Calculate the ph of a solution containing 0.0451 m potassium hydrogen tartrate and 0.028 m dipotassium tartrate. The ka values for tartaric acid are 9.20 * 10-4 (ka1) and 4.31 * 10-5 (ka2).

Given buffer:

potassium hydrogen tartrate/dipotassium tartrate (KHC4H4O6/K2C4H4O6)

[KHC4H4O6] = 0.0451 M

[K2C4H4O6] = 0.028 M

Ka1 = 9.2 * 10^-4

Ka2 = 4.31*10^-5

Based on Henderson-Hasselbalch equation;

pH = pKa + log [conjugate base]/[acid]

where pka = - logKa

In this case we will use the ka corresponding to the deprotonation of the second proton i. e. ka2

pH = - log Ka2 + log [K2C4H4O6]/[KHC4H4O6]

= - log (4.31*10^-5) + log [0.0451]/[0.028]

pH = 4.15