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1. The problem statement, all variables and given/known data

What is the pH of a solution in which 30.0mL of 0.010 M NaOH are added to 10.0mL of .010 M H2SO4?

2. Relevant equations

3. The attempt at a solution

So first thing I did was write the equation.

2NaOH + H2SO4 ----> Na2SO4 + 2H2O

I never used this equation after this which makes me think I already messed up. I perform the following:

.03L(.010M) = 3*10^-4 mol NaOH

.01L(.010M) = 1*10^-4 mol H2SO4

I then compute concentration of H2SO4 by: 1*10^-4/.01L = .01

pH = -log(.01) = 2.0 pH

I suspect I am missing something here. Any pointers?

Thanks

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# Homework Help: PH of solution

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