$\mathrm{AgX}(\mathrm{s})+2\mathrm{NH}{}_3\rightleftharpoons [\mathrm{Ag}(\mathrm{NH}{}_3){}_2]{}^{+}+\mathrm{X}{}^{-}$. Given $K_f([\mathrm{Ag}(\mathrm{NH}{}_3){}_2{]}^{+})=1.6\times 10^7$; $K_{sp}$: $\mathrm{AgCl}=1.6\times 10^{-10}$, $\mathrm{AgBr}=5.0\times 10^{-13}$, $\mathrm{AgI}=8.5\times 10^{-17}$. Treat the free $[\mathrm{NH}{}_3]$ as constant at $1.0\mathrm{M}$. Select the correct statement(s).

1. A$0.010\mathrm{mol}$ of $\mathrm{AgCl}$ dissolves completely in $1.0\mathrm{L}$ of such ammonia
2. B$0.010\mathrm{mol}$ of $\mathrm{AgBr}$ dissolves completely in $1.0\mathrm{L}$ of such ammonia
3. CThe equilibrium constant for dissolution of $\mathrm{AgBr}$ in ammonia is $8\times 10^{-6}$
4. D$\mathrm{AgI}$ is more soluble than $\mathrm{AgBr}$ in ammonia because its $K_{sp}$ is smaller