Two aqueous solutions are mixed: 50.0 mL of 1.60×10−2 M H2SO4 and 50.0 mL of 3.75×10−2 M NaOH.

Question

Two aqueous solutions are mixed: 50.0  mL of 1.60×10−2 M  H2SO4 and 50.0  mL of 3.75×10−2 M   NaOH.

what is the PH of the following solution?

Anonymous · Accepted Answer

so what the h is the answer

DrBob222 · Answer

The trick to these question is to recognize what you have in the final solution.
Write the equation.
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O

moles H2SO4 = M x L = ??
moles NaOH = M x L= ??
moles H2SO4 required to use all of it will be moles H2SO4 x 2 (since there are two moles NaOH for every mole of H2SO4). Look at those numbers, see which is in excess and use that to calculate either the OH or the H depending upon the one in excess.

Post your work if you get stuck.