Why violet colour of [Ti(H2O)6]Cl3 disapear (colourless) on heating heating ?

[Ti(H₂O)₆]Cl₃ is an octahedral violet colour complex; the violet colour of this complex is due to d-d transition of a single (d¹) electron from t₂g lower level to eg higher level by absorbing corresponding energy of yellow green region of light and emitted energy corresponding to violet region and hence appears violet in colour. But on heating it is dehydrated and water molecules (ligand) removed so in absence of ligand splitting of D orbitals does not occur hence it becomes colourless.

Similarly  anhydrous CuSO₄ is white , but CuSO₄ .5H₂O is Blue in Colour.

Related Question:

Although both [Mn(H2O)6]2+ and [FeF6]3- have a d5 configuration and high-spin complexes. But the dilute solutions of Mn2+ and Fe +3 complexes are therefore colorless. Why?

Which of the Complex of the following pairs has the highest value of CFSE?
Colour of Complexes due to charge transfer:
Why violet colour of [Ti(H2O)6]Cl3 disapear (colourless) on heating heating ? 
Why [Ni(CN)4]-2 is colourless while [Ni(H2O)4]-2 although both have +2 oxidation state and 3d*8 configuration ?
Why [FeF6]3– is colourless whereas [CoF6]3– is coloured ? 
Why Fe(CO)5 is colourless while Fe(bipy)(CO)3 is intensely purple in colour ?
Why all the tetrahedral Complexes are high spin Complexes ?