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Molar Solubility Formula:
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Molar solubility (S) is the maximum amount of a salt that can dissolve in a given amount of solvent at a specific temperature, expressed in moles per liter (mol/L). It is derived from the solubility product constant (K_sp) of the salt.
The calculator uses the molar solubility formula:
Where:
Explanation: For a salt with general formula AxBy, the stoichiometric factor ν = x + y, and the relationship between solubility and K_sp is given by K_sp = [A]x[B]y = (xS)x(yS)y.
Details: Molar solubility calculations are essential in chemistry for predicting precipitation reactions, designing chemical processes, understanding environmental behavior of compounds, and in pharmaceutical applications for drug formulation.
Tips: Enter K_sp value in mol²/L² and the stoichiometric factor ν (must be a positive integer). For example, for AgCl (ν=2), CaF₂ (ν=3), or Al(OH)₃ (ν=4).
Q1: What is the stoichiometric factor (ν)?
A: The stoichiometric factor is the sum of the coefficients in the balanced dissolution equation. For example, for Ag₂CrO₄ → 2Ag⁺ + CrO₄²⁻, ν = 2 + 1 = 3.
Q2: When is this formula applicable?
A: This simplified formula applies to salts where the cation and anion have a 1:1 ratio in the dissolution products. For complex salts, the relationship may be different.
Q3: What factors affect K_sp values?
A: K_sp is temperature-dependent and specific to each salt. It remains constant for a given salt at a constant temperature, regardless of the presence of other ions.
Q4: How does temperature affect solubility?
A: For most salts, solubility increases with temperature, but there are exceptions. The K_sp value changes with temperature accordingly.
Q5: What are common K_sp values for typical salts?
A: Common values range from 10⁻¹⁰ for very insoluble salts like AgCl to 10⁻² for more soluble salts. The calculator handles the full range of positive values.