I\'m really struggling with this question. Working on it for a while with no luc

Question

I'm really struggling with this question. Working on it for a while with no luck.

A solution containing both Mn2+ and Cd2+ at 0.1M each is saturated with H2S gas at 25C and 1 atm, The [H+] is adjusted with HCL to 0.30M.

A) Will the sulfides of these metals precipitate under these conditions?

B) Calculate the maximum concentration of Cd2+ and Mn2+ that can remain in solution.

Ksp for MnS = 1.0x10^-13; Ksp for CdS= 1.0x10^-26

In a saturated solution of H2S at 1 atm and 25C, [H2S] = 0.10 M

Ka1 (H2S)= 1.8x10^-5; Ksp fr Fe(OH)2=1.6x10^-14

Answers are given: A) [OH-] = 1.8x10^-6 M and B) No

Explanation / Answer

Ksp [MnS]= [Mn2+]*[S2-]...............1
Ksp [CdS]= [Cd2+]*[S2-]................2
Ka [H2S]= [H+]`2*[S2-].................3
first solve for H+ ions
using 1 and 3 dividing


you will get H+

in the same way solve for
Cd2+..........

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