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

Assertion :Solubility of AgCl in NH3(aq.) is greater than in pure water. Reason: When AgCl dissolve in NH3(aq.), complex ion formation Ag(NH3)+2 takes place and solubility equilibria of AgCl shifted in forward direction.

A
Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
Assertion is correct but Reason is incorrect
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
Both Assertion and Reason are incorrect
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
Solubility of AgCl in NH3(aq.) is greater than in pure water because when AgCl dissolve in NH3(aq.) it will form complex ion with Ag+ and formation of Ag(NH3)+2 takes place and because of this solubility equilibria of AgCl shifted in forward direction and it dissolve more with respect to pure water.

Ag++2NH3(aq)[Ag(NH3)2]+

flag
Suggest Corrections
thumbs-up
0
similar_icon
Similar questions
View More
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Solubility and Solubility Product
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon