How would you use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.17 M in HCHO_2 and 0.10 M in NaCHO2?

Answer 1

#pH=3.51#

In order to use the Henderson-Hasselbalch equation, you will need the acid dissociation constant #K_a# of formic acid, which is #K_a=1.8xx10^(-4)#.

Therefore, Henderson-Hasselbalch equation is written as:

#pH=pK_a+log(([NaCHO_2])/([HCHO_2]))#

#=>pH=3.74+log((0.10cancel(M))/(0.17cancel(M)))#

#=>pH=3.51#

Here is a video that explains buffer solution and the Henderson-Hasselbalch equation and it is origin and use.
Acid - Base Equilibria | Buffer Solution.

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Answer 2

Peyton Adams

pH = pKa + log([A^-]/[HA])

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.