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Molar Solubility Formula:
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Molar solubility refers to the maximum amount of a substance that can dissolve in a given amount of solvent at a specific temperature, expressed in moles per liter (mol/L). For 1:1 electrolytes, it can be calculated directly from the solubility product constant.
The calculator uses the molar solubility formula for 1:1 electrolytes:
Where:
Explanation: This formula applies specifically to 1:1 electrolytes where the dissolution reaction follows the pattern AB(s) ⇌ A⁺(aq) + B⁻(aq). The molar solubility equals the square root of the solubility product constant.
Details: Calculating molar solubility is essential in chemistry for predicting precipitation reactions, designing analytical methods, understanding solubility equilibria, and in pharmaceutical applications where drug solubility affects bioavailability.
Tips: Enter the solubility product constant (K_sp) value. The value must be positive and non-zero. The calculator will compute the molar solubility in moles per liter for 1:1 electrolytes.
Q1: What is a 1:1 electrolyte?
A: A 1:1 electrolyte is a compound that dissociates into one cation and one anion per formula unit, such as NaCl, AgCl, or CaSO₄.
Q2: Does this formula work for all electrolytes?
A: No, this specific formula (S = √K_sp) only applies to 1:1 electrolytes. Different stoichiometries require different formulas.
Q3: What are typical K_sp values?
A: K_sp values range from very small (10⁻³⁰ for very insoluble compounds) to larger values for more soluble compounds. Common values are in the range of 10⁻⁵ to 10⁻¹⁰.
Q4: How does temperature affect molar solubility?
A: Temperature significantly affects solubility. K_sp values are temperature-dependent, so calculations should use K_sp values at the specific temperature of interest.
Q5: What about electrolytes with different stoichiometries?
A: For AB₂ type electrolytes (like CaF₂), the formula is S = ∛(K_sp/4); for A₂B type, it's S = ∛(K_sp/4); and for AB₃ type, it's S = ⁴√(K_sp/27).