So we're doing a Neutralization Lab, help please on the concepts?
So the lab begins with us adding Acetic Acid, a weak acid, in an Erlenmeyer Flask, a certain quantity. Then we are suppose to use our Buret, after adding the Indicator, to drip NaOH(Sodium Hydroxide) into the Erlenmeyer Flask by 2mL at a time.

So the problem I have is mainly on the pre-lab questions: One of the question goes:
"Calculate the Equivalence point when 50.0 mL of 0.10M Acetic Acid is neutralized by 0.10 M NaOH"

Question

So we're doing a Neutralization Lab, help please on the concepts?
So the lab begins with us adding Acetic Acid, a weak acid, in an Erlenmeyer Flask, a certain quantity. Then we are suppose to use our Buret, after adding the Indicator, to drip NaOH(Sodium Hydroxide) into the Erlenmeyer Flask by 2mL at a time.

So the problem I have is mainly on the pre-lab questions: One of the question goes:
"Calculate the Equivalence point when 50.0 mL of 0.10M Acetic Acid is neutralized by 0.10 M NaOH"

anonymous · Answer

Find But some of my classmates keep on telling me that the equivalence point IS the Neutralization point, but I don't understand: Acetic Acid is a weak acid, and the Molarity and the Volume of the NaOH and Acetic Acid are both equal, therefore their moles are equal.

SO if their moles are equal... and Acetic Acid will dissolve in few quantity, and give off less H+, how is it neutralized? At that point, won't there be way more OH- than H+? In fact, all of the H+ will be consumed and the solution would be basic and pH will be higher than 7!

Am I missing something here about Neutralization Reactions and Equivalence point or something else? Please help!