# pH value of a buffer solution of HClO and NaClO [closed]

So,
I have 200mL of HClO 0,64M.
I mix it with 0,1mol of NaClO.
How should I calculate the pH?

So far this is what I've done.

Considering:

$\ce{NaClO + H2O -> Na+ + ClO-}$

With n(NaClO) = n(ClO-) = 0.1mol,

I calculated the molarity of the conjugate base:

[ClO-] = 0.1mol/0.2L = 0.5M.

Then I applied the Henderson-Hesselbalch equation:

pH = pKa + log([ClO-]/[HClO]) = 7.53 + log(0.781M) = 7.422

In this case I didn't consider the variation to the solution volume due to the addition of NaClO. So, is this correct?

• This is a homework question. We have a policy which states that ‎you should show your thoughts and/or efforts into solving the problem. It'll make us certain that ‎we aren't doing your homework for you. Otherwise, this question may get closed.‎ Please edit in your full reasoning or thoughts on this. – airhuff Nov 24 '17 at 19:48
• I'm a college student, this is not a homework question. I've already solved it but I'm not sure about the result. I would like to compare my result with someone who know exactly how to solve it. – Scanfi98 Nov 24 '17 at 19:55
• Please see the homework link in my above comment to learn what qualifies as a homework type of question and how to ask one. You can get help with this here, you just need to follow the guidelines. Best of luck. – airhuff Nov 24 '17 at 19:59
• In addition to the problem that this would be considered a homework question, it also qualifies as an amirite question (seeks to consider confirmation or clarification on an already derived answer) which we have determined to be a bad fit for the site. – Jan Nov 25 '17 at 13:10