# Why is the esterification reaction of formic acid and isopropyl alcohol hard to do?

${\left({H}_{3} C\right)}_{2} C H O H + H C \left(= O\right) O H \stackrel{{H}^{+} , \Delta}{\rightarrow} {\left({H}_{3} C\right)}_{2} C H O \left(O =\right) C H$
The product has a normal boiling point of $68.2$ ""^@C, whereas formic acid has a normal boiling point of $100.2$ ""^@C. The other starting material, isopropyl alcohol, has a normal boiling point of $82.6$ ""^@C. There should be little difficulty in purifying the ester by distillation as the volatile fraction....