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The document discusses the solubility product constant (Ksp) and its applications in calculating molar solubility for various compounds, including lead carbonate, copper(I) iodide, silver sulfate, barium sulfate, and silver chloride. It provides examples of equilibrium expressions, Ksp calculations, and the conditions under which precipitates form when mixing solutions.

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How do you write the Ksp expression?

The equilibrium expression, Ksp, is a ratio of products over reactants and can be written as Ksp = [products]/[reactants]. This expression represents the equilibrium between an ionic solid and its ions in solution.

What is the equilibrium constant expression for the Ksp of Ca3 PO4 2?

Concentration Relationships in Saturated Solutions In a saturated solution, the concentrations of the ions are related through the Ksp expression. For Ca3(PO4)2, Ksp = [Ca2+]^3[PO43-]^2.

What is the Ksp at equilibrium?

The solubility product constant, Ksp, is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the level at which a solute dissolves in solution. The more soluble a substance is, the higher the Ksp value it has.

What is the formula for calculating Ksp?

10:30 41:51 And then times the phosphate ion concentration raised to the second power. So the concentration ofMoreAnd then times the phosphate ion concentration raised to the second power. So the concentration of calcium. Thats 4.932 times 10 to the negative seven.

How is solubility product written?

Since the equilibrium constant refers to the product of the concentration of the ions that are present in a saturated solution of an ionic compound, it is given the name solubility product constant, and given the symbol Ksp.

What is the expression for the solubility product constant?

So, the expression for the solubility product constant is: Ksp = [Cu2+]^3[PO4 3-]^2, because the coefficients of Cu2+ and PO4 3- are 3 and 2, respectively.

How do you write the solubility expression?

The solubility of a substance in a liquid may also be expressed as the quantity of solute per quantity of solution, rather than of solvent. For example, following the common practice in titration, it may be expressed as moles of solute per litre of solution (mol/L), the molarity of the latter.

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