In $1.0\mathrm{M}$ aqueous $\mathrm{NH}{}_3$ the silver halides dissolve as $\mathrm{AgX}(\mathrm{s})+2\mathrm{NH}{}_3\rightleftharpoons [\mathrm{Ag}(\mathrm{NH}{}_3){}_2]{}^{+}+\mathrm{X}{}^{-}$. Use $K_f([\mathrm{Ag}(\mathrm{NH}{}_3){}_2]{}^{+})=1.6\times 10^7$ and $K_{sp}$: $\mathrm{AgCl}$ $1.8\times 10^{-10}$, $\mathrm{AgBr}$ $5.0\times 10^{-13}$, $\mathrm{AgI}$ $8.5\times 10^{-17}$. Select the correct statement(s).

1. A$\mathrm{AgCl}$ dissolves in $1.0\mathrm{M}$ $\mathrm{NH}{}_3$ to more than $0.04\mathrm{M}$
2. B$\mathrm{AgBr}$ dissolves in $1.0\mathrm{M}$ $\mathrm{NH}{}_3$ to less than $1.0\times 10^{-3}\mathrm{M}$
3. C$\mathrm{AgI}$ dissolves in $1.0\mathrm{M}$ $\mathrm{NH}{}_3$ to less than $1.0\times 10^{-4}\mathrm{M}$
4. DThe solubility of $\mathrm{AgCl}$ in $1.0\mathrm{M}$ $\mathrm{NH}{}_3$ is about 17 times that of $\mathrm{AgBr}$