calculate the equilibrium pH of an aqueous solution thatcontains 2.55 g of Al(OH

Question

calculate the equilibrium pH of an aqueous solution thatcontains 2.55 g of Al(OH)3 (s) (ignore the contribution of waterionization on pH) ksp= 2.00x10-32. also, what is activitycoefficient of Al3+ i found the molar solubility and therefore the concentrationof OH- to get the pOH and then pH. where do i take intoaccount the 2.55g? calculate the equilibrium pH of an aqueous solution thatcontains 2.55 g of Al(OH)3 (s) (ignore the contribution of waterionization on pH) ksp= 2.00x10-32. also, what is activitycoefficient of Al3+ i found the molar solubility and therefore the concentrationof OH- to get the pOH and then pH. where do i take intoaccount the 2.55g?

Explanation / Answer

the coefficient of Al3+ would be one: Al(OH)3 --> Al3+ + 3OH- I approached your question the same way you did. I don't think youneed the 2.55 g. It is probably extra information. My answer was: pH = 5.72

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