If the Ksp for aluminum hydroxide is 1.9 x 10-33, calculate the solubility (in mol/liter) of Al(OH)3 in a solution of 0.100 M NaOHA1.9 x 10-30 B1.9 x 10-36 C7.0 x 10-32 D5.1 x 10-35 E2.9 x 10-9 The answer is A, but why? i tried dividing the values but get the power of -32someone please explain quickly?
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First, write out the ksp expression: ksp 1.9x10^-33 [Al 3+] [OH-]^3 Next, fill in the given info, or do an ICE chart: 1.9x10^-33 (x) (0.100 + 3x)^3 0.100 + 3x rounds to just 0.100 because 3x is negligible 1.9x10^-33 (x) (0.100)^3 Solve using simple algebra: x 1.9x10^-30 -Hope this helps
