wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Find the minimum concentration of Pb2+ ions that will initiate the precipitation of PbSO4 from a solution containing 0.005 mol L1 of SO24 ions?
(Given Ksp for BaSO4=1.8×108 )

A
3.6×106 mol L1
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
4.5×105 mol L1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
0.9×104 mol L1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
2.7×109 mol L1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A 3.6×106 mol L1
If ionic product [Pb2+][SO24] is greater than Ksp for PbSO4, then the precipitation of PbSO4 will start.
So,
Qsp>Ksp

[Pb2+][SO24]>1.8×108
For the limiting case, i.e. when precipitation just starts
[Pb2+][SO24]=1.8×108
[Pb2+]×(0.005)=1.8×108
[Pb2+]=3.6×106 mol L1
Thus, minimum concentration of Pb2+ ions required for the precipitation of PbSO4 is 3.6×106 M.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
Join BYJU'S Learning Program
CrossIcon