'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.'

Question

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!

Answer 1

The thing in my mind is are the base, acid monoprotic?

Answer 2

help. I dont see a way.

Answer 3

Unfortunately I don't know. The problem only calls them a strong base and a strong acid, so I assumed they were monoprotic.

Answer 4

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.