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14 Φεβ 2024 · The equilibrium constant for the dissolution of a sparingly soluble salt is the solubility product (K sp) of the salt. Because the concentration of a pure solid such as Ca 3 (PO 4 ) 2 is a constant, it does not appear explicitly in the equilibrium constant expression.
- Solubility Product Constant, Ksp
The solubility product constant, Ksp , is the equilibrium...
- Solubility Product Constant, Ksp
30 Ιαν 2023 · 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.
The solubility product constant, or K sp, is the equilibrium constant of a solute dissolving in a solvent to form a solution. A solute is soluble if more than 1 g dissolves in 100 mL of water. The solubility product constant is generally used for a sparingly soluble solute that does not entirely dissolve.
The solubility expression is K s p = [A b +] a [B a −] b. The first equation is known as a dissociation equation, and the second is the balanced K s p expression. For these equations: A and B represent different ions and solids. In these equations, they are also referred to as "products".
In general, the solubility product of a compound represents the product of molar concentrations of ions raised to the power of their respective stoichiometric coefficients in the equilibrium reaction. Here's an example to better demonstrate the concept.
8 Απρ 2019 · With the solubility product expression, we can calculate the solubility of a sparingly soluble substance that ionizes completely in water. Example (1): What mass (in grams) of Ba (IO3)2 (487 g/mol) can be dissolved in 500 mL of water at 25 °C? Solution: – The solubility product constant for Ba (IO3)2 is 1.57 × 10-9 (see table above).
Ksp and Solubility. The Ksp of a slightly soluble ionic compound may be simply related to its measured solubility provided the dissolution process involves only dissociation and solvation, for example: MpXq(s) ⇌ pMm + (aq) + qXn − (aq) For cases such as these, one may derive Ksp values from provided solubilities, or vice-versa.
