A solution of 0.1MKMnO4 is used for the reaction, S2O2−3+2MnO−4+H2O⟶MnO2+SO2−4+OH−. What volume of solution in mL will be required to react with 0.158g of Na2S2O3? (in mL as nearest integer)
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Solution
The redox changes are as follows:
(S2+)2⟶2S6++8e[ENa2S2O3=M8] Mn7++3e⟶Mn4+ ('n' factor for KMnO4=3) ∴Meq.ofKMnO4=Meq.ofS2O2−3 0.1×3×V=0.1581588×1000 ∴V=26.67mL