Chemical Forums
Chemistry Forums for Students => Analytical Chemistry Forum => Topic started by: RaelAerosolKid on January 07, 2021, 08:17:04 PM
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So we have this titration curve: https://imgur.com/a/SsU9HKB
We have what the question asks you: https://imgur.com/a/GrHaTsb
And all the info that should be necessary: https://imgur.com/a/BcxTwHq
Problem is if I don't even have the concentration of the acids how am I going to answer the first question?
And how am I going to answer the second question? Do I have to guess by looking at the graph that the pH of the diluted solution is something like 0.9 and start from there?
The third question is the only one that seems "doable" to me, but I'm still very lost.
I only asking you guys to "solve" this because I think this can be a really unique question (had never seen something like this) with some really intricate solution.
And I might be totally lost because I'm only beginning to learn analytical chemistry.
Thanks in advance
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What does the statement "if there is still sulfuric acid in the process solution" mean for you - at pH 2 you may expect approximately NH4HSO4/(NH4)2SO4 molar ratio about 1 (this is crude approximation - real pH is about 2.9); real pH of NH4HSO4 solution is about 1.8 and you started titraton ot pH 0.9.
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But... how do you know that without knowing the original concentration of the acids? I'm still totally lost
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Start by finding out what is getting neutralized at each inflection point (hint: depends on pKa values).
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Ok, will try. Thanks