Question
Oxidation number of $S$ in $N{a_2}S{O_4}$ is
$2 + x - 2 \times 4 = 0$
$x = + 6$.
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Given $\mathrm{R}=8.31\, \mathrm{~J} \,\mathrm{~K}^{-1} \,\mathrm{~mol}^{-1} ; \log 6.36 \times 10^{-3}=-2.19$ $\left.10^{-4.79}=1.62 \times 10^{-5}\right]$
(Atomic mass, $Ag =108, Br =80\, g\, mol ^{-1}$ )