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Chemistry · EQUILIBRIUM
हिन्दीThe ionization constant of a weak base \( \text{NH}_3 \) is \( 1.77 \times 10^{-5} \) at \( 298\text{ K} \). What is the ionization constant (\( K_a \)) of its conjugate acid \( \text{NH}_4^+ \)? (Given: \( K_w = 1.0 \times 10^{-14} \))
Correct answer · Option 3
\( 5.64 \times 10^{-10} \)
Explanation
For a conjugate acid-base pair, \( K_a \times K_b = K_w \). Therefore, \( K_a = \frac{1.0 \times 10^{-14}}{1.77 \times 10^{-5}} = 5.64 \times 10^{-10} \).
