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Q. 4.2

Write a net ionic equation for any precipitation reaction that occurs when dilute solutions of the following ionic compounds are mixed.

(a) NaOH and $Cu(NO_{3})_{2}$           (b) $Ba(OH)_{2}$ and $MgSO_{4}$           (c) $(NH_{4})_{3}PO_{4}$ and $K_{2}CO_{3}$

STRATEGY

 $Na^{+}$ and $OH^{-}$ from NaOH; $Cu^{2+}$ and $NO^{-}_{3}$ from  $Cu(NO_{3})_{2}$ $NaNO_{3}$ and $Cu(OH)_{2}$ $NaNO_{3}$ is soluble; $Cu(OH)_{2}$ is insoluble. $Cu^{2+}(aq)$ + 2$OH^{-}(aq)$ → $Cu(OH)_{2}(s)$. (a) Ions in solution Possible precipitates Solubility Net ionic equation $Ba^{2+}$ and $OH^{-}$ from $Ba(OH)_{2}$; $Mg^{2+}$ and $SO^{2-}_{4}$ from $MgSO_{4}$ $Mg(OH)_{2}$ and $BaSO_{4}$ Both $BaSO_{4}$ and $Mg(OH)_{2}$ are insoluble. $Mg^{2+}(aq)$ + $2OH^{-}(aq)$ → $Mg(OH)_{2}(s)$ $Ba^{2-}(aq)$ + $SO^{2-}_{4}(aq)$ → $BaSO_{4}(s)$ (b) Ions in solution Possible precipitates Solubility Net ionic equation $NH^{+}_{4}$ and $PO_{4}^{3-}$ from $(NH_{4})_{3}PO_{4}$; $K^{+}$ and $CO_{3}^{2-}$ from $K_{2}CO_{3}$ $(NH_{4})_{2}CO_{3}$ and $K_{3}PO_{4}$ Both $(NH_{4})_{2}CO_{3}$ and $K_{3}PO_{4}$ are soluble. no reaction (c) Ions in solution Possible precipitates Solubility Net ionic equation