Consider the following electrochemical cell at standard condition. Au(s) | QH₂, Q ∥ NH₄X (0.01 M) ∥ Ag⁺ (1 M)…

Question

Consider the following electrochemical cell at standard condition.
$$ \mathrm{Au(s)} \mid \mathrm{QH_2}, \mathrm{Q} \parallel \mathrm{NH_4X}\,(0.01 \, 	ext{M}) \parallel \mathrm{Ag^+}\,(1 \, 	ext{M}) \mid \mathrm{Ag(s)}, \qquad E_{cell} = +0.4 \, 	ext{V} $$
The couple $$\mathrm{QH_2}/\mathrm{Q}$$ represents the quinhydrone electrode; the half cell reaction is given below.

The $$pK_b$$ value of the ammonium halide salt $$(\mathrm{NH_4X})$$ used here is _____ (nearest integer).

(Given: $$E^\circ_{\mathrm{Ag^+}/\mathrm{Ag}} = +0.8 \, 	ext{V}$$ and $$\frac{2.303RT}{F} = 0.06 \, 	ext{V}$$)

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