Asked by MikeSo
Im really sorry I got sidetracked:P This is the question I wanted to ask you
In a saturated solution of silver sulfite, the concentration of silver ion is 3.6 x 10^-4 mol/L. The Ksp of silver sulfite willl be what?
Sorry about that
In a saturated solution of silver sulfite, the concentration of silver ion is 3.6 x 10^-4 mol/L. The Ksp of silver sulfite willl be what?
Sorry about that
Answers
Answered by
DrBob222
Do you mean silver sulfite or silver sulfide. I will assume you mean what you wrote. Nothing will change, except the formula, if it is Ag2S.
Ag2SO3 ==> 2Ag^+ + SO3=
Ksp = (Ag^+)^2(SO3^=)
(Ag^+) = 3.6 x 10^-4 from the problem.
(SO3^=) = 1/2 that.
Plug into the Ksp expression and calculate Ksp.
Ag2SO3 ==> 2Ag^+ + SO3=
Ksp = (Ag^+)^2(SO3^=)
(Ag^+) = 3.6 x 10^-4 from the problem.
(SO3^=) = 1/2 that.
Plug into the Ksp expression and calculate Ksp.
Answered by
MikeSo
Ksp = [SO3][Ag]^2 / [Ag2SO3]
= [1.8 x 10^-4][3.6 x 10^-4]^2 /
[ ]
Would I divide by 1.8 x 10^-4 since there is one mole of Ag2So3?
= [1.8 x 10^-4][3.6 x 10^-4]^2 /
[ ]
Would I divide by 1.8 x 10^-4 since there is one mole of Ag2So3?
Answered by
DrBob222
Ksp = (Ag^+)^2(SOc^=).
The denominator is 1, not (Ag2SO3).
This is not an equilibrium constant. No Ksp has anything on the bottom except 1.
The denominator is 1, not (Ag2SO3).
This is not an equilibrium constant. No Ksp has anything on the bottom except 1.
Answered by
sasha
AHHH help i have no idea!!!
Answered by
jul ardian
KSP for Au2 S
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