Problem: The Ksp of Al(OH)3 is 2 X 10-32. At what pH will a 0.2-M Al 3+ solution begin to show precipitation of Al(OH)3?

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Al(OH)3(s) Al3+(aq) + 3 OH(aq)

Ksp=productsreactantsKsp=[Al3+][OH-]32.0×10-32=(0.2 M)(3x)3

2.0×10-32=(0.2)(27x3)2.0×10-325.4=5.4x35.43.7037×10-333=x33

x = 1.5472x10-11

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The Ksp of Al(OH)3 is 2 X 10-32. At what pH will a 0.2-M Al 3+ solution begin to show precipitation of Al(OH)3?

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