Caculate solubility of MnS in a buffer solution of given pH. K sp of MnS and 
& 
for H 2 S are given.
Text Solution
Verified by ExpertsCHECK THE SOLUTION.
Let the new solubility of MnS = x
∴ [Mn 2+ ] = x = Initial concentration of S 2– ions, but free S 2– ions will be less because some of the S 2– ions will react with H + from buffer to form HS – and H 2 S.
[Mn 2+ ] = x = [S 2– ] + [HS – ] + [H 2 S] .....
free
Let us calculate the value of [HS – ] & [H 2 S], in terms of free [S 2– ] ion. For that, consider :
HS – 
H + + S 2– H 2 S 
H + + HS –
K 2 = 
K 1 = 
∴ [HS – ] = 
....
and [H 2 S] = 
= 
....
Put & in
x = [S 2– ] 
x = 
x = 
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