What concentration of SO32- is in equilibrium with Ag2SO3(s) and 2.90 × 10-3 M Ag ?...
What concentration of SO32- is in equilibrium with Ag2SO3(s) and 2.90 × 10-3 M Ag ? The Ksp of Ag2SO3 can be found here.
Homework Answers
The solubility product for the reaction is equilibrium constant where the solid ionic compound dissociates into its ions in a solution. Solubility product is denoted as
. Solubility product value relates to the saturated solution and indicates the precipitate level of the compound.
Solubility product value of the compound depends on the concentrations of its ions in a solution.
Example: AB is any solid ionic compound.
![AB(s) =A* (aq) +B* (aq)
K = A*B*]](http://img.homeworklib.com/questions/d8b7b480-f658-11eb-b33c-61d547068173.png?x-oss-process=image/resize,w_560)
Precipitation: If the solubility product value is lesser than the concentration of the ions present in the solution, the compound precipitates in the solution.
Given ionic solid is 
Equilibrium equation of the ionic compound
Now
Solubility product of the ionic compound
![K. =[Ag*] [s0,?]](http://img.homeworklib.com/questions/d9875400-f658-11eb-b837-bfece0e5cec8.png?x-oss-process=image/resize,w_560)
Given that
The concentration 
ion is 
Solubility product of the given ionic solid is 
Now
![K. = [Ag*] [s0,]
1.5*10*4 =(2.90x10)[s0,]
[S0,]= _1.5*10-
(2.90x103)
=1.78x10M](http://img.homeworklib.com/questions/daa399d0-f658-11eb-9265-f16d0a83d5fe.png?x-oss-process=image/resize,w_560)
Therefore, the concentration of 
is 
The concentration of is
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