1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

# On adding 0.1 M solution each of [Ag+], [Ba+2], [Ca+2] in a Na2SO4, solution, species first precipitated is: [Ksp, BaSO4=10−11 M, Ksp CaSO4=10−6, Ksp Ag2SO4=10−5]

A
Ag2SO4
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
BaSO4
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
CaSO4
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
all of these
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

## The correct option is B BaSO4 For Ag2SO4; Ksp=[Ag+]2 [SO2−4] ∴ [SO2−4] needed for precipitation of Ag2SO4>Ksp[Ag+]2 = 10−501.×0.1=10−3 M For BaSO4:Ksp=[Ba2+] [SO2−4] SO2−4 needed for precipitation of BaSO4>Ksp[Ba2+] = 10−110.1=10−10M For CaSO4; Ksp=[Ca2+] [SO2−4] ∴ [SO2−4] needed for precipitation of CaSO4>Ksp[Ca2+]=10−60.1=10−5M Thus, minimum [SO2−4] is required for precipitation of BaSO4 and hence it is precipitated out first.

Suggest Corrections
7
Join BYJU'S Learning Program
Related Videos
Introduction to Limits
MATHEMATICS
Watch in App
Explore more
Join BYJU'S Learning Program