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Q.1 10.78 g of H3PO4 in 550 ml solution is 0.40 N.
Thus this acid :
(A) has been neutralised
to HPO42–
(B) has been neutralized
to PO42–
(C) has been reduced to
HPO32–
(D) has been neutralised
to H2PO4–
Q.2 0.1 mol of MnO4– (in acidic medium) can :
(A) oxidise 0.5 mol of Fe2+
(B) oxidise 0.166 mol of
FeC2O4
(C) oxidise 0.25 mol of C2O42–
(D) oxidise 0.6 mol of Cr2O72–
Q.3 Which of the
following quantities are independent of temperature
(A) Molarity
(B) mole fraction
(C) molality
(D) normality
Q.4 1 mol BaF2 + 2mol H2S4 →resulting mixture will be
neutralised by :
(A) 1 mol of KOH
(B) 2 mol of Ca(OH)2
(C) 4 mol KOH
(D) 2 mol of KOH
Q.5 Which of the
following represent redox reactions :
(A) Cr2O72– + 2OH– →2CrO42– + H2O
(B) 2CrO42– + 2H+ → Cr2O72– + H2O
(C) 2MnO4– + 3Mn2+ + 4OH → 5 MnO2 + 2H2O
(D) 2Cu+ → Cu + Cu2+
Q.6 When (NH4)2 Cr2O7 is heated :
(A) there is oxidation of
N
(B) there is reduction of
Cr
(C) net reaction is
disproportionations
(D) net reaction is
neutralisation
Q.7 Which of the
following are disproportionation reaction ?
(A) 2RCHO → RCOOCH2R
(B) 4H3PO3 →3H3 PO4 + PH3
(C) NH4NO3 → N2O + 2H2O
(D) PCl5 →PCl3 + Cl2
Q.8 For the reaction
: H3PO4 + Ca(OH)2 CaHPO4 + 2H2O
1 mol
1 mol
Which are true statements
:
(A) equivalent weight of H3PO4 is 49
(B) resulting mixture is neutralised by 1 mol of
KOH
(C) CaHPO4 is an acid salt
(D) 1 mol of H3PO4 is completely neutralised by 1.5
mol of Ca(OH)2.
Q.9 3H3PO2 → PH3 + 2H3PO3 . In this reaction :
(A) H3PO2 undergoes disproportionation
(B) equivalent weight of
H3PO2 is 22
(C) equivalent weight of
H3PO2 is 49.5
(D) NaH2PO2 is not acid salt.
Q.10 11.2 g of mixture
of MCl (volatile) and NaCl gave 28.7 g of white ppt with excess of AgNO3 solution. 11.2 g of same mixture
on heating gave a gas that on passing into AgNO3 solution gave 14.35 g of white ppt. Hence:
(A) ionic mass of M+ is 18
(B) mixture has equal mole fraction of MCl and
NaCl
(C) MCl and NaCl are in 1 : 2 molar ratio
(D) ionic mass of M+ is 10
Q.11 H2C2O4 and NaHC2O4 behave as acids as well as
reducing agents. which are correct statement?
(A) equivalent weight of H2C2O4 and NaHC2O4 are equal to their molecular
weights when behaving
as reducing agents
(B) 100 ml of 1 N solution of each is
neutralised by equal volume of 1M Ca(OH)2
(C) 100 ml of 1 N solution of each is
neutralised by equal volume of 1N Ca(OH)2
(D) 100 ml of 1 M solution of each is oxidised
by equal volumes of 1M KMnO4
Q.12 Which of the
following are primary standard substances ?
(A) Na2CO3.10H2O
(B) NaOH
(C) Na2B4O7.10H2O
(D) KMnO4
Q.13 Which of the
following statements are correct ?
(A) the point at which an equivalent amount of
the titrant is added is called the equivalence point.
(B) the point at which the reaction is observed
to be complete is called the end point
(C) at the end point of a reaction there is no
change in the properties of the solution
(D) at the equivalence point of a reaction the
stoichiometric amount of the titrant is not added
Q.14 100 mL of a 0.1 M
SO42- solution is :
(A) 10 millimoles
(B) 5 millimoles
(C) 20 milliequivalents
(D) 40 milliequivalent
Q.15 Which of
following will be
present in the solution formed
when 50 mL of 0.1 M HCl is mixed with 50 mL of 0.1 M NaOH ?
(A) 4.5 m mol of H+
(B) 0.05 m mol of OH-
(C) 0.05 M NaCl
(D) 10-7 M of H+ ion
Q.16 Which of the
following statements are correct ?
(A) during the titration of a strong acid
against a strong base, the pH at the at the equivalence point will be neutral
(B) during the titration of a weak acid against
a strong base, the pH at the at the equivalence point will be alkaline
(C) during the titration of a weak acid against
a strong base, the pH at the at the equivalence point will be acidic
(D) during the titration of a weak acid against
a weak base, the pH at the at the equivalence point will be neutral
Q.17 During the
titration of a mixture of Na2CO3 and NaHCO3 against HCl,
(A) phenolphthalein is used to detect the first
end point
(B) phenolphthalein is used to detect the second
end point
(C) methyl orange is used to detect the second
end point
(D) methyl red is used to detect the first end
point
Q.18 1 mol of H2SO4 will exactly neutralize
(A) 2 mol of ammonia
(B) 1 mol of Ba(OH)2
(C) 0.5 mol of Ba(OH)2
(D) 2 mol of KOH
Q.19 At the end point
there is a sharp change of colour in the indicator. This happens because the
(A) pH at the end point changes sharply
(B) structure of the indicator changes
(C) colour of indicator is adsorbed by water
(D) dissociation
constants of acids and bases differ by ten
Q.20 ‘20 volumes’ of H2O2 is equal to :
(A) 20% H2O2 by mass
(B) 6% H2O2 by mass
(C) 1.764 N
(D) 3.528 N
Q.21 A solution of Na2S2O3 is standardized
iodometrically against 0.1262 g
of KBrO3. This process requires 0.45 mL of Na2S2O3 solution. What is the strength of
the Na2S2O3 ?
(A) 0.2 M
(B) 0.1 M
(C) 0.05 N
(D) 0.1 N
Q.22 Which of the
following expressions is correct ( n = no. of moles of the gas, NA = Avogadro constant, m =
mass of molecule of the gas, N= no. of
molecules of the gas)
(A) n = mNA
(B) m = nNA
(C) N = nNA
(D) m = mn/NA
Q.23 In which of the
following pairs do 1g of each have an equal number of molecules?
(A) N2O and CO
(B) N2 and C3O2
(C) N2 and CO
(D) N2O and CO2
Q.24 Among the
following, which solutions contain equal numbers of millimoles ?
(A) 100 mL of 0.05 M H2SO4
(B) 200 mL of 0.0 M NaOH
(C) 100 mL of 0.10 M Na2C2O4
(D) 200 mL of 0.025 MKOH
Q.25 1 mol of ions contains
(A) 4NA electrons
(B) 7NA protons
(C) 7NA neutrons
(D) 14NA protons
Q.26 11.2 L of gas at
stp weighs 14.0 g. The gas could be :
(A) N2O
(B) NO2
(C) N2
(D) CO
Q.27 The oxidation
number of Cr = + 6 in :
(A) FeCr2O4
(B) KCrO3Cl
(C) CrO5
(D) [Cr(OH)4]–
Q.28 The oxidation
number of carbon is zero in :
(A) HCHO
(B) CH2Cl2
(C) C6H12O6
(D) C12H22O11
Q.29 Which of the
following are not redox reactions ?
(A) Mg + N2 ¾® Mg3N2
(B) K4[Fe(CN)6] + H2SO4 + H2O ¾® K2SO4 + CO + FeSO4 + (NH4)2SO4
(C) I2 + 3Cl2 ¾® ICl3
(D) CuSO4 + NH3 ¾® [Cu(NH3)4]SO4
Q.30 Which of the following are redox reactions ?
(A) NaIO3 + NaHSO3 ¾® NaHSO4 + Na2SO4 + I2 + H2O
(B) FeCl3 + K4[Fe(CN)6] ¾® KCl + Fe4[Fe(CN)6]3
(C) AgCl + Na2S2O3 ¾® Na3[Ag(S2O3)2] + NaCl
(D) NaBiO3 + MnSO4 + HNO3®
HMnO4 + Bi(NO3)3 + NaNO3 + Na2SO4 + H2O
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