Cobalt(II) sulfide, #"CoS"#, has a #K_(sp)# value of #3.0 xx 10^(-26)#. What is the solubility of #"CoS"# in mol/L?
The idea here is that cobalt(II) sulfide,
This means that when cobalt(II) sulfide is dissolved in water, only a tiny fraction of the ions will dissociate.
Your goal here is to calculate the molar concentration of these dissociated ions. To do that, use an ICE table and the dissociation equation for cobalt(II) sulfide.
If you take
#" " "CoS"_ ((s)) rightleftharpoons " ""Co"_ ((aq))^(2+) " "+" " "S"_ ((aq))^(2-)#
By definition, the product solubility constant will be
#K_(sp) = ["Co"^(2+)] * ["S"^(2-)]#
In your case, you have
#K_(sp) = s * s = s^2#
This means that
#s = sqrt(K_(sp)) = sqrt(3.0 * 10^(-26)) = 1.7 * 10^(-13)#
You can thus say that the molar solubility of cobalt(II) sulfide is equal to
#s = color(green)(|bar(ul(color(white)(a/a)color(black)(1.7 * 10^(-13)"mol L"^(-1))color(white)(a/a)|)))#
This means that for every mole of cobalt(II) sulfide added to one liter of water, you will only get a concentration of