What is the pH of the solution created by combining 11.40 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)?
with 8.00 mL of the 0.10 M HC2H3O2(aq)?
Here is the chart that i am supposed fill out:
mL NaOH pH w/ HCl pH w/ HC2H3O2
11.40 _________ ____________
Here's the second part of the problem.
I need to complete the chart too
mL NaOH pH w/ HCl pH w/ HC2H3O2
11.40 _________ _____________
The charts make no sense to me. Actually, the problem, as stated, doesn't make a lot of sense, either. What about re-writing and/or re-posting it in standard format. If there are two problems, make two problems out of it.
IF the first problem is a mixture of NaOH and HCl, it is done this way.
NaOH + HCl ==> NaCl + H2O
Determine moles NaOH. M x L = moles NaoH.
Determine moles HCl. M x L = moles HCl.
Subtract one from the other, determine which is in excess (I think it is NaOH in excess) divide moles excess by volume in liters and that will give you the OH^-. Then pOH = -log(OH^-) and pH = 14 - pOH.
It appears that the second part of the problem is an attempt at making a buffered solution but I can't tell what is what.