Introductory Chemistry (5th Edition)

Published by Pearson
ISBN 10: 032191029X
ISBN 13: 978-0-32191-029-5

Chapter 15 - Chemical Equilibrium - Exercises - Problems - Page 569: 87

Answer

The molar solubility of $MgCO_3$ in pure water is equal to $2.61 \times 10^{-3}M$.

Work Step by Step

1. Write the $K_{sp}$ expression: $ MgCO_3(s) \lt -- \gt 1Mg^{2+}(aq) + 1CO_3^{2-}(aq)$ $6.82 \times 10^{-6} = [Mg^{2+}]^ 1[CO_3^{2-}]^ 1$ 2. Considering a pure solution: $[Mg^{2+}] = 1S$ and $[CO_3^{2-}] = 1S$ $6.82 \times 10^{-6}= ( 1S)^ 1 \times ( 1S)^ 1$ $6.82 \times 10^{-6} = S^ 2$ $ \sqrt [ 2] {6.82 \times 10^{-6}} = S$ $2.61 \times 10^{-3} = S$ - This is the molar solubility value for this salt.
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