Equivalent Ma...

Equivalent Mass

Trending Questions

What is the n-factor of $H_{3} P O_{3}$ ?

1 or 2
3
1
1 or 2 or 3

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What is the equivalent weight of Iron in Ferric Chloride?

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Q. In the following reaction,

N a_{2} S_{2} O_{3}

is converted to

N a_{2} S_{4} O_{6}

2 N a_{2} S_{2} O_{3} + I_{2} \to N a_{2} S_{4} O_{6} + 2 N a I

The equivalent weight of

N a_{2} S_{2} O_{3}

for this reaction is:
(The molecular weight of

N a_{2} S_{2} O_{3} = M)

$M$
$\frac{M}{4}$
$\frac{M}{2}$
$\frac{M}{3}$

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Q. when BrO3^- ion react with Br^- ion in acidic medium , Br2 is liberated.the equivalent mass of Br2 in the reaction is (M=molar mass of Br2) (1)5/3M (2)3/5M (3)4/6M (4)5/8M

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5

moles of a mixture of

F e S O_{4}

and

F e_{2} (S O_{4})_{3}

required

150 m L

1.0 M K M n O_{4}

in acidic medium for the complete neutralisation. Calculate the mole fraction of

F e S O_{4}

in the initial mixture.

$0.2$
$0.33$
$1.5$
$0.15$

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Q. 30. N2 + 3*H2--->2*NH3 , molecular weight of NH3 and N2 are X1 and X2, their equivalent weight are Y1 and Y2, then (Y1-Y2) is (1)2*X1-X2/6 (2)X1-X2 (3)3*X1-X2 (4)X1-3*X2

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Equal volumes of 10% $\frac{v}{v}$ of HCl is mixed with 10% $\frac{v}{v}$ NaOH solution. If density pure NaOH is 1.5 times that of pure HCl then the resultant solution be

Neutral
Acidic
Basic
Can't be predicted

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Q. What is the equivalent weight of Sodium Oxide (Na2O)? Is it 62 or 31g?

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Calculate the valency factor of the following:
(i) Ca $\to$ ${C a}^{2 +}$ + 2 $e^{-}$
(ii)K $\to$ $K^{+}$ + $e^{-}$

(iii) ${M n}^{7 +}$ + 5 $e^{-}$ $\to$ ${M n}^{2 +}$

2, 1, 5
2, 1, 7
1, 3, 7
1, 2, 5

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Q. On heating

0.199 g

of a metallic oxide in a stream of hydrogen,

0.045 g

of water is formed. Find the equivalent weight of the metal.

$61.2 g$
$31.8 g$
$12.7 g$
$15.5 g$

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Q. What volume of 0.25M Hcl is required to react completely with 22.6g of Na2co3 according to the equation Na2Co3+2Hcl=2Nacl=H20 (2) The molecular mass of organic compound is 78% and and its %composition is 92.4%C and 7.6%H.Find the molecular formula of the compound.

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1.20 g

sample of

N a_{2} C O_{3}

and

K_{2} C O_{3}

was dissolved in water to form

100 m L

of a solution.

20 m L

of this solution required

40 m L

0.1 N H C l

for complete neutralization. Calculate the weight of precipitate in the mixture if another

20 m L

of this solution is treated with excess of

B a C l_{2}

$0.394 g$
$0.596 g$
$0.604 g$
$0.115 g$

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Q. 35.Calculate the equivalent weight of following underlined CuSO4 + KI > Cu2I2 + K2SO4 + I2

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Q. Find the equivalent weight of

K M n O_{4}

in the given reaction, if the molar mass of

M n O_{4}^{-}

is 'M' ?

K M n O_{4} \to M n^{2 +}

(acidic medium)

$41.6$
$21.6$
$11.6$
$31.6$

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Q. The equivalent weight of Mohr’s salt,

F e S O_{4} . (N H_{4})_{2} S O_{4} .6 H_{2} O

is equal to:

Molar weight of Mohr’s salt
One-fourth of the molar weight
Half of its molar weight
One-third of the molar weight

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Q. The equivalent weight of a divalent metal is

W

. The molecular weight of its chloride

$W + 35.5$
$2 W + 35.5$
$W + 71$
$2 W + 71$

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Q. Consider the following redox reaction:

N a B r O_{3} + 6 H^{+} + 6 e^{-} \to N a B r + 3 H_{2} O

Calculate the weight of sodium bromate

(N a B r O_{3})

required to prepare

0.6 N

100 m L

solution.
(Given : Molar mass of

N a B r O_{3} = 151 g m o l^{- 1}

)

$2 g$
$0.151 g$
$1.51 g$
$15.1 g$

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Q. 43. The initial concentration of was twice of initial concentration of B.At equilibrium the concentration of C was thricethe concentration of B calculate Kc andkp

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Q. A

10 g

sample of

C u S

and

C u_{2} S

was treated with

100 m L

1.25 M K_{2} C r_{2} O_{7}

to produce

C r^{3 +}, C u^{2 +}

and

S O_{2}

. The excess oxidant was reacted with

50 m L

F e^{2 +}

solution.

25 m L

of the same

F e^{2 +}

solution required

0.875 M K M n O_{4}

under acidic condition, the volume of

K M n O_{4}

used was

20 m L

. Find the percentage of

C u_{2} S

in the sample.
Given: molar mass of

C u

63.5 g m o l^{- 1}

$28.7 %$
$71.3 %$
$57.4 %$
$42.6 %$

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3 g

of an oxide of a metal is converted to form

5 g

of its chloride. The equivalent weight of the metal is:

$33.25 g$
$45.63 g$
$63.57 g$
$98.81 g$

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Q. in alkaline medium what will be the equivalent weight of I2 on its conversion to iodate ion

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Calculate the n-factor for $N H_{4} O H$

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Q. Commercially available conc. HCl contains 38% HCl by mass. What is the molarity of this solution? Density is 1.19g/cm3

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Q. The number of moles of oxalate ions oxidized by one mole of

M n O_{4}^{-}

ion in acidic medium.

$\frac{5}{2}$
$\frac{2}{5}$
$\frac{3}{5}$
$\frac{5}{3}$

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M g

can reduce

N O_{3}^{-}

N H_{3}

in basic medium.

N O_{3}^{-} (a q) + M g (s) + H_{2} O \to M g (O H)_{2} (s) + O H^{-} (a q) + N H_{3} (g)

25.0 m L

sample of

N O_{3}^{-}

solution was treated with

M g (s)

. The

N H_{3} (g)

was passed into

100 m L

0.15 N H C l

.
The excess of

H C l

required

32.10 m L

0.10 N N a O H

for neutralization. What was the molarity of

N O_{3}^{-}

ions in the original sample?

$0.47125$
$0.3025$
$3.025$
$0.5005$

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Q. P4+3 NaOH+3 H2O→ PH3+3 NaH2PO2The equivalent mass of p4 in the above reaction is \lbrack M is the molecular mass of P4\rbrack

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Q. Write chemical reactions to show the amphoteric nature of water.

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Q. 1.85 g sample of an arsenic containing compound pesticide was chemically converted to AsO3- AND TITRATED WITH Pb(AsO4)2. IF 20 ML OF 0.1 M Pb2+ is required to reach the equivalence point , the mass percentage of arsenic in te pesticide sample is closest to

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Gram equivalent mass is constant for a given substance.

True
False

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Q. When non-stoichiometric compound

F e_{0.95} O

is heated in the presence of oxygen, it converts into

F e_{2} O_{3}

, then which of the following statements are correct?

Equivalent weight of $F e_{0.95} O$ is $\frac{M}{0.5}$ where $M$ is molecular weight of $F e_{0.95} O$
The number of moles of $F e^{3 +}$ and $F e^{2 +}$ in $1 m o l e$ of $F e_{0.95} O$ are $0.1$ and $0.85$ respectively
The number of moles of $F e^{3 +}$ and $F e^{2 +}$ in $1 m o l e s$ of $F e_{0.95} O$ are $0.85$ and $0.10$ respectively
The $%$ composition of $F e^{2 +}$ and $F e^{3 +}$ in the non-stoichiometric compound is $89.47 %$ and $10.53 %$ respectively

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