Posted by **anonymous** on Sunday, April 11, 2010 at 6:19am.

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?

- chemistry -
**DrBob222**, Sunday, April 11, 2010 at 1:40pm
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.

- chemistry -
**Anonymous**, Thursday, July 11, 2013 at 7:39am
so what the h is the answer

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