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

1. 40

2. 48

3. 60

4. 80

In the conversion, H₂SO₄ $\to \hspace{0.17em}$H₂S₂O₈ which process occurs?

1. Oxidation

2. Reduction

3. Oxidation as well as reduction

4. Neither oxidation nor reduction

Oxidation number of carbon in CH₂Cl₂ is 

1. -4

2. +4

3. -2

4. zero

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

(1) 60

(2) 69

(3) 108

(4) 54

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)

(1) 5%

(2) 10%

(3) 50%

(4) none

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

(1) M

(2) $\frac{\text{M}}{\text{2}}$

(3) $\frac{\text{M}}{4}$

(4) $\frac{\text{M}}{6}$

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

(1) $\frac{5}{2}$

(2) $\frac{2}{5}$

(3) $\frac{3}{5}$

(4) $\frac{5}{3}$

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

1. M/4

2. M/8

3. M/1

4. M/2

(M= molecular weight of Na₂S₂O₃)

Which of the following equations is a balanced one

(1) 5BiO₃^-+ 22H⁺ + 2${\mathrm{Mn}}^{2+}$ → 5Bi³⁺ + 7H₂O + 2MnO₄^–

(2)5BiO₃^- + 14H⁺ + 2${\mathrm{Mn}}^{2+}$ → 5Bi³⁺ + 7H₂O + 2MnO₄^–

(3)2BiO₃^- + 4H⁺ + 2Mn²⁺ → 6Bi³⁺ + 2H₂O + MnO₄^–

(4) 6BiO₃^-+ 12H⁺ + 2Mn²⁺ → 6Bi³⁺ + 6H₂O + 2MnO₄^–

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

(1) 0.20 N

(2) 0.50 N

(3) 0.25 N

(4) 0.40 N