If the ion product concentration is greater than the Ksp value a precipitate will form. If it equals the Ksp the solution is saturated and no precipitate forms.
It means a precipitate will form
Precipitates will form
Ion product < Ksp Unsaturated solution Ion product = Ksp Saturated solution Ion product > Ksp Supersaturated solution
A precipitate will form
Ksp
due to the solubility product constant(ksp)
ksp= [Ca2+][Cl-]^2 = (x)((2x)^2) Ksp =4x^3 where x= the amount soluble of one mole of product
Solubility product constant, Ksp, uses concentrations of soluble (dissolved) substances. A solid is not dissolved.
Ksp or solubility product is meaured for aqueous solutions of salts, for acids is Ka , for bases is Kb and for water is Kw.
If there is no reaction occuring to change the molecular structure of the substance, you have to look at the ionic product of the substance. When the ionic product is more than the Ksp of the substance, there would be precipitation of the substance
Ksp= [Products]^mole ratio so Ksp=[Ag+][NO3] Since you didnt provide any numerical values, that's as far as you can go. You can look for known Ksp values at certain temperatures in some AP Chemistry books or online.
It will decrease the Ksp