Asked by Manali
What is the pH of the solution created by combining 12.40 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)?
I know how to solve for HCl but not with HC2H3O2.
with 8.00 mL of the 0.10 M HC2H3O2(aq)?
I know how to solve for HCl but not with HC2H3O2.
Answers
Answered by
DrBob222
NaOH + HC2H3O2 ==> NaC2H3O2 + H2O
moles NaOH = M x L = ??
moles HC2H3O2 = M x L = ??
See which is in excess when NaOH is added to HC2H3O2. If NaOH is in excess the pH is determined by excess OH. If HC2H3O2 is in excess, then you have a mixture of acetic acid and sodium acetate which is a buffer and you use the Henderson-Hasselbalch equation.
moles NaOH = M x L = ??
moles HC2H3O2 = M x L = ??
See which is in excess when NaOH is added to HC2H3O2. If NaOH is in excess the pH is determined by excess OH. If HC2H3O2 is in excess, then you have a mixture of acetic acid and sodium acetate which is a buffer and you use the Henderson-Hasselbalch equation.
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