Reaction Beaker
Status: Dissolved
Precipitate: 0.00 g
Ion Product Q vs Ksp
Q (Ion Product):
1.00e-10
Ksp (Solubility Product):
1.77e-10
Saturated
Particle View
Cations (M⁺)
Anions (X⁻)
Precipitate (MX)
Ion Concentrations
Reaction Equation
M⁺(aq) + X⁻(aq) ⇌ MX(s)
Precipitation Reaction Controls
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Ksp:
1.77e-10
Solubility:
1.33e-5 M
Formula:
AgCl
Solution 1 (Cation)
Solution 2 (Anion)
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Precipitation Equations
Dissociation Equilibrium:
MX(s) ⇌ M⁺(aq) + X⁻(aq)
Solubility Product:
Ksp = [M⁺][X⁻]
Ion Product:
Q = [M⁺]₀ × [X⁻]₀
Precipitation Condition:
Q > Ksp → Precipitate forms
Equilibrium Condition:
Q = Ksp → Saturated solution
Molar Solubility from Ksp:
s = √Ksp (for MX type)
Common Ion Effect:
s = Ksp / [common ion]
What is Precipitation?
Precipitation is a chemical reaction where two soluble salts in solution combine to form an insoluble solid called a precipitate.
Solubility Product Constant (Ksp)
Ksp represents the maximum product of ion concentrations at equilibrium.
Ion Product (Q) and Precipitation Criteria
Q > Ksp: Precipitate forms. Q = Ksp: Saturated. Q < Ksp: Dissolved.
Common Precipitates
AgCl, BaSO₄, PbI₂, AgBr, CaCO₃, PbSO₄ with their Ksp values and properties.
Factors Affecting Precipitation
Concentration, temperature, pH, common ion effect, complex formation.
Applications
Qualitative analysis, gravimetric analysis, water treatment, wastewater treatment.
Kinetics vs Thermodynamics
Nucleation, crystal growth, supersaturation, particle size effects.