Asked by Anonymous
How many moles of Fe(OH)2 will dissolve in 1.00L of water buffered at pH = 12.00? Fe(OH)2 has Ksp = 1.8 Ã 10^-15.
How would I do this? Should I make an ice table? I know the pOH = 2.00.
How would I do this? Should I make an ice table? I know the pOH = 2.00.
Answers
Answered by
DrBob222
Ksp = (Fe^2+)(OH^-)^2.
If pOH is 2 then OH^- is 10^-2 or 0.01. Plug that in, solve for (Fe^2+) and that will be the solubility in mols/L. You have 1 L of solution so that is the # mols.
If pOH is 2 then OH^- is 10^-2 or 0.01. Plug that in, solve for (Fe^2+) and that will be the solubility in mols/L. You have 1 L of solution so that is the # mols.
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