Chemistry: The Molecular Science (5th Edition)

The molar solubility of this compound in pure water is equal to: $3.7 \times 10^{-6}M$
1. Write the $K_{sp}$ expression: $ZnCO_3(s) \lt -- \gt 1Zn^{2+}(aq) + 1C{O_3}^{2-}(aq)$ $1.4 \times 10^{-11} = [Zn^{2+}]^ 1[C{O_3}^{2-}]^ 1$ 2. Considering a pure solution: $[Zn^{2+}] = 1x$ and $[C{O_3}^{2-}] = 1x$ $1.4 \times 10^{-11}= ( 1x)^ 1 \times ( 1x)^ 1$ $1.4 \times 10^{-11} = 1x^ 2$ $1.4 \times 10^{-11} = x^ 2$ $\sqrt [ 2] {1.4 \times 10^{-11}} = x$ $3.742 \times 10^{-6}M = x$ - This is the molar solubility value for this salt.