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If S(1), S2, S3 and S4 are the solubilit...

If `S_(1), S_2, S_3 and S_4` are the solubilities of AgCl in water, in 0.01 M `CaCl_2,` in 0.01 M NaCl and in 0.05 M `AgNO_3` respectively at a certain temperature, the correct order of solubilities is

A

`S_(1) gt S_(2) gt S_(3) gt S_(4)`

B

`S_(1) gt S_(3) gt S_(2) gt S_(4)`

C

`S_(1) gt S_(2)=S_(3) gt S_(4)`

D

`S_(1) gt S_(3) gt S_(4) gt S_(2)`

Text Solution

Verified by Experts

The correct Answer is:
B
0.01 M `CaCl_2 =0.02 M Cl^(-)`
0.01 M NaCl=0.01 `M Cl^(-)`
0.05 M `AgNO_3=0.05 M Ag^+`
`[Ag^+] [Cl^(-)]=K_(sp) ("const")`
Hence, `S_(2)=K_(sp)/(0.02) =50 K_(sp), S_(3)=(K_(sp))/(0.01)=100 K_(sp)`
`S_(4)=(K_(sp))/(0.05)=20 K_(sp), (S_(1)=sqrt(K_(sp)) ="maximuim")`
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