Given the Following Equilibrium Constants, Zn4IO₃)₂ K_sp = $3.9 \times 10 - 6$

Given the following equilibrium constants, Zn4IO₃) ₂ K_sp = $3.9 \times 10 - 6$ Zn(NH₃) ₄²⁺ K_f = $2.9 \times 10 ^ { 9 }$ determine K for the dissolution of the sparingly soluble salt Zn(IO₃) ₂ in aqueous ammonia (shown below) .
Zn(IO₃) ₂(s) + 4NH₃(aq) ? Zn(NH₃) ₄²⁺(aq) + 2IO₃^-(aq)

A) $1.1 \times 10 ^ { 4 }$
B) $1.3 \times 10 ^ { - 15 }$
C) $7.4 \times 10 ^ { 14 }$
D) $8.8 \times 10 ^ { - 5 }$
E) $2.9 \times 10 ^ { 9 }$