A beaker contains small amounts of the sparingly soluble solids AgCl(s), Fe(OH) (s)
CHEMISTRY · Single correct · AP · Chemistry · Acids and Bases · Acids and Bases
Problem
A beaker contains small amounts of the sparingly soluble solids AgCl(s), Fe(OH)3(s), and CaF2(s). After the mixture is stirred with 1 M HCl until the solution reaches pH 1 and is then filtered, which solid is most likely to have completely dissolved, and why?
(a) CaF2, because added H+ converts F− to HF, shifting its dissolution equilibrium toward ions.
(b) Fe(OH)3, because added H+ reacts with OH−, shifting its dissolution equilibrium toward ions.
(c) AgCl, because Cl− from the acid forms soluble chloride complexes with Ag+.
(d) None of the solids dissolve appreciably because the Ksp values themselves are unaffected by pH.