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Calculating Ksp for Ca3(PO4)2 at 25°C: Step-by-Step Guide
Chapter 16, Problem 93(choose chapter or problem)
Assuming that the solubility of \(C{a_3}{\left( {P{O_4}} \right)_2(s)}\) is \(1.6 \times {10^{ - 7}}\) mol/L at \(25^\circ C\), calculate the \({K_{SP}}\) for this salt. Ignore any potential reactions of the ions with water.
Questions & Answers
QUESTION:
Assuming that the solubility of \(C{a_3}{\left( {P{O_4}} \right)_2(s)}\) is \(1.6 \times {10^{ - 7}}\) mol/L at \(25^\circ C\), calculate the \({K_{SP}}\) for this salt. Ignore any potential reactions of the ions with water.
ANSWER:Step 1 of 3
Molar Solubility
A quantitative representation of the solubility of a salt is molar solubility. It represents the amount of salt (in moles per liter) that can be added to a solvent to generate a saturated solution.
A higher solubility value implies more salt dissolves to form the saturated solution, and salt is more soluble. Therefore, solubility values can be used to compare the solubility of different salts.
The solubility value can be used with the stoichiometric equation to determine the solubility product of a salt, which is a constant for the salt maintained at a constant temperature.
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Calculating Ksp for Ca3(PO4)2 at 25°C: Step-by-Step Guide
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Unravel the concepts of 'Molar Solubility' and 'Solubility Product' to gauge salt solubility. Explore how Calcium Phosphate dissociates in solutions and calculate its unique Ksp value.