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

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

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

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 :