# Barbituric Acid dissociation constant

1. Nov 18, 2014

1. The problem statement, all variables and given/known data
Barbituric acid is a single proton organic acid. Assume it is called "HA". Results show pH 4.22 in a solution of 0.020mol/dm3 of barbituric acid and 0.030mol/dm3 for sodium barbiturate, NaA. Calculate the "acid dissociation constant" for barbituric acid.

2. Relevant equations

3. The attempt at a solution
How do I even start? Through the pH I can calculate number of protons (H3O+) but I don't know where to go from here, since they've added "sodium barbiturate" into the whole equation. Would have been easy (I think) if it was just:

HA + H2O ⇔ A- + H30+

But now there is some sodium barbituric acid, where does the sodium come from? Would appreciate help.

2. Nov 18, 2014

### Staff: Mentor

You can safely assume concentrations of HA and A- to be these given (in other words: once you put the acid and its salt into solution, their concentrations don't change by much due to dissociation; this is obvious if you know how buffers work).