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[H 3 O + ] Aqueous Solutions Brackets means concentration (Molarity) 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] acid base M

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Presentation on theme: "[H 3 O + ] Aqueous Solutions Brackets means concentration (Molarity) 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] acid base M"— Presentation transcript:

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2 [H 3 O + ] Aqueous Solutions Brackets means concentration (Molarity) 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] acid base 0.00001 M0.000000001 M HCl + H 2 O H+H+ Cl -1 + H 3 O + contain both 1x10 -5 M >

3 more acidic 1x10 -3 M 1x10 -11 M > 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] NaOH Na +1 + OH -1 Aqueous Solutions acid HCl + H 2 O Cl -1 + H 3 O + 1x10 -3 M

4 more acidic 1x10 -10 M 1x10 -4 M basic < 1x10 -3 M 1x10 -11 M > 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] NaOH Na +1 + OH -1 Aqueous Solutions acid 1x10 -4 M

5 more acidic 1x10 -10 M 1x10 -4 M basic [H + ] x [OH - ]= 1x10 -14 = K w < 1x10 -3 M 1x10 -11 M > Aqueous Solutions 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] acid

6 pH = - log[H 3 0 + ] or pH = - log[H + ] What is the pH of water? Since water’s [H 3 O + ] is 1x10 -7 M, and pH = - log[H 3 0 + ] pH = - log[1x10 -7 ] pH = - [-7] pH = 7

7 more acidic 1x10 -10 M 1x10 -4 M basic < 1x10 -3 M 1x10 -11 M > Aqueous Solutions 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] acid water pH = 7

8 pH Scale 0 14 7 neutral

9 more acidic 1x10 -10 M 1x10 -4 M basic < 1x10 -3 M 1x10 -11 M > Aqueous Solutions 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] acid water pH = 7 pH = 5

10 More acidic pH Scale 0 14 7 neutral 5

11 more acidic 1x10 -10 M 1x10 -4 M basic < 1x10 -3 M 1x10 -11 M > Aqueous Solutions 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] acid water pH = 7 pH = 5 pH = 3

12 More acidic pH Scale 0 14 7 neutral 5 3

13 more acidic 1x10 -10 M 1x10 -4 M basic < 1x10 -3 M 1x10 -11 M > Aqueous Solutions 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] base [H 3 O + ] acid water pH = 7 pH = 5 pH = 3 pH = 10

14 More acidic pH Scale 0 14 7 neutral 5 3 More basic 10

15 What is the pH of a 0.01M HCl solution? HCl + H 2 O Cl - + H 3 O + 0.01M pH = - log[H 3 0 + ] pH = - log[0.01] pH = - [-2] pH = 2 0.01M

16 What is the pH of a 0.01M Ca(OH) 2 solution? Ca(OH) 2 Ca +2 + 2OH -1 0.01M 0.02M pH = - log[H 3 0 + ] pH = - log[5x10 -13 ] pH = - [-12.3] pH = 12.3 0.01M [H 3 O + ] x [OH - ]= 1x10 -14 = K w [H 3 O + ] x [0.02]= 1x10 -14 [H 3 O + ] = 5x10 -13

17 More acidic pH Scale 0 14 7 neutral 5 3 More basic 10 12.3

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