Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: whitefloss on November 16, 2019, 09:39:15 PM
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For my lab I ran into a bit of a problem.
In this scenario, I will be given an unknown concentration of approximately 1.0M of HCl and and unknown concentration of approximately 0.1M of NaOH. I also have to use 100mL of KHP in this lab to standardize the NaOH first. The lab states that I will be given 100mL of unknown conc. of HCl. The goal of the lab is to find the unknown concentration of HCl.
From basic stoichiometry knowledge, I know that I'll require 1 litre of ~0.1M of NaOH to neutralize 100mL of ~1.0M of HCl. I am confused as to how I am supposed to titrate 1 litre of NaOH since we usually use a 50mL buret to titrate. I tried diluting the amount of 1.0M of HCl but I am still required to titrate a large amount of NaOH. If you could tell me how I am interpreting this wrong that would be great.
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I am confused as to how I am supposed to titrate 1 litre of NaOH
You don't titrate all the acid at once, you titrate several small aliquots.
What volume of NaOH would be needed if you take a 5 mL aliquot of the acid?
Also: don't dilute HCl you were given, that will introduce an additional error.