Question

500 mL of 0.150 M AgNO₃ solution were added in 500 mL of 1.09 M Fe²⁺ solution and the reaction is allowed to reach an equilibrium at $25^{{}^{\circ }}\text{C}$ .
${\left(\text{Ag}\right)}^{+}\left(\text{aq}\right)+{\left(\text{Fe}\right)}^{2+}\left(\text{aq}\right)\rightleftharpoons {\left(\text{Fe}\right)}^{3+}\left(\text{aq}\right)+\text{Ag}\left(\text{s}\right)$
For 25 mL of the final solution, 30 mL of 0.0832 M KMnO₄ were required for oxidation. Calculate the equilibrium constant (in M^-1) of the reaction at $25^{{}^{\circ }}\text{C}$ .
[Report your answer by rounding it up to the nearest whole number]

Answer 1

Answer: 3