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The equivalent weight of a metal is 4.5 and the molecular weight of its chloride is 80. The atomic weight of the metal is:-
1. 18
2. 9
3. 4.5
4. 36

N₂H₄ + IO₃^- + 2H⁺ + Cl^- $\to$ICl + N₂ + 3H₂O
The equivalent masses of N₂H₄ and KIO₃ respectively are :-
1. 8 and 35.6
2. 8 and 87
3. 8 and 53.5
4. 16 and 53.5

What is the equivalent weight of H₃PO₃ in the following disproportionation reaction:-
H₃PO₃ $\to$H₃PO₄ + PH₃
1. $\frac{M}{6}$   
 2. $\frac{M}{2}$ 
3.  $\frac{2M}{3}$ 
 4. $\frac{M}{3}$

In the following reaction
Al + Fe₃O₄ $\to$Al₂O₃ + Fe
The total number of electrons transferred will be-
1. 6
2. 8
3. 8/3
4. 24

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
(1) 78%
(2) 98%
(3) 89%
(4) 79%

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
(1) 0.40 N and 0.05 N
(2) 0.05 N and 0.35 N
(3) 0.50 N and 0.25 N
(4) 0.40 N and 0.5 N

A brown ring complex compound is formulated as $\left[Fe{\left(H_{2}O\right)}_{5}NO\right]S{O}_4.$ The oxidation state of iron is 
1. 1
2. 2
3. 3
4. 0

 The strongest oxidising agent among the following is -
1. $Br{O}_3^{-}/B{r}^{2+},E^o=+1.50$
2. $F{e}^{3+}/F{e}^{2+},E^o=+0.76$
3. $Mn{O}_4^{-}/M{n}^{2+},E^o=+1.52$
4. $C{r}_2{O}_7^{2-}/C{r}^{3+},E^o=+1.33$

In an alkaline medium ClO₂ oxidize H₂O₂ in O₂ and reduces itself in Cl^– . How many moles of H₂O₂ will be oxidized by one mole of ClO₂?

Equivalent mass of FeS₂ in the half reaction, ${\mathrm{FeS}}_2\to {\mathrm{Fe}}_2{\mathrm{O}}_3+{\mathrm{SO}}_2$ is :
1. M/10
2. M/11
3. M/6
4. M/1

The equivalent mass of HCl in the given reaction is :
${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7+14 \mathrm{HCl}\to 2\mathrm{KCl}+2{\mathrm{CrCl}}_3+3{\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{O}$
1. 16.25
2. 36.5
3. 73
4. 85.1

Equivalent mass of ${\mathrm{H}}_3{\mathrm{PO}}_2$ when it disproportionate into ${\mathrm{PH}}_3$ and ${\mathrm{H}}_3{\mathrm{PO}}_3$ is :
1. M
2. M/2
3. M/4
4. 3M/4

In the following reaction, ${\mathrm{As}}_2{\mathrm{S}}_3+{\mathrm{H}}^{+}+{\mathrm{NO}}_3^{-}\to \mathrm{NO}+{\mathrm{H}}_2\mathrm{O}+{\mathrm{AsO}}_4^{3-}+{\mathrm{SO}}_4^{2-}$, the equivalent mass of ${\mathrm{As}}_2{\mathrm{S}}_3$ is related to its molecular mass by:
1. M/2
2. M/4
3. M/24
4. M/28

Sulphur forms the chlorides ${\mathrm{S}}_2{\mathrm{Cl}}_2$ and ${\mathrm{SCl}}_2$. The equivalent mass of sulphur in ${\mathrm{SCl}}_2$ is :
1. 8 g/mol
2. 16 g/mol
3. 64.8 g/mol
4. 32 g/mol
 

The equivalent mass of an element is 4. Its chloride has a vapour density 59.25. Then, the valency of the elements is :
1. 4
2. 3
3. 2
4. 1
 

$6\times {10}^{-3}$ mole ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ reacts completely with $9\times {10}^{-3}$ mole ${\mathrm{X}}^{\mathrm{n}+}$ to give ${\mathrm{XO}}_3^{-}$ and ${\mathrm{Cr}}^{3+}$. The value of n is :
1. 1
2. 2
3. 3
4. None of these

What mass of ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4.2{\mathrm{H}}_2\mathrm{O}$ (mol. mass = 126) should be dissolved in water to prepare 250 mL of centinormal solution which act as a reducing agent ?
1. 0.63 g
2. 0.1575 g
3. 0.126 g
4. 0.875 g

The equivalent mass of salt, ${\mathrm{KHC}}_2{\mathrm{O}}_4.{\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4.4{\mathrm{H}}_2\mathrm{O}$ when it act as reducing agent is :
1. $\frac{\mathrm{Mol}. \mathrm{mass}}{1}$
2. $\frac{\mathrm{Mol}. \mathrm{mass}}{2}$
3. $\frac{\mathrm{Mol}. \mathrm{mass}}{3}$
4. $\frac{\mathrm{Mol}. \mathrm{mass}}{4}$

The equivalent mass of divalent metal is W. The molecular mass of its chloride is ::
1. W + 35.5
2. W + 71
3. 2W + 71
4. 2W + 35.5

When ${\mathrm{BrO}}_3^{-}$ ion reacts with ${\mathrm{Br}}^{-}$ in acidic medium, ${\mathrm{Br}}_2$ is liberated. The equivalent mass of ${\mathrm{Br}}_2$ this reaction is :
1. $\frac{5\mathrm{M}}{8}$
2. $\frac{5\mathrm{M}}{3}$
3. $\frac{3\mathrm{M}}{5}$
4. $\frac{4\mathrm{M}}{6}$

If ${\mathrm{m}}_{\mathrm{A}}$ gram of a metal displaces ${\mathrm{m}}_{\mathrm{B}}$ gram of another metal B from its salt solution and if equivalent mass are ${\mathrm{E}}_{\mathrm{A}}$ and ${\mathrm{E}}_{\mathrm{B}}$ respectively then equivalent mass of A can be expressed as :
1. ${\mathrm{E}}_{\mathrm{A}}=\frac{{\mathrm{m}}_{\mathrm{A}}}{{\mathrm{m}}_{\mathrm{B}}}\times {\mathrm{E}}_{\mathrm{B}}$
2. ${\mathrm{E}}_{\mathrm{A}}=\frac{{\mathrm{m}}_{\mathrm{A}}\times {\mathrm{m}}_{\mathrm{B}}}{{\mathrm{E}}_{\mathrm{B}}}$
3. ${\mathrm{E}}_{\mathrm{A}}=\frac{{\mathrm{m}}_{\mathrm{B}}}{{\mathrm{m}}_A}\times {\mathrm{E}}_{\mathrm{B}}$
4. ${\mathrm{E}}_{\mathrm{A}}=\sqrt{\frac{{\mathrm{m}}_{\mathrm{A}}}{{\mathrm{m}}_{\mathrm{B}}}\times {\mathrm{E}}_{\mathrm{B}}}$