1. For silver chloride, the reaction is AgCl <-> Ag+ and Cl- and ksp= 1.8 x 10^-
ID: 998899 • Letter: 1
Question
1. For silver chloride, the reaction is AgCl <-> Ag+ and Cl- and ksp= 1.8 x 10^-10 a. Determine the concentration of chloride ions in a saturated (at equilibrium) solution)
b. Use your answer from part a to calculate the mass of silver chloride that can be dissolved in 100 ml of water
2. For sodium chloride the reaction is Nacl<-> Na+ and Cl-
a. determine the concentration of chloride ions in a saturated solution
b. Use your answer from part a to calculate the mass of sodium chloride that can be dissolved in 100 ml of water
3. We generally state that sodium chloride is soluble in water and silver chloride is insoluble in water. What does it mean to be soluble or insoluble?
Thanks!
Explanation / Answer
1) Ksp of AgCl = 1.8 x 10^-10 = [Ag+][Cl-]
Let solubility of AgCl = s
1.8 x 10^-10 = [s][s]
s = 1.34 X 10^-5 Moles / L ] = concentration of chloride ion in saturated solution
b) solubility of AgCl = 1.34 X 10^-5 moles / L
Therefore mass which can be dissolved in one litre = Molarity X molecular weight of AgCl = 1.34 X 10^-5 X 143.3 g / L
= 0.00192 g / L
So the mass which can be dissolved in 100mL = 1.92 X 10^-4 grams
b) the solubility product of NaCl= 36 [approx]
Ksp = [Na+][Cl-] = s X s
s= solubility of NaCl
36 = s^2
s = 6 moles / Ltire= concentration of chloride ion in the saturated solution
b) solubility of NaCl in 1L = 6 moles
Mass solubility of NaCl in 1L= moels X molecualr weight == 6 X 58.5 = 351 g / Litre
so solubility in 100mL = 35.1 grams [approx]
3) The solubility is less means that the ionic product of AgCl is much much greater than the Ksp and hence it is less soluble or forms ppt easily
While for NaCl, the ionic product is less than Ksp upto very high concentration hence it is highly soluble in water
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