What is the color of the $[Ti(H_2O)_6]^{3+}$ complex?

Given below are two statements,one is labelled as Assertion $A$ and the other is labelled as Reason $R$.
Assertion $A$: $[CoCl(NH_3)_5]^{2+}$ absorbs at a lower wavelength of light with respect to $[Co(NH_3)_5(H_2O)]^{3+}$.
Reason $R$: It is because the wavelength of the light absorbed depends on the oxidation state of the metal ion.
In the light of the above statements,choose the correct answer from the options given below:

The number of unpaired $d$-electrons in $[Co(H_2O)_6]^{3+}$ is $\qquad$

The electronic configuration of a metal ion in its complex is $[Ar] 3d^4$. For this metal complex,$\Delta_o < P$ ($P=$ energy required for electron pairing in a single orbital). The distribution of electrons in the complex is:

Which of the following complex ions absorbs the light of minimum wavelength?

Using crystal field theory,draw energy level diagrams,write the electronic configuration of the central metal atom/ion,and determine the magnetic moment value for the following:
$(i)$ $[CoF_{6}]^{3-}, [Co(H_{2}O)_{6}]^{2+}, [Co(CN)_{6}]^{3-}$
$(ii)$ $[FeF_{6}]^{3-}, [Fe(H_{2}O)_{6}]^{2+}, [Fe(CN)_{6}]^{4-}$