4.11: pH and pOH Chemistry 12.

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Presentation transcript:

4.11: pH and pOH Chemistry 12

4.11 Math Review Log 10(1000)= 3 103 = 1000

4.11 Math Review Log 10(1000)= 3 103 = 1000

4.11 pH scale Tells us if solution is acidic, basic or neutral Is calculated using [H3O+] Is an easier way to communicate [H3O+] Water has a pH of seven The concentration of the hydronium ion in water is 1.0 x 10-7

4.11 pH formula pH = -log [H3O+]

In pH, only digits after the decimal are considered significant 4.11 E.g. What is the pH of 0.0035 M HCl? pH = -log [H3O+] pH = -log [0.0035] pH = 2.4555931956 = 2.46 In pH, only digits after the decimal are considered significant

4.11 What is pOH of last example? pH + pOH =14 14 – pH = pOH 14 – 2.4559 = 11.54

4.11 E.g. What is [H3O+] of a solution with a pH of 11.50? [H3O+] = 10(-pH) [H3O+] = 10(-11.50) = 3.16227766 x 10-12 = 3.2 x 10-12 2 sig figs 2 sig figs

Recall: pH =11.50 & we calculated [H3O+] 4.11 [OH-] of last example? (2 possible ways) [OH-] = Kw/ [H3O+] = 1.0 x 10-14/ 3.16227766 x 10-12 = 3.2 x 10-3 pOH = 14 – 11.50 = 2.50 [OH-] = 10(-pOH) = 10(-2.50) Recall: pH =11.50 & we calculated [H3O+]

4.11 Summary

[H3O+] [OH-] pOH pH Kw = [H3O+]=10-pH [OH-][H3O+] pH = -log [H3O+] 14= pH+ pOH pOH = -log [OH-]

Calculations Assignment (p. 12-19) 4.11 Read & Highlight Calculations Assignment (p. 12-19) Hebden # 47-57