$[Br^-] = [Cl^-] = [CO_3^{2-} ] = [AsO_4^{3-}] = 0.1\,M$.
Which compound will precipitate with lowest $[Ag^+]$ ?
$(2)$ $\left[\mathrm{Ag}^{+}\right]_{\text {required }}=1.8 \times 10^{-9}$
$(3)$ $\left[\mathrm{Ag}^{+}\right]_{\text {required }}=\sqrt{\frac{\mathrm{K}_{\mathrm{r}}}{\left[\mathrm{CO}_{3}^{2-}\right]}}=\sqrt{\frac{8.1 \times 10^{-12}}{0.1}}=9 \times 10^{-6}$
$(4)$ $\left[\mathrm{Ag}^{+}\right]_{\text {required }}=\sqrt{\frac{\mathrm{K}_{\mathrm{r}_{2}}}{\left[\mathrm{AsO}_{4}^{3-}\right]}}=3 \sqrt{\frac{1 \times 10^{-12}}{0.1}}=10^{-7}$
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$(A)\, F^-, Na^+, Mg^{+2}$ $(B) \,Ni, Cu, Zn$
$(C)\, N^{-3}, Cs^+, H^-$ $(D)\, Li, He, Be^{+2}$
| column $I$ | column $II$ |
| $(A)$ $CO _2( s ) \rightarrow CO _2( g )$ | $(p)$ phase transition |
| $(B)$ $CaCO _3( s ) \rightarrow CaO$ (s) $+ CO _2( g )$ | $(q)$ allotropic change |
| $(C)$ $2 H \bullet \rightarrow H _2( g )$ | $(r)$ $\Delta H$ is positive |
| $(D)$ $P_{\text {(white, solid) }} \rightarrow P_{\text {(red, solid) }}$ | $(s)$ $\Delta S$ is positive |
| $(t)$ $\Delta S$ is negative |
