posted by THOMAS on .
hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question.
What is the pH when enough 0.10 M NaOH Base (in mL) is added to neutralize 8 mL of 0.10 M HC2H3O2 Acid? HCl Acid?
I already solved for the pH of HCl and HC2H3O2 for the previous questions, but this question puzzles me because they do not really give you that much information to solve the question. What gets plugged into the pH = pKa + log(base/acid) equation? We do not have a value for pKa or the log(base/acid).
This is what was sent to Sara:
"When a strong acid is added (exactly neutralized) to a strong base, the salt produced is neutral (neither cation nor anion is hydrolyzed) and the pH = 8.
When a weak acid and a salt of the weak acid are present in solution, you have a buffered solution and you must use the Henderson-Hasselbalch equation to solve for the pH.
pH = pKa + log [(base)/(acid)]"
Wouldn't the pH be 7 for the strong acid, not 8? I'm confused....
Thomas, I just finished answering this question at your original post. Take a peek at that and if you don't understand what I have written, re-post here and I'll pick it up.