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Molar Solubility Formula for 1:1 Salt:
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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 salts, the molar solubility can be directly calculated from the solubility product constant (K_sp).
The calculator uses the molar solubility formula for 1:1 salts:
Where:
Explanation: For a 1:1 salt like AgCl or BaSO₄ that dissociates into equal numbers of cations and anions, the molar solubility equals the square root of the solubility product constant.
Details: Calculating molar solubility is essential for predicting precipitation reactions, understanding solubility equilibria, and determining the maximum concentration of ions in solution before precipitation occurs.
Tips: Enter the solubility product constant (K_sp) value. The calculator will compute the molar solubility for a 1:1 salt. Ensure K_sp value is positive and valid.
Q1: What are 1:1 salts?
A: 1:1 salts are ionic compounds that dissociate into one cation and one anion per formula unit, such as AgCl, BaSO₄, or CaCO₃.
Q2: Does this formula work for all salts?
A: No, this simple square root relationship only applies to 1:1 salts. For other stoichiometries (like 1:2 or 2:3 salts), different formulas are needed.
Q3: What units should K_sp be in?
A: K_sp is typically unitless in calculations, but it represents equilibrium concentrations. Ensure your K_sp value matches the expected units for your system.
Q4: How does temperature affect solubility?
A: Temperature significantly affects both solubility and K_sp values. Most K_sp values are given at 25°C unless otherwise specified.
Q5: What if my salt has a different stoichiometry?
A: For salts with different cation:anion ratios (like Ag₂CrO₄ or Ca₃(PO₄)₂), you'll need to use different solubility product relationships based on the dissociation equilibrium.