My book(Page $259$ section $9.5.5$) says that the color mainly comes from absorption of light in the coordination compound:
The color is complementary of the wavelength it absorbs , the wavelength left over is the color of the complex.
But there are two instances of these coordination complexes: $\ce{[Co(NH3)5(H2O)]^{3+}}$ which absorbs blue green light of wavelength $\pu{500nm}$ which appears to be red in color and
$\ce{[Ti(H2O)6]^{3+}}$ which absorbs blue green light of wavelength $\pu{498nm}$ which appears to be violet in color.
Question: If a color of a complex is determined with what color it absorbs then why is it that two complex's have the same absorption region yet appear to be in different colours