The number of `S^(2-)` ions present in `1 L` of `0.1 (M) H_(2)S` solution having `[H^(+)]=0.1 (M)` is
( Given `H_(2)ShArr2H^(+)+S^(2-) K_(a)=1.1xx10^(-21)`)

The number of S^(2-) ions present in 1L of 0.1 MH_(2)S [K_(a(H_(2)S)) = 10^(-21)] solution having [H^(o+)] = 0.1M is:

The number of S^(2-) ions present in 1L of 0.1 MH_(2)S [K_(a(H_(2)S)) = 10^(-21)] solution having [H^(o+)] = 0.1M is:

What is the pH of 0.01M H_(2)S solution ? Also determine [HS^(-)] & [S^(2-)] Given: For H_(2)S ,K_(a_(1))=9xx10^(-8),K_(a_(2))=1.2xx10^(-13)

What are the concentration of H_(3)O^(+) , HS^(+) and S^(2-) in 0..01 M H_(2)S solution , given {:(H_(2)S,+,H_(2)O,hArr,H_(3)O^(+),+,HS^(-),K_(at),=1.1 xx10^(-7),),(HS,+,H_(2)O,hArr,H_(3)O^(+),+,S^(2),K_(at),=1.0xx10^(-14),):} .

The K_(sp) of FeS = 4 xx 10^(-19) at 298 K. The minimum concentration of H^(+) ions required to prevent the precipitation of FeS from a 0.01 M solution Fe^(2+) salt by passing H_(2)S(0.1M) (Given H_(2)S k_(a_1) xx k_(b_1) = 10^(-21) )

The K_(sp) of FeS = 4 xx 10^(-19) at 298 K. The minimum concentration of H^(+) ions required to prevent the precipitation of FeS from a 0.01 M solution Fe^(2+) salt by passing H_(2)S(0.1M) (Given H_(2)S k_(a_1) xx k_(b_1) = 10^(-21) )

Approximate pH of 0.01M aqueous H_(2)S solution, when K_(1) and K_(2) for H_(2)S at 25^(@)C are 1xx10^(-7) and 1.3xx10^(-13) respectively: