Google Answers: pH of a buffer

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Q: pH of a buffer ( No Answer, 2 Comments )

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Subject: pH of a buffer
Category: Science > Chemistry
Asked by: stef44-ga
List Price: $2.00

Posted: 15 Mar 2004 13:11 PST
Expires: 14 Apr 2004 14:11 PDT
Question ID: 317009

What's the pH of a buffer solution of formic acid HCOOH: K3=1.8 x 10(on -4)
[HCOO]=0.5 M and [HCOOH]=0.15 M?
 Note: Henderson-Hasselback Equation is: pH=pK3 + log[A]/[HA]

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Comments

Subject: Re: pH of a buffer
From: stantheman-ga on 16 Mar 2004 16:34 PST

HCOO  =   0.5
HCOOH =   0.15
K3    =   1.8 x 10e(-4)
pK3   =  -log(K3) = 3.745

log(HCOO/HCOOH) = log(.5)/.15) = 0.523

pH    =   pK3 + log(HCOO/HCOOH) = 3.745 + 0.523 + 4.268

Subject: Re: pH of a buffer
From: stef44-ga on 16 Mar 2004 20:45 PST

thanks a lot for the answer.
i mistyped Ka and pKa: K3 was suppose to be Ka and pK3 was suppose to
be pKa. i see that you stuck with my 'acronyms' and went through
calcualtions anyway.
thanks again

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