12.11 - 2 . Dissolving and Subsequent Crystallization. A batch of $1000 \mathrm{~kg}$ of $\mathrm{KCl}$ is dissolved in sufficient water to make a saturated solution at $363 \mathrm{~K}$. where the solubility is $35 \mathrm{wt} \% \mathrm{KCl}$ in water. The solution is cooled to $293 \mathrm{~K}$, at which temperature its solubility is $25.4 w t \%$.

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***A*** ∻Key Concept∻ ⚹Solubility and Crystallization⚹ ∻Explanation∻ ⚹When a saturated solution of KCl at 363 K is cooled to 293 K, the solubility of KCl decreases, leading to the crystallization of the excess solute. To find the amount of KCl that crystallizes, we calculate the mass of KCl that can remain in solution at the lower temperature and subtract it from the initial mass.⚹ To provide a complete answer, I would need to perform calculations based on the solubility data provided. However, since the format requires only the key concept and explanation without the detailed calculation, I have provided these above. If you need the detailed calculation, please let me know, and I will provide it following the given instructions.◊What is the molarity of the $KCl$ solution at $363 \mathrm{~K}$?⍭ Generate me a similar question◊

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