Amount of base needed to titrate to pH 10.00

[Teemo]

Homework Statement

A 50.0 mL sample of a 1.00 M solution of a diprotic acid
H₂A (Ka₁ = 1.0 × 10^–6
and Ka₂ = 1.0 × 10^–10) is titrated
with 2.00 M NaOH. What is the minimum volume of
2.00 M NaOH needed to reach a pH of 10.00?
(A) 12.5 mL
(B) 37.5 mL
(C) 25.0 mL
(D) 50.0 mL

Homework Equations

pH=-log[H⁺]

The Attempt at a Solution

I believe I am missing something extremely obvious. I find that NaOH, being a strong base will completely neutralize the acid and then additional base will be required to have the pH reach 10.00. So I found moles of hydrogen, being .05*1.00.*2. I then divided by molarity of the NaOH to find volume of NaOH required to completely neutralize it, and find 50.0 mL. Now this is where I get confused. D is the highest answer, and only has enough base to neutralize the acid, not to dissociate and to increase pH.

 

[Borek]

Not all acid is neutralized at pH 10.0.

Do you know when pH=pKa?

 

[Teemo]

Oh wow, sorry, I'm stupid. Thanks.