If the value of K_b for pyridine is 1.8 *10^-⁹, calculate the equilibrium constant for C₅H₅NH⁺(aq)+ H₂O(l)$\Leftrightarrow$ C₅H₅N(aq)+ H₃O⁺(aq) A) -1.8 * 10^-⁹ B) 1.8 * 10^-¹⁶ C) 5.6 * 10⁸ D) 1.8 * 10^-⁹ E) 5.6 * 10^-⁶

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The Answer of If the value of K_b for pyridine is 1.8 *10^-⁹, calculate the equilibrium constant for C₅H₅NH⁺(aq)+ H₂O(l)$\Leftrightarrow$ C₅H₅N(aq)+ H₃O⁺(aq) A) -1.8 * 10^-⁹ B) 1.8 * 10^-¹⁶ C) 5.6 * 10⁸ D) 1.8 * 10^-⁹ E) 5.6 * 10^-⁶

If the Value of Kb for Pyridine Is 1 ⇔\Leftrightarrow⇔ C5H5N(aq)+ H3O+(aq) A) -1

If the Value of K_b for Pyridine Is 1 $\Leftrightarrow$ C₅H₅N(aq)+ H₃O⁺(aq)
A) -1