Equilibria involving physical processes; equilibrium in chemical processes; law of chemical equilibrium; equilibrium constants Kp and Kc; Le Chatelier's principle; ionic equilibrium — Bronsted-Lowry and Lewis acids/bases; ionisation of weak acids and bases; pH; common ion effect; buffer solutions; solubility product; hydrolysis of salts.
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Q1 · Equilibrium · EASY
For the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), the equilibrium constant Kc is 0.5 at a certain temperature. What is the value of Kc for the reverse reaction 2NH3(g) ⇌ N2(g) + 3H2(g) at the same temperature?
Q2 · Equilibrium · MEDIUM
A buffer solution contains 0.1 M acetic acid (CH3COOH) and 0.1 M sodium acetate (CH3COONa). If the Ka of acetic acid is 1.8 × 10^-5, what is the pH of this buffer solution?
Q3 · Equilibrium · MEDIUM
According to Le Chatelier's principle, what will happen to the equilibrium position of the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) (ΔH = -198 kJ/mol) when the temperature is increased?
Q4 · Equilibrium · MEDIUM
The solubility product (Ksp) of silver chloride (AgCl) is 1.8 × 10^-10 at 25°C. What is the molar solubility of AgCl in pure water at this temperature?
Q5 · Equilibrium · HARD
For the gaseous equilibrium PCl5(g) ⇌ PCl3(g) + Cl2(g), Kp = 1.8 at 250°C. If the partial pressures at equilibrium are: P(PCl3) = 0.6 atm and P(Cl2) = 0.6 atm, what is the partial pressure of PCl5 at equilibrium?