Question

How does acetic acid dissociate with temperature? What is the chemical equation?

Please add explanation, chemistry is my weakest subjects

Answer 1

The acid-base equilibrium is....

`H_3C-CO_2H(aq) + H_2O rightleftharpoonsH_3C-CO_2^(-) + H_3O^+`

Explanation:

As written, the equilibrium lies to the left hand side, towards the reactant side. We would expect that if we raised the temperature, i.e. pumped in heat, the equilibrium would shift to the right, to the product side, in that we supply energy to BREAK the strong(ish) hydrogen-oxygen bond....

At room temperature, `K_a=1.76xx10^-5`, which is fairly low....and most of the acetic acid would be undissociated.....

I would normally insist upon quoting units of `pK_a` at various temperatures, in order to demonstrate the change in aicid dissociation. Alas, I cannot find any.