Ionic EquilibriumHard
Question
Unexposed silver halides are removed from photographic film when they react with sodium thiosulphate to form the complex ion Ag(S2O3)23−. What amount of Na2S2O3 is needed to prepare 1 L of a solution that dissolves 0.1 moles of AgBr by the formation of Ag(S2O3)23−? Ksp of AgBr = 4.0 × 10–13 and Kf of Ag(S2O3)23− = 1.6 × 1012.
Options
A.3.25 g
B.3.25 moles
C.0.325 moles
D.6.5 moles
Solution
$AgBr(s) + 2S_{2}O_{3}^{2 -} \rightleftharpoons Ag\left( S_{2}O_{3} \right)_{2}^{3 -} + Br^{-}$
0.1 a M 0 0
Eqn/final 0 a – 0.2 0.1 0.1
$K_{eq} = 4 \times 10^{- 13} \times 1.6 \times 10^{12} = \frac{0.1 \times 0.1}{(a - 0.2)^{2}} \Rightarrow a = 0.325$
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Among the following the weakest base is :-...Let the colour of the indicator HIn (colourless) will be visible only when its ionised form (pink) is 25% or more in a s...The degree of hydrolysis of a salt of weak acid and weak base in its 0.1 M solution is found to be 50%. If the molarity ...What is the pH of 4 × 10–3 M–Y(OH)2 solution assuming the first dissociation to be 100% and second dissociation to be 50...Which of the following mixtures will act as buffer ?...