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

A solution has 0.1 M in each KCl, KBr and K2CrO4 and to this solution solid AgNO3 is gradually added. Assume there is no change in the volume of the solution given:
Ksp(AgCl)=1.7×1010
Ksp(AgBr)=5.0×1013 and Ksp(K2CrO4)=1.9×1012
The concentration of first ion when the second ion starts precipitating is about:

A
0.1M
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
0.03M
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
0.003M
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
0.0003M
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
Solution

The correct option is D 0.0003M
[Ag+] to start the ppt. Of Cl
=Ksp(AgCl)[Cl]=1.7×10100.1=1.7×109 M
When Cl starts precipitating
[Br]=Ksp(AgBr)[Ag+]=5×10131.7×109=3×104 M

flag
Suggest Corrections
thumbs-up
0
similar_icon
Similar questions
View More
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Synthesis of Alkyl Halides
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon