Topic: pH of KPi buffer (Read 12023 times)

enahs · « **on:** October 02, 2008, 08:39:48 PM »

Ok, I had to calculate this today at work and thought it might make a good little question. It has been so long since I have done any serious pH calculations I am ashamed it took me longer then it should have

.

What is the final pH if you add 0.25μL of 1M Perchloric Acid to 0.75μL of a solution buffered to pH 7.4 with "50 mM Potassium Phosphate" buffer?

AWK · « **Reply #1 on:** October 03, 2008, 01:15:15 AM »

Hint
Stronger acid replaces the weaker

Borek · « **Reply #2 on:** October 03, 2008, 04:15:59 AM »

That, plus stoichiometry and Henderson-Hasselbalch.

AWK · « **Reply #3 on:** October 03, 2008, 04:42:07 AM »

This is an excess of HClO₄!

Borek · « **Reply #4 on:** October 03, 2008, 05:02:14 AM »

Yes, overlooked that.

Still, that will be obvious after stoichiometry step.

Topic: pH of KPi buffer (Read 12023 times)

enahs

pH of KPi buffer

AWK

Re: pH of KPi buffer

Borek

Re: pH of KPi buffer

AWK

Re: pH of KPi buffer

Borek

Re: pH of KPi buffer

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