1 mole of equimolar mixture of ferric oxalate and ferrous oxalate will require x mol of KMnO4 in acidic medium for complete oxidation. x is
Eq. mass of KMnO4 in acidic medium
0.5 mol of
Total mol of KMnO4 consumed = 0.6 + 0.3 = 0.9
In iodometric estimation of Cu2+ ions, the following reactions take place
If 100mL of CuSO4 solution added to an excess of KI requires 50mL of 0.2 M Na2S2O3, the molarity of CuSO4 solution is
0.66 g H3PO2 will require x mL of 0.1 M NaOH for complete neutralization .x is
20mL solution containing 0.1 M each of HCl and HNO3 required x mL of 0.1 M NaOH for complete neutralization. In another experiment to 20mL of original solution, excess of AgNO3 is added and the precipitate of AgCl is filtered off. The entire filtrate along with washings required y mL of the same NaOH solution for neturalization. Then, which of the following relation is correct?
10g sample of H2O2 just decolorised 100mL of 0.1 M KMnO4 in acidic medium. % by mass of H2O in the sample is
KMnO4 reacts with oxalic acid as :
Hence, 50mL of 0.04 M KMnO4 is acidic medium is chemically equivalent to
Solution A and B of H2SO4 have respective molarities to be 5.0 and 1.0 In order to prepare 10L of 8 N H2SO4, what volumes of A and B solutions need be mixed?
You are given 1 L of 2 N H2SO4 and 1 L 5 N H2SO4. What will be the maximum volume of 1.5 M H2SO4 that you can prepare from these two solutions?
5 mol of mixture of Mohr’s salt and Fe2(SO4)3 requires 500mL of MK2Cr2O7 for complete oxidation in acidic medium. The mole % of the Mohr’s salt in the mixture is
For the reaction : 2H3PO2 → H3PO4 +PH3 , the equilvant mass of H3PO2 is
If x g is the mass of NaHC2O4 required to neutralize 100 mL of 0.2 MNaOH and y g that required to reduce 100 mL of 0.02 M KMnO4 in acidic medium, then