CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

The concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0×1019M. If 10 mL of this is added to 5 mL of 0.04 M solution of the following:
FeSO4,MnCl2,ZnCl2 and CdCl2. in which of these solutions precipitation will take place?

Given KspforFeS=6.3×1018.MnS=2.5×1013.ZnS=1.6×1024.CdS=8.0×1027


Solution

For precipitation to take place, it is required that the calculated ionic product exceeds the Ksp value.
Before mixing: 
[S2]=1.0×1019M and [M2+]=0.04M
volume = 10 mL    volume = 5mL
After mixing: 
[S2]=?[M2+]=?volume=(10+5)=15mLVolume=15mL
[S2]=1.0×1019×1015=6.67×1020M[M2+]=0.04×515=1.33×102M
Ionic product =[M2+][S2]=(1.33×102)(6.67×1020)=8.87×1022
This ionic product exceeds the Ksp of Zns and CdS. Therefore, precipitation will occur in CdCl2 and ZnCl2 solutions. 


Chemistry
NCERT Textbook
Standard XI

Suggest Corrections
thumbs-up
 
0


similar_icon
Similar questions
View More


similar_icon
Same exercise questions
View More


similar_icon
People also searched for
View More



footer-image