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Q.1 1 gram molecule of chlorine combines with a certain
weight of a metal giving 111 g of its chloride. The same
weight of the metal displaced 2 g of hydrogen from an acid.
The atomic weight of the metal
(assuming its valency to be 2) is :
(A) 40
(B) 20
(C) 80
(D) none of these
Q.2 A solution of
KMnO4 is reduced to MnO2. the normality of
solution is 0.6 N. The molarity is
(A) 1.8 M
(B) 0.6 M
(C) 0.2 M
(D) 0.1 M
Q.3 9 gm of Al (at.
Wt. = 27) will react completely with an
acid to give :
(A) one mole of H2
(B) one half mole of H2
(C) one-third mole of H2
(D) none of these
Q.4 Number of moles
of electrons taken up when 1 mole of
NO3– ions is reduced to 1 mole of NH2OH is :
(A) 2
(B) 4
(C) 5
(D) 6
Q.5 What volume of
chlorine at STP is required to liberate all
the iodine from 200 ml of 0.2 M KI solution :
(A) 896 ml
(B) 448 ml
(C) 224 ml
(D) 672 ml
Q.6 5 ml of N HCl,
20 ml N/2 H2SO4 and 30 ml of N/3
HNO3 are mixed together and volume
made to 1 litre. The normality
of resulting solution is :
(A) N/5
(B) N/10
(C) N/20
(D) N/40
Q.7 Equivalent mass
of Na2S2O3 in its reaction with I2 is equal to :
(A) molar mass
(B) molar mass/2
(C) molar mass/3
(D) molar mass/4
Q.8 A certain
compound has the molecular formula X4O6.
If 10 gm of compound contains
5.62 g of X, the atomic mass of X :
(A) 32 amu
(B) 37 amu
(C) 42 amu
(D) 48 amu
Q.9 The no. of mol. of the independent species present in one
mole of potash alum
(A) 32
(B)16
(C) 38
(D) 64
Q.10 How many gram of H3PO4 would be needed to
100 gm of Mg (OH)2 ?
(A) 66.7 gm
(B) 252 gm
(C) 112.6 gm
(D) 168 gm
Q.11 Hardness of water
sample is 300 ppm CaCO3. Hence its
molarity is :
(A) 0.3 M
(B) 0.030 M
(C) 0.003 M
(D) 0.0015 M
Q.12 What weight of CuSO4.5H2O must be taken to make 0.5
litre of 0.01 M Cu2+ ions solution ?
(A) 12.45 gm
(B) 1.245 gm
(C) 6.24 gm
(D) 100 gm
Q.13 Calculate the
volume of CO2 produced by the combustion
of 40 ml of acetone vapors in presence of excess of oxygen
(A) 12 ml
(B) 1.20 ml
(C) 120 ml
(D)
11.2 ml
Q.14 A partially dried
clay mineral contains 8% water. The
original sample contained 12 % water and 45 % silica. The %
of silica in the partially dried sample is nearly :
(A) 50 %
(B) 49 %
(C) 55 %
(D) 47 %
Q.15 When one gram
mole of KMnO4 reacts with HCl,
the volume of chlorine liberated
at NTP will be :
(A) 11.2 litres
(B) 22.4 litres
(C) 44.8 litres
(D) 56.0 litres
Q.16 8 g of sulphur is
burnt to form SO2 which is
by Cl2 water. The solution is treated
with BaCl2 solution.
The amount of BaSO4 precipitated is :
(A) 1 mole
(B) 0.5 mole
(C) 0.24 mole
(D) 0.25 mole
Q.17 1 gram of a carbonate of a metal was dissolved in 25 ml
of 1N HCl. The resulting liquid required 5 ml of N
NaOH
for neutralization. The eq. wt. of metal carbonate is :
(A) 100
(B) 30
(c) 40
(D) 50
Q.18 Sulphuryl chloride SO2Cl2 reacts with water to give a
mixture of H2sO4 and HCl. How many moles of NaOh would
be needed to neutralize the
solution formed by adding 1
mole of SO2Cl2 to excess of water .
(A) 1
(B) 3
(C) 2
(D) 4
Q.19 Hydrogen peroxide in aqueous solution decomposes on
warming to give oxygen according to the equation
2H2O2(aq.) ¾® 2H2O(l) + O2(g) under conditions where
one mole of gas occupies 24 dm3, 100 cm3 of XM solution
of H2O2 produces 3dm3 of O2. X is thus :
(A) 2.5
(B) 1
(C) 0.5
(D) 0.25
Q.20 In an experiment
50 ml of 0.1 M solution of a salt
reacted with 25 ml of 0.1 M
solution of sodium sulphite.
The half equation for the oxidation of sulphite ion is –
SO32– (aq.) + H2O(l) ¾® SO42– (aq.) + 2H+ (aq.) + 2e–
If the
oxidation number of metal in the salt was 3,
what would be the new oxidation
number of metal ?
(A) 0
(B) 1
(C) 2
(D) 4
Q.21 One mole of a
mixture of CO and CO2 requires exactly 20
gram of NaOh in solution
for complete conversion of all the CO2
into Na2CO3. How many grams more of NaOh
would it require for
conversion into Na2CO3 if the mixture (one mole) is
completely
oxidized to cO2 .
(A) 60 grams
(B) 80 grams
(C) 40
grams
(D) 20 grams
Q.22 When BrO3– ion reacts with Br– ion in acid solution Br2
is liberated the equivalent
weight of KBrO3 in this reaction is :
(A) M/8
(B) M/3
(C) M/5
(D) M/6
[ where M is the molar
mass ]
Q.23 A solution
contains both Na2cO3 and NaHCO3 was treated
with excess of Cacl2 solution and filtered. The
precipitate weighed
m1 grams. On adding NaOH in drops to
the filtrate avoiding excess,
a further m2 grams was precipitated. If after
adding excess CaCl2,
the solution (had not been
filtered) but was simply boiled and then
filtered, what would be the total
weight of the precipitate ?
(A) (m1 + m2) grams
(B) (m1 + m2/2) grams
(C) (m1 + m2) /2 grams
(D)
(m2+m1/2) grams
Q.24 2 grams of a gas mixture of CO and CO2 on reaction with
excess I2O5 yield 2.54 grams of I2. 7What would be the weight
% of CO in the original mixture ?
(A) 70.1
(B) 75.3
(C) 68.4
(D) 80.7
Q.25 One gram of a
mixture of Na2CO3 and NaHcO3
consumes y gram equivalents of HCl for complete neutralisation.
One gram of the mixture is strongly heated, then cooled
and the
residue treated with HCl. How
many gram equivalents of HCl
would be required for complete neutralisation :
(A) 2y gram equivalent
(B) y gram equivalents
(C) 3y/4 gram equivalents
(D) 3y/2 gram equivalents
Q.26 In an organic
compound of molar mass greater than 100
containing only C, H and N, the
percentage of C is 6 times the
percentage of H while the sum of the percentages of C and H
is 1.5 times the percentage of N.
What is the least molar mass :
(A) 175
(B) 140
(C) 105
(D) 210
Q.27 One gram of a
variable alloy of lead and tin yielded on
treatment with conc. HNO3, filtration and heating 0.42 grams
of SnO2. If all the lead in one gram of alloy is converted into
PbSO4, what will be the weight of PbSO4 obtained ?
(A) 0.98
(B) 1 g
(C) 1.07 g
(D) 0.95 g
Q.28 An iodide
solution, ½ litre containing 0.664 grams
of KI per litre, required 100 ml
of a certain solution of
Ce4+ ion for complete reaction. What is the
normality of
the Ce4+ solution ?
(A) 0.04
(B) 0.004
(C) 0.02
(D) none of these
Q.29 A solution contains Na2CO3 and NaHCO3. 10 ml of the
solution required 2.5 ml of 0.1 M H2SO4 for neutralisation using
phenolphthalein as indicator. Methyl orange is then added when
a further 2.5 ml of 0.2 M H2SO4 was required. The amount
of Na2CO3 and NaHCO3 in 1 litre of the solution is :
(A) 5.3 g & 4.2 g
(B) 3.3 g & 6.2 g
(C) 4.2 g & 5.3 g
(D) 6.2 g & 3.3 g
Q.30 0.7 g of a sample
of Na2CO3. x H2O were dissolved
in water and the volume was made
to 100 ml . 20 ml of this
solution required 19.8 ml of N/10
HCl for
complete
neutralization. The value of x is :
(A) 7
(B) 3
(C) 2
(D) 5
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