0.1 moles of Barium hydroxide is dissolved in a 50 ml solution. Normality of the solution is-----N

$$\begin{gathered} \mathrm{N}=\mathrm{Number} \mathrm{of} \mathrm{gram} \mathrm{equivalents}\times \frac{1}{\mathrm{V}\left(\mathrm{l}\right)}; \\ \mathrm{N}=\mathrm{Number} \mathrm{of} \mathrm{gram} \mathrm{equivalents}\times \frac{1000}{\mathrm{V}\left(\mathrm{ml}\right)}; \\ \mathrm{Number} \mathrm{of} \mathrm{gram} \mathrm{equivalents}=\frac{{\mathrm{w}}_{\mathrm{solute}}}{\mathrm{GEW} \mathrm{of} \mathrm{solute}}; \\ \mathrm{Number} \mathrm{of} \mathrm{gram} \mathrm{equivalents}=\mathrm{Number} \mathrm{of} \mathrm{moles}\times \mathrm{Valency}; \\ \mathrm{Ba}{\left(\mathrm{OH}\right)}_2 \mathrm{is} \mathrm{a} \mathrm{diacidic} \mathrm{base} ; \\ \mathrm{N}=0.1\times 2\times \frac{1000}{50}=4 \mathrm{N} ; \end{gathered}$$