Chapter 12, Problem 90AE

Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows:

${\text{CH}}_3\text{OH}\left(aq\right)\rightleftharpoons {\text{H}}_2\text{CO}\left(aq\right)+{\text{H}}_2\left(aq\right)$

Assuming the value of K for this reaction is 3.7 × 10⁻¹⁰, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?