Sparingly soluble salts maintains their solubilityproduct value in their saturated solutions irrespective of the sources of the ions .what is the molar solubility of AgNO_3in a 0.1 M H_2Ssolution buffered at pH= 2 (K_1 and K_2 "of "H_2S " are "10^(4) and 10^(-8)respectively)(K_(sp) " of "Ag_2S = 4xx 10^(-13) )(Note : No Ag_2Sprecipitate should be formed)

Sparingly soluble salts maintains their solubilityproduct value in the

1.	Sparingly soluble salts maintains their solubilityproduct value in their saturated solutions irrespective of the sources of the ions .what is the molar solubility of AgNO_3in a 0.1 M H_2Ssolution buffered at pH= 2 (K_1 and K_2 "of "H_2S " are "10^(4) and 10^(-8)respectively)(K_(sp) " of "Ag_2S = 4xx 10^(-13) )(Note : No Ag_2Sprecipitate should be formed)
Answer» ` 0.01 M` ` 0. 02 M` ` 0. 03 M` ` 0. 04 M` Solution :`PH= 2 , [H^(+) ] =10 ^(-2) M` ` K_a =([H^(+) ][S^(-2) ])/( [H_2S] ) rArr 10 ^(-12)=( 10 ^(-4) [S^(-2)])/( 10^(-1) ) ` ` [S^(-2) ]= 10 ^(-9)M` ` Ag_2S hArr 2Ag^(+) +S^(_2) ` ` K_(Sp)=[Ag^(+) ]^(2) [S^(-2) ], 4 xx10 ^(-13) =[Ag^(+) ]^(2) (10 ^(-9))` ` [Ag^(+) ]= 2xx 10 ^(-2) =0.02 M`