$(a)\;-1\qquad(b)\;0\qquad(c)\;+1\qquad(d)\;+2$

Firstly, the overall (addition of all) oxidation state of a neutral compound must be zero. In $[Pt(NH3)3Cl]Cl,$ the central metal atom is the Platinum(Pt).

Hence (d) is the correct answer.

Elements like H, F, Cl, O, N have its usual oxidation state as +1,-1,-1,-2,-3 respectively.

If we plug these oxidation states into the compound, $[x+3*(-3+3)-1]+(-1)$ will be the case.

Because this compound is a neutral compound, oxidation state for $Pt (x)$ should be $+2$.

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