Equilibrium

A state where forward and reverse

A state where forward and reverse reactions occur at equal rates, maintaining constant concentrations of reactants and products. Examples include H2O(

For reaction aA + bB ⇌

For reaction aA + bB ⇌ cC + dD, Kc = [C]^c[D]^d/[A]^a[B]^b. For gaseous reactions, Kp uses partial pressures. Relationship: Kp = Kc(RT)^Δn where Δn =

When equilibrium is disturbed by changing

When equilibrium is disturbed by changing concentration, pressure, or temperature, the system adjusts to minimize the disturbance. Adding reactants sh

Arrhenius

Arrhenius: acids produce H⁺, bases produce OH⁻. Brönsted-Lowry: acids are proton donors, bases are proton acceptors. Lewis: acids accept electron pair

pH =

pH = -log[H⁺], pOH = -log[OH⁻], pH + pOH = 14 at 25°C. Kw = [H⁺][OH⁻] = 1×10⁻¹⁴. Acidic solutions: pH < 7, Basic solutions: pH > 7, Neutral: pH = 7.