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
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.
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?
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.
AHHH help i have no idea!!!
KSP for Au2 S
That's alright! To find the Ksp of silver sulfite, we need to use the given concentration of silver ion. The Ksp expression for silver sulfite can be written as:
Ksp = [Ag+]²[SO₃²⁻]
We are given that the concentration of silver ion ([Ag+]) is 3.6 x 10^-4 mol/L. Since silver sulfite is considered saturated, we assume that all the silver sulfite dissociates to produce silver ion and sulfite ion (SO₃²⁻).
Now, we can substitute the given concentration of silver ion into the Ksp expression:
Ksp = (3.6 x 10^-4 mol/L)²[SO₃²⁻]
However, we don't know the concentration of sulfite ion ([SO₃²⁻]) in the saturated solution. In this case, we assume that the concentration of sulfite ion is equal to the concentration of silver ion, because 1 mole of silver sulfite dissociates to produce 1 mole of silver ion and 1 mole of sulfite ion.
Thus, we can substitute the concentration of silver ion ([Ag+]) into the Ksp expression for sulfite ion as well:
Ksp = (3.6 x 10^-4 mol/L)²(3.6 x 10^-4 mol/L)
Now, we can calculate the value of Ksp:
Ksp = (3.6 x 10^-4)² x (3.6 x 10^-4) = 4.6656 x 10^-11
Therefore, the Ksp of silver sulfite is 4.6656 x 10^-11.