The values of K_(sp) of two sparingly soluble salts, Ni(OH)_(2) and AgCN are 2.0xx10^(-15) and 6.0xx10^(-17), respectively. Which salt is more soluble ? Explain.

The values of K_(sp) of two sparingly soluble salts, Ni(OH)_(2) and Ag

1.	The values of K_(sp) of two sparingly soluble salts, Ni(OH)_(2) and AgCN are 2.0xx10^(-15) and 6.0xx10^(-17), respectively. Which salt is more soluble ? Explain.
Answer» Solution :`{:(NI(OH)_(2),hArr,Ni^(2+),+,2OH^(-),,,),(s,,s,,2s,,,):}` `K_(SP) = s (2s)^(2) = 4 s^(3 ) = 2.0 xx 10^(-15) `. This gives `s=5.8xx10^(-5)` mol `L^(-1)` `{:(AgCN,hArr,"Ag"^(+),+,CN^(-),,,),(s,,s,,s,,,):}` or `s=sqrt(K_(sp))=sqrt(6.0xx10^(-17))=7.8xx10^(-9) ` mol `L^(-1)`