Question

On the hydrolysis of esters according to the reaction: HCOO⁻(aq)+H₂O(l)⇌HCOOH(aq)+OH⁻(aq) To which the equilibrium will shift, if at a fixed temperature: a. Be deluted (water is added)? b. NaOH is added? c. Pressure is enlarged?

Answer 1

`HCOO^(-)(aq) + H_2O(l) rightleftharpoons HCOOH(aq) + OH^(-)(aq)`

If the solution is diluted, the reaction will shift left, because (i) water isn't in the equilibrium expression, and (ii) each product is in aqueous solution.

If `NaOH` is added, then we have increased the concentration of hydroxide ions. The reaction will shift left to re-equilibrate and consume the excess `OH^-`.

Pressure will have no effect in this case because none of the reagents are gases.