A saturated aqueous solution of at contains excess solid at the bottom of the flask

CHEMISTRY · Single correct · AP · Chemistry · Equilibrium · Equilibrium

Problem

A saturated aqueous solution of

\mathrm{AgCl}

25^{\circ}\text{C}

contains excess solid

\mathrm{AgCl(s)}

at the bottom of the flask. Pure water is added, doubling the total volume while temperature remains constant. Which statement most accurately predicts what happens to the system before the new equilibrium is reached? (a) Some

\mathrm{Ag^+}

and

\mathrm{Cl^-}

ions precipitate as

\mathrm{AgCl}

until the ionic product again equals

K_{sp}

, so the total amount of dissolved silver ions decreases. (b) More

\mathrm{AgCl}

dissolves until the ionic product again equals

K_{sp}

, so the total amount of dissolved silver ions increases. (c) After dilution the concentrations of

\mathrm{Ag^+}

and

\mathrm{Cl^-}

remain exactly one-half their original values because

K_{sp}

is unchanged. (d) The equilibrium constant

K_{sp}

becomes smaller upon dilution, so no additional solid dissolves.

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