?Consider the reaction\(\mathrm{CaSO}_{4}(s) \rightleftharpoons \mathrm{Ca}^{2+}(a
Chapter 15, Problem 15.55(choose chapter or problem)
Consider the reaction
\(\mathrm{CaSO}_{4}(s) \rightleftharpoons \mathrm{Ca}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)\)
At \(25^{\circ} \mathrm{C}\), the equilibrium constant is \(K_{c}=2.4 \times 10^{-5}\) for this reaction.
(a) If excess \(\mathrm{CaSO}_{4}(s)\) is mixed with water at \(25^{\circ} \mathrm{C}\) to produce a saturated solution of \(\mathrm{CaSO}_{4}\), what are the equilibrium concentrations of \(\mathrm{Ca}^{2+}\) and \(\mathrm{SO}_{4}^{2-}\) ?
(b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of \(\mathrm{CaSO}_{4}(s)\) needed to achieve equilibrium?
Text Transcription:
CaSO_4(s) \rightleftharpoons Ca^2+(a q)+SO_4^2-(a q)
25^circ C
K_c=2.4 \times 10^-5
CaSO_4(s)
Ca^2+
SO_4^2-
CaSO_4(s)
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