10.6 g of a substance of molecular weight 106 was dissolved in 100 ml 10 ml of this solution was pipetted out into a 1000 ml flask and made up to the mark with distilled water. The molarity of the resulting solution is

Weight of the substance(W)=10.6g

Molecular weight of substance = 106 g

Volume of solution (V) = 100ml

$$\begin{gathered} \mathrm{M}=\frac{\mathrm{w}\times 1000}{\mathrm{M}\times \mathrm{V}\left(\mathrm{ml}\right)} \\ \mathrm{M}=\frac{10.6\times 1000}{106\times 100} \\ \mathrm{M} = 1\mathrm{M} \end{gathered}$$

When 10ml of this sol. is diluted to 1000ml,

$$\begin{gathered} {\mathrm{V}}_1{\mathrm{M}}_1={\mathrm{V}}_2{\mathrm{M}}_2 \\ 10\times 1=1000\times {\mathrm{M}}_2 \\ {\mathrm{M}}_2={10}^{-2}\mathrm{M} \end{gathered}$$

Hence, the correct answer (B).${10}^{-2}M$