Pyridine, C₅H₅N, is a weak base: C₅H₅N + H₂O ⇌ C₅H₅NH⁺ + OH⁻, with Kb = 1.6 × 10⁻⁹ at 298 K. What is the pH of a 0.25 mol L⁻¹ solution of pyridine at 298 K? Take Kw = 1.0 × 10⁻¹⁴ and log 2 = 0.301.

ChemistryMediumHigh School (11–12)Acids, Bases and Salts › Acids and Bases JEE Main

Pyridine, $\text{C}_5\text{H}_5\text{N}$ , is a weak base: $\text{C}_5\text{H}_5\text{N} + \text{H}_2\text{O} \rightleftharpoons \text{C}_5\text{H}_5\text{NH}^+ + \text{OH}^-$ , with $K_b = 1.6 \times 10^{-9}$ at $298\ \text{K}$ . What is the pH of a $0.25\ \text{mol L}^{-1}$ solution of pyridine at $298\ \text{K}$ ? Take $K_w = 1.0 \times 10^{-14}$ and $\log 2 = 0.301$ .

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← At a certain temperature, Kc for 2 NO(g) + O₂(g) ⇌ 2 NO₂(g) is 1.6 × 10³, and Kc for 2 NO₂(g) ⇌ N₂O₄(g) is 4.0, both with concentrations in mol L⁻¹. What is the value of Kc at this temperature for NO(g) + 1/2 O₂(g) ⇌ 1/2 N₂O₄(g)?Baking soda breaks down when heated: 2 NaHCO₃(s) ⇌ Na₂CO₃(s) + CO₂(g) + H₂O(g), and the forward change is endothermic. Some NaHCO₃ is heated in a closed vessel until equilibrium is reached, with all three solids or gases present. Which statement about this equilibrium is correct? →

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