Question
Calculate the percentages of neutral and protonated forms present in a solution of $0.0010 \mathrm{M}$ pyrimidine at $\mathrm{pH}=7.3 .$ The $\mathrm{p} K_{\mathrm{a}}$ of pyrimidinium ion is 1.3 .
Step 1
The Henderson-Hasselbalch equation is given by: pH = pKa + log ([A-]/[HA]) where pH is the pH of the solution, pKa is the acid dissociation constant, [A-] is the concentration of the deprotonated form (neutral form in this case), and [HA] is the concentration Show more…
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