The concentration of silver ions in the equilibrium mixture can be found bytitration with potassium thiocyanate. Silver thiocyanate precipitates.Ag+(aq) + CNS–(aq) AgCNS(s) When all the silver ions have reacted, a deep red complex ion ofiron(III) thiocyanate forms. In an experiment, 25.0 cm3 of 0.100 mol dm–3 silver nitrate solution was addedto 25.0 cm3 of 0.100 mol dm–3 of iron(II) sulfate solution, mixed thoroughly, andallowed to stand overnight in an air-tight container. 10.0 cm3 samples of the reaction mixture were then titrated with 0.0200 mol dm–3potassium thiocyanate solution. The average titre was 5.60 cm3. (i) The initial concentrations of silver ions and iron(II) ions in the reactionmixture are the same. Calculate this initial concentration in mol dm–3. can some one help me on this question