Calculate the pH of a mixture containing 50.0 mL (0.50M) H2SO4 and 50.0 ml (0.50M) NaOH.
I have no idea where to start!I need a walk through if possible! I've tried everything and I get the wrong answer every time!
My calculator is on the blink; I can't do a calculation.
H2SO4 + NaOH ==> H2O + NaHSO4
NaHSO4 + NaqOH ==> H2O + Na2SO4
50 mL H2SO4 x 0.5M = 25 millimoles.
50 mL NaOH x 0.50M = 25 mmols.
Therefore, the first H must have been replaced and you are left with NaHSO4 in the solution at the equivalence point. (NaHSO4) = 25 mmols/100 mL = 0.25M
.....HSO4^- + H2O ==> H3O^+ + SO4^2-
I....0.25..............0.......0
C....-x................x.......x
E....0.25-x...........x.........x
k2 = (H^+)(SO4^2-)/(HSO4^-)
Substitute and solve for (H^+) then convert to pH.