Govt Exams
Qc = Kc indicates equilibrium. If Qc > Kc, reaction shifts backward; if Qc < Kc, reaction shifts forward.
According to the second law of thermodynamics, entropy of an isolated system increases or remains constant (ΔSuniverse ≥ 0).
Boiling point elevation depends only on the number of solute particles, not their identity, making it a colligative property.
Using Henry's Law: S = KH × P = 1.67 × 10⁻³ × 0.8 = 1.34 × 10⁻³ mol/L
The pH changes most steeply at the equivalence point in an acid-base titration because the buffer capacity is minimum at this point.
For AgCl ⇌ Ag⁺ + Cl⁻, Ksp = [Ag⁺][Cl⁻] = s × s = s². Therefore, s = √(1.8 × 10⁻¹⁰) = 1.34 × 10⁻⁵ M
Both larger atomic radius and greater shielding effect in sodium make the valence electron easier to remove compared to hydrogen's single electron.
Osmotic pressure: π = CRT where C is molar concentration. It's a colligative property dependent on number of solute particles.
Entropy is an extensive property (depends on amount of substance). Refractive index, surface tension, and density are intensive properties.
At constant temperature and pressure, ΔG < 0 is the criterion for spontaneity, where ΔG = ΔH - TΔS.