+-log%5BH3O%2B%5D+pOH+%3D+-log%5BOH-%5D+pH+%2B+pOH+%3D+14.jpg "B. pH Scale - Formulas. pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14.")
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B. pH Scale What is the pH of 0.050 M HNO3? pH = -log[H3O+]
Acidic or basic? Acidic
![B. pH Scale What is the pH of M HNO3 pH = -log[H3O+]](http://slideplayer.com./slide/14077406/86/images/7/B.+pH+Scale+What+is+the+pH+of+M+HNO3+pH+%3D+-log%5BH3O%2B%5D.jpg "Acidic or basic Acidic.")
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B. pH Scale What is the molarity of HBr in a solution that has a pOH of 9.6? pH + pOH = 14 pH = 14 pH = 4.4 pH = -log[H3O+] 4.4 = -log[H3O+] -4.4 = log[H3O+] [H3O+] = 4.0 10-5 M HBr Acidic
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