A groundwater contains 1.8 mg/L of iron as Fe 3+. What pH is required to precipitate all but 0.30 mg/L of the iron at 25 C?
2006-09-24 17:11:16 · 2 answers · asked by HH 1 in Science & Mathematics ➔ Chemistry
To solve it consider that PO4(3-) is a weak base...
I'll need the Ka of its conjugate acid, to work this out...
actually this is a bad problem... since PO4(3-) can accept up to 3 protons from water, giving the system a buffering effect...
also, I think your teacher wants you to go with
Ks = {Ferric Ion} {Phosphate Ion}
10^-21.9 = (0.0018 g/ 55.85 g/mol) {Phosphate concentration}
Get the phosphate concentration and work out the pH from it's Kb (or its conjugate acid's Ka) I assume you know how to do this...
2006-09-24 17:30:33 · answer #1 · answered by kb27787 2 · 0⤊ 0⤋
Doing your homework here, eh?
I can't help you; good luck!
:-)
2006-09-25 00:14:36 · answer #2 · answered by ThomasR 4 · 0⤊ 2⤋