Mark H.

asked • 03/15/22

Would it increase the acid concentration?

The actual concentration of the NaOH used was 0.125 M, how would this error affect the calculation of the Molarity of an unknown acid?


Christen H.

tutor
Hi Mark! I am slightly confused on what you are asking it seems like you have left information out.
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03/16/22

Mark H.

thats how the question is worded
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03/16/22

Christen H.

tutor
That is the entire question? It seems that it is asking about a titration but there is no information on the said titration.
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03/16/22

1 Expert Answer

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JACQUES D. answered • 03/16/22

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I assume that you are titrating the acid with the "known" NaOH solution. When titrating a monoprotic acid, the titration equation for the equivalence point is


MAVA = MBVB A = acid, B=Base


When you solve for MA= MBVB/VA you "know MB" , you set VA, and you get VB from experiment.


If MB is lower than expected and used in the equation, more volume of base will be needed to neutralize the acid. This results in calculating a higher concentration of the acid than it actually is.

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Mark H.

thank you so much
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03/16/22

JACQUES D.

tutor
If it is a titration, then the acid concentration is what it is. As I said, if you are thinking that the standard base is higher concentration than it really is, you will think that the acid is higher than it really is. If your mistake is in the other direction, that makes the conclusion go the other way.
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03/16/22

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