Asked by Emmanuel
Ground water intially contains 1.800mg/L of iron as Fe3+. What must the pH be raised to in order to precipitat all but 0.30mg/L of iron. The tempertaure is 25 degrees celcius
Answers
Answered by
DrBob222
Fe(OH)3 ==> Fe^+3 + 3OH^-
Ksp = (Fe^+3)(OH^-)^3
You want (Fe^+3) to be 0.3 mg/L. Change that to moles/L, plug into the Ksp expression, and solve for OH^-, then convert to pH. Post your work if you get stuck.
Ksp = (Fe^+3)(OH^-)^3
You want (Fe^+3) to be 0.3 mg/L. Change that to moles/L, plug into the Ksp expression, and solve for OH^-, then convert to pH. Post your work if you get stuck.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.