From the definition of Ksp, the product of the concentrations of Ag+ and Cl- can be no more than (1.8 X 10-10)/0.35 = 5.1 X 10-10. Since the only named material that is a source of silver ions is AgCl and the concentrations are molar, this is the maximum possible solubility of AgCl.
1.8 10-5
dicuss the significance of the Ksp of AgCl on the accuracy of the mohr's test
7.9 10-5
Ksp
the higher the Ksp value the more soluble a compound is.
It gives us an indication of its solubility in water. A large solubility constant (Ksp) means it is easily water-soluble. A small Ksp means it is generally insoluble in water.
(AgCl has Ksp = 1.8 x 10-10)-5.1 x 10-10
dicuss the significance of the Ksp of AgCl on the accuracy of the mohr's test
7.9 10-5
9.9 x 10-11
1.2x10-2
Ksp
C.2.1 x 10-4
the higher the Ksp value the more soluble a compound is.
Common Ions tend to suppress reactions Think of LeChatelier's principle You could also use a comparison of Q to Ksp I can't really think of a situation where increasing Ag+ or Cl- would increase solubility. Most of the time Q will be larger than Ksp, so the reaction will shift over to to the solid.
The solution is supersaturated
It gives us an indication of its solubility in water. A large solubility constant (Ksp) means it is easily water-soluble. A small Ksp means it is generally insoluble in water.
1.0 x 10-12