In $AgN{O_3},\;Ag$ is in $+1$ oxidation state.
In $CuS{O_4},\;Cu$ is in $ +2 $ oxidation state.
Equivalent weight of $Ag =\frac{{108}}{1} = 108$
Equivalent weight of $Cu = \frac{{63.6}}{2} = 31.8$
$\frac{{{M_1}}}{{{M_2}}} = \frac{{{E_1}}}{{{E_2}}}$ ; $\frac{{10.79}}{{{M_{Cu}}}} = \frac{{108}}{{31.8}}$
${M_{Cu}} = \frac{{10.79 \times 31.8}}{{108}} = 3.2\;gm$.
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Statement $I$: $\mathrm{PF}_5$ and $\mathrm{BrF}_5$ both exhibit $\mathrm{sp}^3 \mathrm{~d}$ hybridisation.
Statement $II$: Both $\mathrm{SF}_6$ and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ exhibit $\mathrm{sp}^3 \mathrm{~d}^2$ hybridisation.
In the light of the above statements, choose the correct answer from the options given below: