512 marks

Equilibrium

This chapter covers chemical and ionic equilibrium, including equilibrium constants, Le Chatelier's principle, and acid-base equilibria.

24 Topics

50h prep

4% subject weight

24 Topics

Meaning of equilibrium

2m1/10

📌 Key FormulaState where rates of forward and reverse reactions are equal.

The concept of dynamic equilibrium

2m1/10

📌 Key FormulaMicroscopic activity, macroscopic constancy.

Equilibria involving physical processes

2m1/10

📌 Key FormulaPhase equilibrium.

Solid-liquid, liquid - gas and solid-gas equilibria

2m1/10

📌 Key FormulaMelting, vaporization, sublimation.

Henry's law

2m2/10

📌 Key FormulaPartial pressure of gas ∝ mole fraction in liquid.

General characteristics of equilibrium involving physical processes

2m1/10

📌 Key FormulaConstant at constant T.

Equilibrium involving chemical processes

2m1/10

📌 Key FormulaReversible reactions.

Law of chemical equilibrium

2m2/10

📌 Key FormulaK_c = [C]^c[D]^d / [A]^a[B]^b

Equilibrium constants (Kp and Kc) and their significance

2m3/10

📌 Key FormulaK_p = K_c (RT)^{Δn}

The significance of ΔG and ΔG^0 in chemical equilibrium

2m3/10

📌 Key FormulaΔG = ΔG° + RT ln Q, at equilibrium ΔG=0, ΔG° = -RT ln K

Factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst

2m2/10

📌 Key FormulaLe Chatelier's principle.

Le Chatelier’s principle

2m2/10

📌 Key FormulaEffect of change in conditions on equilibrium.

Ionic equilibrium

2m1/10

📌 Key FormulaEquilibrium involving ions.

Weak and strong electrolytes

2m1/10

📌 Key FormulaDegree of ionization.

Ionization of electrolytes

2m2/10

📌 Key FormulaOstwald's dilution law for weak electrolytes.

Various concepts of acids and bases and their ionization

Arrhenius. Bronsted - Lowry and Lewis

2m1/10

📌 Key FormulaDefinitions.

Acid-base equilibria (including multistage ionization) and ionization constants

2m2/10

📌 Key FormulaK_a, K_b, pK_a, pK_b

Ionization of water

2m1/10

📌 Key FormulaK_w = [H⁺][OH⁻] = 10⁻¹⁴ at 25°C

pH scale

2m2/10

📌 Key FormulapH = -log[H⁺], pOH = -log[OH⁻], pH + pOH = 14

Common ion effect

2m2/10

📌 Key FormulaSuppression of ionization of weak electrolyte by adding strong electrolyte with common ion.

Hydrolysis of salts and pH of their solutions

2m3/10

📌 Key FormulaSalts of weak acid/strong base, strong acid/weak base, weak acid/weak base.

The solubility of sparingly soluble salts

2m2/10

📌 Key FormulaS, K_sp relation.

Buffer solutions

2m3/10

📌 Key FormulaHenderson-Hasselbalch equation pH = pK_a + log([salt]/[acid])

Solubility products

2m3/10

📌 Key FormulaK_sp = [cation]^a[anion]^b for sparingly soluble salt.

512 marks

Equilibrium

This chapter covers chemical and ionic equilibrium, including equilibrium constants, Le Chatelier's principle, and acid-base equilibria.

24 Topics

50h prep

4% subject weight

24 Topics

Meaning of equilibrium

2m1/10

📌 Key FormulaState where rates of forward and reverse reactions are equal.

The concept of dynamic equilibrium

2m1/10

📌 Key FormulaMicroscopic activity, macroscopic constancy.

Equilibria involving physical processes

2m1/10

📌 Key FormulaPhase equilibrium.

Solid-liquid, liquid - gas and solid-gas equilibria

2m1/10

📌 Key FormulaMelting, vaporization, sublimation.

Henry's law

2m2/10

📌 Key FormulaPartial pressure of gas ∝ mole fraction in liquid.

General characteristics of equilibrium involving physical processes

2m1/10

📌 Key FormulaConstant at constant T.

Equilibrium involving chemical processes

2m1/10

📌 Key FormulaReversible reactions.

Law of chemical equilibrium

2m2/10

📌 Key FormulaK_c = [C]^c[D]^d / [A]^a[B]^b

Equilibrium constants (Kp and Kc) and their significance

2m3/10

📌 Key FormulaK_p = K_c (RT)^{Δn}

The significance of ΔG and ΔG^0 in chemical equilibrium

2m3/10

📌 Key FormulaΔG = ΔG° + RT ln Q, at equilibrium ΔG=0, ΔG° = -RT ln K

Factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst

2m2/10

📌 Key FormulaLe Chatelier's principle.

Le Chatelier’s principle

2m2/10

📌 Key FormulaEffect of change in conditions on equilibrium.

Ionic equilibrium

2m1/10

📌 Key FormulaEquilibrium involving ions.

Weak and strong electrolytes

2m1/10

📌 Key FormulaDegree of ionization.

Ionization of electrolytes

2m2/10

📌 Key FormulaOstwald's dilution law for weak electrolytes.

Various concepts of acids and bases and their ionization

Arrhenius. Bronsted - Lowry and Lewis

2m1/10

📌 Key FormulaDefinitions.

Acid-base equilibria (including multistage ionization) and ionization constants

2m2/10

📌 Key FormulaK_a, K_b, pK_a, pK_b

Ionization of water

2m1/10

📌 Key FormulaK_w = [H⁺][OH⁻] = 10⁻¹⁴ at 25°C

pH scale

2m2/10

📌 Key FormulapH = -log[H⁺], pOH = -log[OH⁻], pH + pOH = 14

Common ion effect

2m2/10

📌 Key FormulaSuppression of ionization of weak electrolyte by adding strong electrolyte with common ion.

Hydrolysis of salts and pH of their solutions

2m3/10

📌 Key FormulaSalts of weak acid/strong base, strong acid/weak base, weak acid/weak base.

The solubility of sparingly soluble salts

2m2/10

📌 Key FormulaS, K_sp relation.

Buffer solutions

2m3/10

📌 Key FormulaHenderson-Hasselbalch equation pH = pK_a + log([salt]/[acid])

Solubility products

2m3/10

📌 Key FormulaK_sp = [cation]^a[anion]^b for sparingly soluble salt.