If you are asking what is the dissociation constant (Kb) for HPO₄², you want be able to solve for it with the information given; you have to look up the Ka for HPO₄² in a book.
Ka for HPO₄²=4.2 x10^-13
Solving for Kb,
Kb=Kw/Ka= 1 x 10^-14/4.2 x10^-13 =2.40 x 10^-2
This answer is not one of your answer choices, so I'm a little stuck on this one.
It's Kw/k2 for H3PO4.
I'm sure you remember Kw = 1E-14.
How do you know which ka to use? There is one on the base side of the chart, and one of the acid side of the chart. For the one of the acid side of the chart, the Ka is 2.2*10^-13 And for the one on the base side of the chart, it is 6.2*10^-8.
With that being said,
Kb=Kw/Ka= 1 x 10^-14/6.2 x10^-8 =1.6 x10^-7
Thanks so much :) So if we were to find the Ka, then we would use the ka on the acid side of the chart?
Correct me if I'm wrong but
HPO4^2- + HOH ==> H2PO4^- + OH^-
k3 for H3PO4= 4.2E-13 = (H^+)(PO4^3-)/(HPO4^-) and that doesn't contain the ions needed for HPO4^2- to act as a base. k2 for H3PO4 does.
k2 = (H^+)(HPO4^2-)/(H2PO4^-)
I think the answer is c.
Yes, the way your reference is set-up. Remember, Kw= Ka*Kb. if you want to know the Kb, you need to know the Kw and Ka. If you want to know the Kb, you need to know the Ka and Kw.
Its c, I used the wrong Ka value when I initially did it.
Thanks soo much to both of you :)
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