Given that sodium acetate is a salt and is highly soluble in water, I am wondering how will the change in the pH of the media affect the solubility of the salt.
My postulation is as such:
CH3COONa ----> CH3COO- + Na+ (fully dissociated)
CH3COO- + H2O <---> CH3COOH + OH- (equilibrium)
Hence, in low pH condition, H+ will increase and hence scavenge OH-. The equilibrium for the second equation will be shifted to the right and hence forming more acetic acid (uncharged) and decreasing the solubility of the salt.
In the case for Aniline Hydrochloride, it is a salt and is highly soluble in water. Hence the equations can be written as such:
ArNH2.HCl ---> ArNH3+ + Cl- (fully dissociated)
ArNH3+ + H2O <---> ArNH2 + H3O+ (equilibrium)
Hence, in low pH condition, H+ will increase. The equilibrium for the second equation will be shifted to the left and hence forming more aniline cation (soluble species) and increasing the solubility of the salt.
Many of my colleagues have answers that contradict mine, so I'm wondering if the above explanation is correct.