In the following unbalanced reaction

A²⁺ + B³⁺ $\to$A⁴⁺ + B

The total number of e^- transferred during reaction is 

Which of the following is not an intramolecular redox reaction?

 The compound having oxygen in - 1 oxidation state is:-

What will be the value of x and y by balancing the reaction

C₂H₅OH + X I₂ + Y OH^- $\to$CHI₃ + HCO₂^- + 5I^- + 5H₂O

Which is the correct set that can only act as an oxidant?

Which one is correct about CH₂ = CCl₂?

N₂H₄ + IO₃^- + 2H⁺ + Cl^- $\to$ICl + N₂ + 3H₂O

The equivalent masses of N₂H₄ and KIO₃ respectively are :-

In which of the following compound oxidation state of Fe is zero:-

In the given reaction,

xBrO_3^- + yCr⁺³ + zH₂O $\to$Br₂ + CrO₄^2- + H⁺

The coefficients x, y, and z are respectively-

What is the equivalent weight of H₃PO₃ in the following disproportionation reaction:-

H₃PO₃ $\to$H₃PO₄ + PH₃

Identify the substance acting as an oxidant in the following reaction:

BaCl₂ + Na₂SO₄$\to$BaSO₄ + 2NaCl

In the following reaction

Al + Fe₃O₄ $\to$Al₂O₃ + Fe

The total number of electrons transferred will be-

A metallic oxide contains 40% oxygen then equivalent weight of metal is 

3Cl₂ + 6NaOH $\to$5NaCl + NaClO₃ + 3H₂O, the equivalent weight of NaOH will be

In the conversion, H₂SO₄ $\to$H₂S₂O₈ which process occurs?

Oxidation number of carbon in CH₂Cl₂ is 

Equivalent weight of a metal oxide is 20, the equivalent weight of sulphate of same metal will be 

15 gm Ba(MnO₄)₂ sample containing inert impurity is completely reacting with 100 ml of '11.2 V' H₂O₂, then what will be the % purity of Ba (MnO₄)₂ in the sample ? (Atomic mass Ba = 137, Mn = 55)

The equivalent mass of H₃BO₃ (M = Molar mass of H₃BO₃) in its reaction with NaOH to from Na₂B₄O₇ is equal to –

The number of moles of ferrous oxalate oxidised by one mole of KMnO₄ is

In the reaction Na₂S₂O₃ + 4Cl₂ + 5H₂O → Na₂SO₄ + H₂SO₄ + 8HCI the equivalent weight of Na₂S₂O₃ will be

(M= molecular weight of Na₂S₂O₃)

Which of the following equations is a balanced one

An excess of NaOH was added to 100 mL of a ferric chloride solution. This caused the precipitation of 1.425 g of Fe(OH)₃. Calculate the normality of the ferric chloride solution

In the reaction CrO₅ + H₂SO₄ → Cr₂(SO₄)₃ + H₂O + O₂

The number of moles of O_{2 liberated by one mole of CrO}5 _{will be -}

0.4g of a polybasic acid H_nA (all the hydrogens are acidic) requires 0.5g of NaOH for complete neutralization. The number of replaceable hydrogen atoms in the acid and the molecular weight of 'A' would be : (Molecular weight of the acid is 96 gms.)

25.0 g of FeSO₄.7H₂O was dissolved in water containing dilute H₂SO₄, and the volume was made up to 1.0 L. 25.0 mL of this solution required 20 mL of an N/10 KMnO₄ solution for complete oxidation. The percentage of FeSO₄^. 7H₂O in the acid solution is

25 mL of a solution containing HCl and H₂SO₄ required 10 mL of a 1 N NaOH solution for neutralization. 20 mL of the same acid mixture on being treated with an excess of AgNO₃ gives 0.1425 g of AgCf. The normality of the HC and the normality of the H₂SO₄ are respectively

If 10 gm of V₂O₅ is dissolved in acid and is reduced to V²⁺ by zinc metal, how many moles of I₂ could be reduced by the resulting solution if it is further oxidized to VO²⁺ ions?

[Assume no change in state of Zn²⁺ions] (V = 51, O =16, I = 127) :

0.70 g of mixture (NH₄)₂ SO₄ was boiled with 100 mL of 0.2 N NaOH solution till all the NH₃(g) evolved and get dissolved in solution itself. The remaining solution was diluted to 250 mL. 25 mL of this solution was neutralized using 10 mL of a 0.1 N H₂SO₄ solution. The percentage purity of the (NH₄)₂ SO sample is

A mixed solution of potassium hydroxide and sodium carbonate required 15 mL. of an N/20 HCI solution when titrated with phenolphthalein as an indicator. But the same amount of the solution when titrated with methyl orange as an indicator required 25 mL of the same acid. The amount of KOH present in the solution is