An equilmolar mixture of Na2C2O4 and H2C2O4 required V1L of 0.1 M KMnO4 in acidic medium for complete oxidation. The same amount of the mixture required V2L of 0.1 M NaOH for neutralization. The ratio of V1 to V2 is
2 : 5
1 mol of H2C2O4 + 1 mol of Na2C2O4 as reductants
1 mol of H2C2O4 as acid = 2 equiv. = 0.1 ×V2 equiv. of
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
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
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
A mixture of K2C2O4 and KHC2O4 required equal volumes of 0.1 M K2Cr2O7 for oxidation and 0.1 M NaOH for neutralization in separate titrations. The molar ratio of K2C2O4 and KHC2O4 in the mixture is :
In an iodometric estimation, the following reactions occur
0.15 mol of CuSO4 of 80% purity was added to excess of KI solution and the liberated iodine required 12 mL 120mL of hypo. The molarity of hypo solution was