To measure the quantity of $$MnCl2$$ dissolved in an aqueous solution, it was completely converted to $$KMnO4$$ using the reaction,$$MnCl2$$ $$+$$ $$K2S2O8$$ $$+$$ $$H2O$$→$$KMnO4$$ $$+$$ $$H2SO4$$ $$+$$ HCl (equation$$ not $$balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic $$acid(225$$ $$g)$$ was added in portions till the color of the permanganate ion disappeared. The quantity of $$MnCl2$$ (in$$ $$mg) present in the initial solution is $$___$$.(Atomic$$ weights in g mol–$$1$$ : Mn $$=$$ $$55$$, Cl $$=$$ $$35.5).

Question

To measure the quantity of $$MnCl2$$ dissolved in an aqueous solution, it was completely converted to $$KMnO4$$ using the reaction,$$MnCl2$$  $$+$$ $$K2S2O8$$  $$+$$ $$H2O$$→$$KMnO4$$  $$+$$ $$H2SO4$$  $$+$$ HCl (equation$$ not $$balanced).Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic $$acid(225$$ $$g)$$ was added in portions till the color of the permanganate ion disappeared. The quantity of $$MnCl2$$ (in$$ $$mg) present in the initial solution is $$___$$.(Atomic$$ weights in g mol–$$1$$ : Mn $$=$$ $$55$$, Cl $$=$$ $$35.5).

Infinity Learn · Accepted Answer

$$MnCl2amole+K2S2O8+H2O$$→$$KMnO4amole+H2SO4+HClC2O4$$−−$$+MnO4$$−→$$CO2meq$$ of $$C2O4$$−−$$=meq$$ of $$MnO4$$− $$2$$×$$0.225/90=a$$×$$5a=1$$×[$$55+71$$]$$=126mg$$

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