At 25°C only 0.0687 moles of LiCl is soluble in 1.00L of water. What is the Kap of the salt at this temperature? LICI (s) Li (aq) + Cl- (aq) Give your answer to 3 significant figures.
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![**Determining the Solubility Product Constant (Ksp) of LiCl at 25°C**
At a temperature of 25°C, it has been observed that 0.0687 moles of LiCl is soluble in 1.00 liter of water. The question posed is: What is the solubility product constant (Ksp) of LiCl at this particular temperature?
**Dissociation Equation:**
\[ \text{LiCl (s) } \rightleftharpoons \text{ Li}^+ \text{(aq) } + \text{ Cl}^- \text{(aq)} \]
**Directions:**
Calculate the Ksp value and provide your answer to three significant figures.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb375a3d6-a030-4649-bb27-4fd4f489b39e%2Ff3b745de-fad4-4af5-8eee-3f5437266376%2F0q2l63s_processed.jpeg&w=3840&q=75)
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