The formation constant of  ${\left[{\text{Cu(NH}}_3{)}_4\right]}^{+2}$ is   $1.25\times {10}^{12}.$  When 0.0125 moles of copper is completely oxidised to +2 oxidation state and put into 1L of 0.25M ${\text{NH}}_{\text{3}}$  solution, the equilibrium concentration of the non-complexed cupric ion is found to be  $a.bc\times {\text{10}}^d$ (a point bc into ten raised to the power d).

Calculate the value of  $a+b+c+d$