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pH of Common Substances Timberlake, Chemistry 7 th Edition, page 335

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Calculating pH pH = -log [H + ] So if [H + ] = 1x10 -5 pH = - log (1x10 -5 ) = 5 Calculate the pH if [H + ] = 1 x 10 -2 MpH = [H + ] = 3.0 x 10 -6 MpH = [H + ] = 8.2 x 10 -6 MpH =

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Convert pH to [H + ] 10 -pH = [H + ] If pH = 5, 10 -pH = 10 -5 = 0.000 01 = 1 x 10 -5 M Calculate the [H+] if pH = 2.37[H + ] = pH = 11.05[H + ] = pH = 6.50[H + ] =

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pH of Common Substance 14 1 x 10 -14 1 x 10 -0 0 13 1 x 10 -13 1 x 10 -1 1 12 1 x 10 -12 1 x 10 -2 2 11 1 x 10 -11 1 x 10 -3 3 10 1 x 10 -10 1 x 10 -4 4 9 1 x 10 -9 1 x 10 -5 5 8 1 x 10 -8 1 x 10 -6 6 6 1 x 10 -6 1 x 10 -8 8 5 1 x 10 -5 1 x 10 -9 9 4 1 x 10 -4 1 x 10 -10 10 3 1 x 10 -3 1 x 10 -11 11 2 1 x 10 -2 1 x 10 -12 12 1 1 x 10 -1 1 x 10 -13 13 0 1 x 10 0 1 x 10 -14 14 NaOH, 0.1 M Household bleach Household ammonia Lime water Milk of magnesia Borax Baking soda Egg white, seawater Human blood, tears Milk Saliva Rain Black coffee Banana Tomatoes Wine Cola, vinegar Lemon juice Gastric juice More basic More acidic pH [H 1+ ] [OH 1- ] pOH 7 1 x 10 -7 1 x 10 -7 7

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pOH pOH= -log [OH - ] 10 -pOH = [OH - ] So if [OH - ] = 4 x 10 -3 M pOH = -log (4 x 10 -3 ) = 2.397 = 2.40 pH + pOH = 14

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[H+][OH-]pHpOH A / B / N 3.2 x 10 -3 1.26 x 10 -5 10.3 7.89

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Complete this for homework… [H+][OH-]pHpOH A / B / N 2.5 x 10 -6 1.0 x 10 -12 12.3 0.9

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Copyright © 2005 Pearson Prentice Hall, Inc. Chapter 2 Atoms, Molecules, and Life.

Copyright © 2005 Pearson Prentice Hall, Inc. Chapter 2 Atoms, Molecules, and Life.

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