Ok, here it is:
A solution of CaF2 has [Ca++] = 3.1 x 10^-4 and [F-] = 1.5 x 10^-3. If PbI2 has Ksp = 3.9 x 10^-11, then will a precipitate form in the solution?
I know that it sounds like that's not all to the question, but it is. This one truly has me stumped. Does anyone know the answer?
2007-04-18 16:20:02 · 4 answers · asked by Random G 3 in Science & Mathematics ➔ Chemistry
The solution does not contain Pb++ so the PbI2 Ksp is irrelevant. You need to know the Ksp of calcium fluoride then do the math to see if it is exceeded.
Is [Ca++]*[F-]^2 > Ksp ?
2007-04-18 16:42:31 · answer #1 · answered by Robert J 2 · 0⤊ 0⤋
You have a Ksp of PbI2 and yet the given concentration are for Ca2+ and F-. I think you mixed up two problems..
2007-04-22 23:18:58 · answer #2 · answered by rEi 3 · 0⤊ 0⤋
geeeeze! Math is my worse subject, yet I am studying to be an RN. This is going to be a LONG, HARD summer session!
2007-04-18 23:27:44 · answer #3 · answered by Anonymous · 0⤊ 0⤋
Question does not make any sense, incomplete data.
2007-04-19 00:02:15 · answer #4 · answered by ag_iitkgp 7 · 0⤊ 0⤋