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Any pchem experts out there? I need a 2nd opinion on a problem.
If I make a soln. of 0.2 M NaH2PO4 and 0.2 M Na2HPO4, what is the concentration of PO4 -3? pKa's for phosphoric acid are 2.23, 7.31, and 12.74.
Here's what I was thinking, I just need a 2nd opinion...
H2PO4 and HPO4 should make a buffer soln:
so pH = pKa(H2PO4) + log ([HPO4]/[H2PO4])
pH = pKa(H2PO4) + 0
pH = 7.31
so [H+] = 4.9 * 10^-8 M
to get [PO4 ]
The Ka for the pKa of 12.74 is 1.82 * 10^-13
Ka = [H+][PO4]/[HPO4]
if [PO4] = x;
x = (Ka * [HPO4]) / [H+]
x = ((1.82 * 10^-13)(0.2 - x)) / (4.9 * 10^-8)
x = ((1.82 * 10^-13)(0.2)) / (4.9 * 10^-8)
x = 7.24 * 10^-7 M
That's what I first though, but I just want a second opinion. Do I need to take into accound any H2PO4 being converted to H3PO4 or anything like that?
If I make a soln. of 0.2 M NaH2PO4 and 0.2 M Na2HPO4, what is the concentration of PO4 -3? pKa's for phosphoric acid are 2.23, 7.31, and 12.74.
Here's what I was thinking, I just need a 2nd opinion...
H2PO4 and HPO4 should make a buffer soln:
so pH = pKa(H2PO4) + log ([HPO4]/[H2PO4])
pH = pKa(H2PO4) + 0
pH = 7.31
so [H+] = 4.9 * 10^-8 M
to get [PO4 ]
The Ka for the pKa of 12.74 is 1.82 * 10^-13
Ka = [H+][PO4]/[HPO4]
if [PO4] = x;
x = (Ka * [HPO4]) / [H+]
x = ((1.82 * 10^-13)(0.2 - x)) / (4.9 * 10^-8)
x = ((1.82 * 10^-13)(0.2)) / (4.9 * 10^-8)
x = 7.24 * 10^-7 M
That's what I first though, but I just want a second opinion. Do I need to take into accound any H2PO4 being converted to H3PO4 or anything like that?