Question: answer question 3 1. Calculate the concentration that OH must exceed in a 0.010M solution of Fe(NO3), in order to precipitate Fe(OH)3. 2. Using the

answer question 3

1. Calculate the concentration that OH must exceed in a 0.010M solution of Fe(NO3), in order to precipitate Fe(OH)3. 2. Using the Fe(OH), solution in problem 1, calculate the solubility of Fe(OH); in grams per liter in a solution buffered at a pH of 3.0. Explain using solubility calculation why Fe(OH)3 will be more or less soluble at a pH of 9.0. 3. (Think question). At what pH should the solution be buffered to only precipitate out Fe(OH)3 when your sample solution contains Fe+3 and Cu 2 ions. If this is not possible, then explain why using solubility rules

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