Ionic EquilibriumHard
Question
Which of the following statements is correct for a solution saturated with AgCl and AgBr if their solubilities in moles per litre in separate solutions are x and y respectively ?
Options
A.[Ag+] = x + y
B.[Ag+] = [Br-] + [Cl-]
C.[Br-] = y
D.[Cl-] > x.
Solution
AgCI ⇋ Ag+ + CI- AgBr ⇋ Ag+ + Br-
x x y y
(x + y) x (x + y) y
So [Ag+] = [Br-] + [CI–]
x x y y
(x + y) x (x + y) y
So [Ag+] = [Br-] + [CI–]
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
When 10 mL of 0.1 M acetic acid (pKa = 5.0), is titrated against 10mL of 0.1 M ammonia solution (pKa = 5.0), the equival...n-coproic acid C5H11COOH found in coconut and palm oil is used in making artificial flavours and it has solubility in wa...The concentration of hydroxyl ion in a solution left after mixing 100 mL of 0.1 M MgCI2 and 100 mL of 0.2 M NaOH (KSP of...2.5 mL of M weak monoacidic base(Kb = 1 × 10-12 at 25o C) is titrated with M HCl in water at 25oC. The concentratio...The strength of an aqueous solution of I2 can be determined by titrating the solution with standard solution of:...