Calculate the pH of the solution which results from the mixing of 100.0 mL of

0.050 NaOH solution with an equal volume of 0.10 M HCl solution.

 

Seems straight forward to me. Strong acid and a strong base, so they'll react completely. You end up with .05M HCl, which is the molarity of H+, so you can just use -log(.05) to get the pH. I get 1.3.

 

But this is apparently incorrect, the answer given is 1.6. Can someone tell me where I went wrong?

see your other thread on the same

Did you take into account dilution? If you add an equal volume of HCl, you now have 200.0 mL of solution.

yeah i said that in his other thread. seen that one before this. he didn't take into account the dilution.

Ohhhhh right. That crazy dilution. Thanks guys, I knew it was something stupid like that.

Well, you were already told that the problem is in dilution, but here is almost identical pH calculation question with explanation.

 

Best,

Borek

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