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500 ml of 0.150 M AgNO ₃ solution is mixed with 500 ml of 1.09 M Fe ²⁺ solution and the reaction is allowed to reach equilibrium at 25^ C . Ag ⁺( aq )+ Fe ²⁺( aq ) Fe ³⁺( aq )+ Ag ( ~s ) For 25 ml of the equilibrium solution, 30 ml of 0.0833 M KMnO ₄ were required for oxidation. Calculate the approximate equilibrium constant for the reaction at 25^ C .

Correct answer

3

Step-by-step solution

Ag ⁺( aq )+ Fe ²⁺( aq ) Ag ( s )+ Fe ³⁺( aq ) array ll No. of mmoles initially & 500 0.15 & 500 1.09 & 0 & 0 & =75 & =545 at equilib & 75-x & 545-x & x & x array On titration of reaction mixture with KMnO ₄ , only Fe ²⁺ reacts with it. Equivalents of Fe ²⁺ in 25 ml = Equivalents of KMnO ₄ (545-x) 1000 25 10⁻³ 1=30 10⁻³ 0.0833 5 aligned & K_c= (545-x) 25 1000 [ Ag ³⁺ ] [ Fe ²⁺ ] = 4.5 ; 545-x (75-45) 1000 (545-45) 1000 =500 ; x=45 & 30 500 aligned 3.0 .

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