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C. Johannesson Ch. 15 & 16 - Acids & Bases II. pH (p. 481 - 491)
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C. Johannesson A. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0 10 -14
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C. Johannesson A. Ionization of Water Find the hydroxide ion concentration of 3.0 10 -2 M HCl. [H 3 O + ][OH - ] = 1.0 10 -14 [3.0 10 -2 ][OH - ] = 1.0 10 -14 [OH - ] = 3.3 10 -13 M Acidic or basic? Acidic
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C. Johannesson pH = -log[H 3 O + ] B. pH Scale 0 7 INCREASING ACIDITY NEUTRAL INCREASING BASICITY 14 pouvoir hydrogène (Fr.) “hydrogen power”
![C. Johannesson pH = -log[H 3 O + ] B.](http://images.slideplayer.com/32/9916539/slides/slide_4.jpg "pH Scale 0 7 INCREASING ACIDITY NEUTRAL INCREASING BASICITY 14 pouvoir hydrogène (Fr.) hydrogen power .")
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C. Johannesson B. pH Scale pH of Common Substances
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C. Johannesson B. pH Scale pH = -log[H 3 O + ] pOH = -log[OH - ] pH + pOH = 14
![C. Johannesson B. pH Scale pH = -log[H 3 O + ] pOH = -log[OH - ] pH + pOH = 14](http://images.slideplayer.com/32/9916539/slides/slide_6.jpg "C. Johannesson B. pH Scale pH = -log[H 3 O + ] pOH = -log[OH - ] pH + pOH = 14")
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C. Johannesson B. pH Scale What is the pH of 0.050 M HNO 3 ? pH = -log[H 3 O + ] pH = -log[0.050] pH = 1.3 Acidic or basic? Acidic
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C. Johannesson B. pH Scale What is the molarity of HBr in a solution that has a pOH of 9.6? pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 Acidic pH = -log[H 3 O + ] 4.4 = -log[H 3 O + ] -4.4 = log[H 3 O + ] [H 3 O + ] = 4.0 10 -5 M HBr
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