I am struggling with the following problem: A reversible reaction where: CH3COOH + H2O--><--CH3COO- + H3O+ The overall solution initially has a CH3COOH concentration of 0.01mol/L and no acetate. The solution has 0.001mol/L of H3O+. Assume that this is constant throughout the experiment. K(equilibrium constant)=4.7*10^-4. Show that the equilibrium conversion is 32%.