Asked by SarahF275

'Given 1.760 L of 0.384 M acid and 0.834 L of 0.724 base, find the final pH. Both the acid and base are strong.'

First I multiplied the volume by the molarity to find the moles of each.

Then I came up with this equation:
HX + YOH --> H2O + YX

(Y isn't yttrium; it's just some base Y)

And I made an ICE chart:

HX_____YOH_____YX
0.676___0.604___0
-0.604__-0.604__+0.604
0.072_____0_____0.604

I figured that since there was excess acid, that would determine the pH, so I took -log(0.072) and got a pH of about 1.143.

I'd just like to know if I'm doing this right, as there are give more problems like this and I don't want to do all of them only to find I'm messing up somewhere.

Thanks!
Answered by bobpursley
The thing in my mind is are the base, acid monoprotic?
Answered by bobpursley
help. I dont see a way.
Answered by SarahF275
Unfortunately I don't know. The problem only calls them a strong base and a strong acid, so I assumed they were monoprotic.
Answered by DrBob222
There is no way without knowing. If you know both are monoprotic it works ok. If both are diprotic it works OK, too. except that there are two H or OH in the excess reagent.
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