Chemistry Why Should the Mole Ratio in Alkaline Buffers Be 5:1 Base to Acid?

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The discussion centers on the mole ratio of base to acid in alkaline buffers, specifically questioning why it should be 5:1. The initial confusion arises from the assumption that the amount of acid should be half that of the base, which is not the case. Clarification is provided that the focus should be on bisulfate rather than sulfuric acid, but the participant still struggles with the calculations. The importance of understanding reaction stoichiometry and the amounts of substances involved is emphasized as crucial to resolving the confusion. Ultimately, the correct interpretation of the mole ratio is essential for forming an effective alkaline buffer.
stunner5000pt
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Homework Statement
Which combination will produce an alkaline buffer

a. 0.1 mol ammonia & 0.05 mol sulfuric acid
b. 0.5 mol ammonia & 0.10 mol sulfuric acid
c. 0.1 mol acetic acid & 0.05 mol NaOH
d. 0.1 mol acetic acid & 0.50 mol NaOH
Relevant Equations
Henderson Hasselbach equation
THe answer is supposed to be (B) but I'm not understanding properly

I initially chose A - to form an alkaline buffer, the # mol of acid should be half of this. But this doesn't seem to be the case

I don't understand why the mol of base in this case should be 5x the mole of acid

your help is greatly appreciated, as always!
 
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Hint: sulfuric acid is diprotic.
 
Ok that does help - so we should be looking at bisulfate rather than sulfuric acid
but wouldn't the concentration of bisulfate be the same i.e. the second part of the henderson hasselbach would still be

for a. log (0.05/0.1) = log(0.5)

and for
b. log(0.1/0.5) = log(0.2)

I feel like i'm missing something obvious ....
 
stunner5000pt said:
a. 0.1 mol ammonia & 0.05 mol sulfuric acid

stunner5000pt said:
bisulfate

Nope, not bisulfate. Just look at the reaction stoichiometry and amounts of substances involved.
 
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