Assuming you titrate both solutions with the same NaOH titrant AND that you are able to titrate to the exact equivalence point, the HCl and the CH3COOH will require the same volume of NaOH BECAUSE:
the equivalence point is reached when moles HCl = moles NaOH and when moles CH3COOH = mols NaOH.
moles HCl = M x L = 0.1 M x 0.01 L = 0.001 moles
moles CH3COOH = 0.1 M x 0.01 L = 0.001 moles
Therefore, both titrations will be the same.
A caveat: I note that you use the term "end-point" and not equivalence point. IF THE INDICATOR YOU USE IS SUCH THAT THE END POINT AND THE EQUIVALENCE POINT IS NOT THE SAME YOU WILL SEE A DIFFERENCE.
Suppose you have two solutions to titrate with NaOH:
(a) 10 mL of 0.1 M HCl, and
(b) 10 mL of 0.1 M CH3COOH.
Would you expect either of the solutions to require different volumes of NaOH in
order to reach an end-point? Explain your answer.
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3 answers