## Introductory Chemistry (5th Edition)

(a) $NaC_2H_3O_2$ is soluble. The ions are: $Na^+$ and $C_2H_3O_2^-$. (b) $Sn(NO_3)_2$ is soluble: The ions are: $Sn^{2+}$ and $NO_3^-$. (c) $AgI$ is insoluble. (d) $Na_3PO_4$ is soluble: The ions are $Na^+$ and $PO_4^{3-}$
Use the information in table 7.2 (Page 217), to predict the solubility of these compounds: (a) $NaC_2H_3O_2$: Compounds with $Na^+$ are soluble. The ions are: $Na^+$ and $C_2H_3O_2^-$. (b) $Sn(NO_3)_2$: Compounds with $NO_3^-$ are soluble: The ions are: $Sn^{2+}$ and $NO_3^-$. (c) $AgI$: Compound with halides, like $I^-$, are most of the time soluble. But, the ones with $Ag^+$ are an exception, so this compound is insoluble. (d) $Na_3PO_4$: Compounds with $Na^+$ are soluble: The ions are $Na^+$ and $PO_4^{3-}$