Which among the following has highest $\mathrm{pH}$ ?

For acidic medium, we know that $\mathrm{pH}$ values range is between $0-6.9$, for neutral it is 7 and for bases it is $7.1-14$. So, $\mathrm{HCl}$ is acidic and $\mathrm{NaOH}$ is basic. Thus, we can straight forward infer that $\mathrm{NaOH}$ has a higher $\mathrm{pH}$ value. Now, 1 mole of sodium hydroxide produces 1 mole of $\mathrm{Na}^{+}$and 1 mole of $\mathrm{OH}^{-}$ions. This means that the concentration of the hydroxide ions will be equal to $\left[\mathrm{OH}^{-}\right]=[\mathrm{NaOH}]=1 \mathrm{M}$ For case $\mathrm{A}$, $$ \begin{aligned} & \mathrm{pOH}=-\log \left[\mathrm{OH}^{-}\right]=-\log [1]=0 \\ & \therefore \quad \mathrm{pH}=14-\mathrm{pOH}=14-0=14 \\ & \text { For case } B \text {, } \\ & {\left[\mathrm{OH}^{-}\right]=[\mathrm{NaOH}]=0.1 \mathrm{M}} \\ & \text { pOH }=-\log [0.1]=1 \\ & \therefore \quad \mathrm{pH}=14-1=13 \\ & \end{aligned} $$ So, pH of $1 \mathrm{M} \mathrm{NaOH}$ is highest among the given solution.