The Redox changes during electrolysis of SnCl2 are:
Anode: 2Cl−→Cl2+2e
Cathode:Sn2++2e→Sn
Also Cl2 formed at anode reacts with SnCl2 to give SnCl4
SnCl2+2e→SnCl4
Now Eq. of SnCl2 lost during elecrolysis = Eq. of Cl2 formed during electrolysis=Eq. of Sn formed during electrolysis
=0.1190.119/2=2×10−3
∴ Eq. of SnCl4 formed = 2×10−3
Total loss in eq. of SnCl2 during complete course=Eq. of SnCl2 lost during electorlysis + Eq. of SnCl2 lost during reaction with Cl2
= 2×10−3+2×10−3=4×10−3
Initial eq. of SnCl2 =\frac { 19 }{ 190/2 } =2\times { 10 }^{ -1 }
∴ Eq.of SnCl2 left in solution
=2×10−1−4×10−3 =0.196.
Also Eq. of SnCl4 formed= 2×10−3=0.002
∴ =MassofSnCl2leftMassofSnCl4formed=0.196×(190/2)0.002×(261/2)=71.34
Hence, the ratio of mass of SnCl2 and SnCl4 in fused state after electrolysis is 71.34.