The Ksp of Al(OH)3 is 2 × 10–32. At what pH will a 0.4 M Al3+ solution begin to show precipitation of Al(OH)3?
6.1
1.0
3.6
3.1
10.4
Al(OH)3 <------------> Al+3 + 3OH-
Ksp = [Al+3] [OH-]3
[Al+3] = S moles /L
[OH-] = 3S moles /L
2.0 x 10-32 = [0.4] [3S]3
2.0 x 10-32 = 0.4 x 27 S3
2.0 x 10-32 = 10.8 S3
S3 = 1.85 x 10-33
S = 1.23 x 10-11
[OH-] = 3S = 3 x 1.23 x 10-11 = 3.69 x 10-11M
pOH = - log [OH-]
pOH = - log [3.69 x 10-11]
pOH = 10.4
pH = 14 - 10.4
pH = 3.6
answer = 3.6
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