Chemical and Ionic Equilibrium
Law of mass action; significance of ΔG and ΔG° in chemical equilibrium; Kp and Kc; reaction quotient; Le Chatelier's principle; solubility product; common ion effect; pH and buffer solutions; acids and bases (Bronsted and Lewis concepts); hydrolysis of salts.
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Take a full mock →Q1 · Chemical and Ionic Equilibrium · EASY
For the equilibrium N₂(g) + 3H₂(g) ⇌ 2NH₃(g), if Kₚ = 1.6 × 10⁻⁴ atm⁻² at 673 K, the value of Kc (in mol²/L²) is approximately: (R = 0.082 L·atm/K·mol)
Q2 · Chemical and Ionic Equilibrium · MEDIUM
The pH of a buffer solution containing 0.1 M CH₃COOH and 0.01 M CH₃COONa is: (pKₐ of CH₃COOH = 4.74)
Q3 · Chemical and Ionic Equilibrium · MEDIUM
At a certain temperature, Kₚ = 0.25 atm for the reaction N₂O₄(g) ⇌ 2NO₂(g). If the equilibrium partial pressure of NO₂ is 0.6 atm, what is the partial pressure of N₂O₄ at equilibrium (in atm)?
Q4 · Chemical and Ionic Equilibrium · EASY
For the reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g), if the equilibrium constant Kₚ at 500 K is 1.5 × 10⁻⁵ atm⁻², what is the relationship between Kₚ and Kc? (R = 0.082 L·atm·mol⁻¹·K⁻¹)