Hi chemical forums!

I've been visiting this site for a while now, i havent really needed to post anything before, but im stuck on this homework problem for a while now, and i cant figure out where I'm wrong.

Given that the stepwise dissociation constants for phosphoric acid are:

Ka1 = 7.5×10-3; Ka2 = 6.2×10-8; Ka3 = 4.8×10-13

We need to find mass of Na2HPO4 and NaH2PO4 needed to make a buffer of 1.10 L, having ionic strength of 0.090 and a pH of 7.45. Assume all activity coefs are 1

so what I did

1) Use Henderson-Hasselbalch equation to find the ratio between two conjugate bases.

pH=pKa + log[A-]/[A--])

7.45=-log(6.2*10^-8)+log([A-]/log[A--])

log([A-]/[A--])= 0.2424

2) Use ionic strength formula to find relationship between these two conjugate bases.

u = [A-] + 3[A--]

u=[NaH2PO4] + 3[Na2HPO4]=0.090

so we have

log([NaH2PO4]/[Na2HPO4])=0.2424 and

[NaH2PO4] + 3[Na2HPO4]=0.090

so our equation becomes

Take x for [NaH2PO4] and y for [Na2HPO4]

7.45=-log(6.2*10^-8)+log((0.09-3*y)/y)

from this, y=0.018958 M

mol(Na2HPO4)= 0.018958 *1.1 L= 0.020854 mol

m(Na2HPO4)=0.020854 mol* 141.95896 g/mol = 2.96 g

However, entering this result leads to an error.

For NaH2PO4 it's same.

I'm not sure where im doing wrong, any help would be appreciated.