Color of Pt(NH3)2Cl2
Pt(NH3)2Cl2 is a coordination complex consisting of a central platinum ion surrounded by two ammonia ligands and two chloride ions. The color of this complex compound depends on the electronic structure of the central metal ion and the ligands attached to it.

Electronic Structure
The color of coordination complexes is primarily due to the absorption of certain wavelengths of light by the complex. The d-orbitals of the central metal ion split into different energy levels in the presence of ligands, creating a series of d-d transitions that can absorb visible light.

Chloro ligands
In the case of Pt(NH3)2Cl2, the chloride ligands are weak field ligands, which lead to smaller energy differences between the d-orbitals. As a result, the absorption of light is shifted towards the UV region, making the complex appear colorless to the human eye.

Ammonia ligands
The ammonia ligands, on the other hand, are strong field ligands that cause a larger splitting of the d-orbitals. This can result in the absorption of certain wavelengths of light in the visible region, giving the complex a color. In the case of Pt(NH3)2Cl2, the color is typically pale yellow due to the presence of ammonia ligands.

Conclusion
In conclusion, Pt(NH3)2Cl2 is typically pale yellow in color due to the presence of ammonia ligands, which cause the absorption of certain wavelengths of light in the visible region. The weak field chloride ligands do not contribute significantly to the color of the complex.