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
The pKa of a weak acid, HA, is 4.80. The pKb of a weak base, BOH, is 4.78. The pH of an aqueous solution of the correspo...To prepare a buffer of pH 8.26 amount of (NH4)2 SO4 to be added to 500 mL of 0.01 M NH4OH solution [pKa (NH4+) = 9.26] i...Species acting as both bronsted acid as well as base :-...The molar solubility in terms of solubility product Ksp is given by the relation...Biodegradable polymer which can be produced fromglycine and aminocaproic acid is :-...