TEST SERIES FOR AIPMT (HALF SYLLABUS) - Career Point

Q.77 During electrolysis of H2O, the molar ratio of H2
and O2 formed is -
(1) 2 : 1 (2) 1 : 2 (3) 1 : 3 (4) 1 : 1
Q.78 At liquid vapour equilibrium the two phases have
equal -
(1) potential energy (2) intermolecular forces
(3) temperature (4) none of these
Q.79 What is the molality of ethyl alcohol (mol. Wt. = 46)
in aqueous solution which freezes at – 10°C ?
(Kf of H2O = 1.86 K molality –1 )
(1) 3.540 (2) 4.567
(3) 5.376 (4) 6.315
Q.80 Which solution would exhibit abnormal osmotic
pressure ?
(1) Aqueous solution of urea
(2) Aqueous solution of common salt
(3) Aqueous solution of glucose
(4) Aqueous solution of sucrose
Q.81 For a reaction of II order kinetics, t1/2 is -
(1) ∝ a (2) ∝ a –3
(3) ∝ a 2 (4) ∝ a –1
Q.82 For a first order reaction A –→ Product, the initial
concentration of A is 0.1 M and after 40 minute it
becomes 0.025 M. Calculate the rate of reaction at
reactant concentration of 0.01 M -
(1) 3.47 × 10 –4 M min –1
(2) 3.47 × 10 –5 M min –1
(3) 1.735 × 10 –6 M min –1
(4) None
Q.83 The pH of an acidic buffer mixture is -
(1) > 7
(2) < 7
(3) = 7
(4) depends upon Ka of acid
Q.84 Which solid is less soluble in 0.50 M HCl than in
water ?
(1) ZnCO3 (2) Hg2Cl2
(3) PbBr2 (4) AgI
Q.85 10 –2 mole of KOH is dissolved in 10 litre of
solution. The pH of the solution is -
(1) 12 (2) 2 (3) 3 (4) 11
Q.86 50% neutralization of a solution of formic acid
(Ka = 2 × 10 –4 ) with NaOH would result in a
solution having a hydrogen ion concentration of -
(1) 2 × 10 –4 (2) 3.7 (3) 2.7 (4) 1.85
Q.77 H2O ds fo|qr vi?kVu ds nkSjku] fufeZRk H2 o O2 dk
eksyj vuqikr gS -
(1) 2 : 1 (2) 1 : 2 (3) 1 : 3 (4) 1 : 1
Q.78 nzo ok"Ik lkE; ij nksuksa voLFkk,¡ ds leku gksrs gS -
(1) fLFkfrt ÅtkZ (2) vUr%v.kqd cy
(3) rki (4) buesa ls dksbZ ugha
Q.79 tyh; foy;u es ,fFky ,YdksgkWy (v.kqHkkj = 46) dh
eksyyrk D;k gS tks– 10°C ij terk gS \
(H2O dk Kf = 1.86 K molality –1 )
(1) 3.540 (2) 4.567
(3) 5.376 (4) 6.315
Q.80 fuEu esa ls dkSulk foYk;u vlkekU; ijklj.k nkc
n'kkZ,xk \
(1) ;wfj;k dk tyh; foy;u
(2) lkekU; yo.k dk tyh; foy;u
(3) Xywdkst dk tyh; foy;u
(4) lqØkst dk tyh; foy;u
Q.81 f}rh; dksfV xfrdh okyh vfHkfØ;k dk t1/2 gS -
(1) ∝ a (2) ∝ a –3
(3) ∝ a 2 (4) ∝ a –1
Q.82 ,d izFke dksfV vfHkfØ;k A –→ mRikn ds fy, A dh
izkjfEHkd lkUnzrk 0.1 M rFkk 40 feuV Ik'pkr~ 0.025 M
gSA 0.01 M dh vfHkdkjd lkUnzrk ij vfHkfØ;k dh nj
Kkr dhft, -
(1) 3.47 × 10 –4 M min –1
(2) 3.47 × 10 –5 M min –1
(3) 1.735 × 10 –6 M min –1
(4) dksbZ ugha
Q.83 ,d vEyh; cQj feJ.k dk pH gksrk gS -
(1) > 7
(2) < 7
(3) = 7
(4) vEy ds Ka ij fuHkZj djrk gS
Q.84 dkSulk Bksl ty dh vis{kk 0.50 M HCl esa de
foys; gksrk gS \
(1) ZnCO3 (2) Hg2Cl2
(3) PbBr2 (4) AgI
Q.85 10 –2 eksy KOH dks 10 yhVj foy;u esa ?kksyk tkrk
gSA foy;u dk pH gS -
(1) 12 (2) 2 (3) 3 (4) 11
Q.86 NaOH }kjk QkWfeZd vEy (Ka = 2 × 10 –4 ) dk 50%
mnklhuhdj.k ds ifj.kkeLo:Ik izkIr foy;u es
gkbMªkstu vk;u dh lkUnzrk gksrh gS -
(1) 2 × 10 –4 (2) 3.7 (3) 2.7 (4) 1.85
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