Toluene $(C_7{H}_8)$ is a component of gasoline and it is contaminating a water body due to a leaky storage tank. The concentration in water of the toluene is $4\mathrm{.}25ppm.$ The starting pH of the water is $3\mathrm{.}0$ and this is a completely un$-$buffered system $($i$.$e$.$ protons that are liberated remain in solution and protons that are consumed are lost from solution during the RXNs taking place$).Fe(OH{)}_3$ is present and will serve as an electron acceptor for toluene oxidation; it is reduced to $F{e}^{2+}.$ Toluene is oxidized to $3$mol acetate $(C_2{H}_3{O}_2^{-})$and $1molC{O}_2.$

The acetate produced intracellularly $($this is a microbial RXN$)$ is released to external medium.

My question $$ given an equilibrium constant $(K_{eq})$ for acetic acid$/$acetate of $1\mathrm{.}99{10}^{-5}$ will the acetate remain as acetate or will it become protonated to form acetic acid?

You can assume:

The microbial reaction is not inhibited by low starting $pH$

Enough $Fe(OH{)}_3$ is present for this $RxN$ to take place

You will need:

A periodic table of the elements