Which among the following is colored?

$\mathrm{CuCl}$ has the copper in $+1$ oxidation state. It has the ten electrons in d-orbital. All the electrons are paired. So, it is not coloured. 

${\mathrm{ScCl}}_3$ has the ${\mathrm{Sc}}^{3+}$. It has the ${\mathrm{d}}^0$ configuration. It has all paired electrons. So, it has no colour.

${\mathrm{CuCl}}_2$ has the ${\mathrm{Cu}}^{2+}$. It has the ${\mathrm{d}}^9$ configuration. So, it has the unpaired electron. So, it can show the colour due to $\mathrm{d}-\mathrm{d}$ transition by the unpaired electron. So, it is coloured compound.

${\mathrm{TiCl}}_4$ has the ${\mathrm{Ti}}^{4+}$. It has the ${\mathrm{d}}^0$ configuration. It has all paired electrons. So, it has no colour.

Hence, the ${\mathrm{CuCl}}_2$ is coloured.