Ionic EquilibriumHard
Question
What is the solubility of Al(OH)3, (Ksp = 1 × 10-33) in a buffer solution pH = 4 ?
Options
A.10-3 M
B.10-6 M
C.10-4 M
D.10-10 M
Solution
pH = 4 ⇒ [H+] = 10-4 M ⇒ [OH-] = 10-10 M
Al (OH)3 ⇋ Al+3 + 3OH-
Ksp (Al (OH)3) = [Al+3] [OH-]3
[Al3+] [OH-]3 = 1 × 10-33
[Al3+] (10-10)3 = 1 × 10-33 ⇒ [Al+3] = 10-3 M
Al (OH)3 ⇋ Al+3 + 3OH-
Ksp (Al (OH)3) = [Al+3] [OH-]3
[Al3+] [OH-]3 = 1 × 10-33
[Al3+] (10-10)3 = 1 × 10-33 ⇒ [Al+3] = 10-3 M
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