Q 1.
When HCl (g) is passed through a saturated solution of common salt, pure NaCl is
precipitated because:
(a) HCl is highly soluble in water
(b) the ionic product [ Na+] [Cl-] exceeds its solubiity product  K sp. 
(c) the Ksp of NaCl is lowered by the presence of Cl- ions
(d) due to unknown reason
Q 2. An acetic acid and sodium acetate buffer has pH = 5.36. The ratio of concentrations
[OAC]/[HOAC]
will be: (given pKa of CH3COOH = 4.76)
(a) 6:1
(b) 4:3
(c) 1:1
(d) 4:1
Q 3.
A certain weak acids has a dissociation constant of 1.0 × 10-4 The equilibrium constant
for its reaction with a strong base is :
(a) 1.0 × 10
(b) 1.0 × 10-10
(c) 1.0 × 1010
(d) 1.1 × 1014
Q 4.
Which of the following buffers have a pH greater than 7 ?
(a) NaHCO3 + Na2CO3
(b) NH3 + (NH4)2 SO4
(c) Na3PO4 + NaH2PO4
(d) all of the above
Q 5.
Which of the following is correct ?
(a) Ka (weak acid) : Kb (conjugate weak base) = Kw
(b) Ka (strong add) . Kb (conjugate weak base) = Kw
(c) Ka (weak acid) . Kb (weak base) = Kw
(d) Ka (weak add). Kb (conjugate strong base) = Kw
Q 6. The pH of a solution is 5.0. Its hydrogen ion concentration Is decreased 100 times, the
solution then
will be:
(a) more acidic
(b) basic
(c) neutral
(d) of the same
acidity
Q 7.
The solubility products of MA, MB, MC and MD are 1.8 × 10-10, 4 × 10-3, 4 × 10-5 and 6
× 10-5 respectively, If a 0.01 M solution of MX is added dropwise to a mixture
containing A, B, C, and D ions, then the one to be precipitated first will be:
(a) MA
(b) MB
(c) MC
(d) MD
Q 8.
Two weak solutions are isohydric when their:
(a) H+ concentrations are same before mixing
(b) H+ concentrations are same before and after mixing
(c) Degree of dissociation are the same
(d) Chemical properties are the same
Q 9.
The solubility of X2X3 is y mol dm-3 Its solubility product is :
(a) 6y4
(b) 64y4
(c) 36y5
(d) 108y5
Q 10. pH of 10-10 molar HCl solution at 25C is approximately:
(a) 10
(b) 7
(c) 1
(d) 14
Q 11. Consider the following:
(i) NaCl
(ii) NH4Cl
(iii) NaCN
(iv) HCl
The correct sequence of increasing order of pH of 0.1M solution of these compounds will
be:
(a) (iv) < (iii) < (ii) < (i)
(b) (iv) < (i) < (ii) < (iii)
(c) (iv) <(ii) < (i) < (iii)
(d) (iii) < (ii) < (i) < (iv)
Q 12. Given Ka1, Ka2 for H2S = 1.1 × 10-21 M3. 1L solution of 0.1 M H2S having [H+] = 0.1 M
contains S2- ions eq to:
(a) 6.62 × 103
(b) 6.62 × 104
(c) 6.62 × 105
(d) 6.62 × 108
Q 13.
va1ue of H3O+ at 298 K will be :
(a) -1.74
(b) -14
pKa
(c) 14
(d) - 2.6
Q 14. Which of the, following solutions containing weak acid and salt of its conjugate base has
maximum buffer capacity ?
(a) [ Salt] > [Acid]
(b) [ Salt] > [Acid]
(c) [ Salt] = [Acid]
(d) Does not depend upon [salt] and [acid]
Q 15. The pH values 1 M solutions of CH3COONa (I), CH3COOH (II), CH3COONH4 (III) and
NaOH (IV) will be in the order:
(a) IV > III > I > II
(b) IV > I > III > II
(c) II > III > I > IV
(d) I > II > III > IV
Q 16. What will be the H+ concentration in a solution prepared by mixing 50 mL of 0.20M
NaCl, 25 mL of 0.10M NaOH and 25 mL of 0.30M HCl.
(a) 0.5 M
(b) 0.05 M
(c) 0.02 M
(d) 0.10 M
Q 17. A buffer solution contains 0.1 M each of acetic acid and sodium acetate. The pH of the
buffer solution is : (pKa(CH3COOH) = 4.75) :
(a) 4.75
(b) 5.75
(c) 6.75
(d) 9.25
Q 18. Which of the following mixtures constitute of buffer?
(a) NaCl + HCl
(b) NH4Cl + (NH4)2SO4
(c) Na2CO3 + NaHCO3
(d) All of these
Q 19. CaCO3 and BaCO3 have solubiity product values 1 × 10-8 and 5 × 10-9 respectively, if
water is shaken up with both solids till equilibrium is reached, the concentration of CO32 
ions will be:
(a) 1.5 × 10-8
(b) 1.225 × 10-4
(c) 2.25 × 10-9
(d) none of these
Q 20. A buffer solution is used in the:
(a) preparation of chrome alum
analysis
(c) precipitation of Zn(OH)2 from ZnSO4
water
(b) removal of PO43 ions in qualitative
(d) determination of the ionic product of
Q 21. Which one of the following is not an acid salt?
(a) NaHSO3
(b) Na2HPO3
(c) NaHC2O4
(d) NaHSO4
Q 22. On adding AlCl3 Aid to water:
(a) the ionization of water increases
(b) the ionization of water decreases
(c) the ionization of water remains constant
(d) the ionic product of water increases
Q 23. Which of the following will occur if a 1.0 M solution of a weak acid is diluted to 0.01
Mat constant temperature?
(a) [H+] will decrease to 0.01 M
(b) pH will decrease by two units
(c) Ka will increase
(d) Percentage ionization will increase
Q 24. Choose the correct statement:
(a) All Lewis acids are Bronsted acids too
(b) All Bronsted bases are Lewis bases
(c) pH value of water increases with rise in temperature
(d) None of the above
Q 25. Which of the following will not hydrolyse in an aqueous solution?
(a) A salt of a strong acid and a strong base
(b) A salt of a strong acid and a weak base
(c) A salt of a weak acid and a strong base
(d) A salt of a weak acid and a weak base
Q 26. Which of the following mixtures constitute a buffer ?
(a) Na2CO3 + HCl
(b) NaOH + NaCl
(c) NH3 + CH3COONH4
(d) None of the above
Q 27. Choose the correct statement:
(a) pH value decreases when NaCl is added to water,
(b) Ionic product of water is 1 × 10-8 at 295 K
(c) All Arrhenius acids are Bronsted acid also
(d) pH of acidic solution is greater than seven
Q 28. pH of solution of 25°C is 2. if the pH is to be doubled then the hydronium ion
concentration of the solution should be:
(a) halved
(b) increased to. 100 times
(c) doubled
(d) decreased to 100 times
Q 29. The effectiveness of a buffer is measured in terms of:
(a) buffer action
(b) buffer capacity
(c) hydrolysis constant
(d) pKa and pKb
Q 30. The pH value of gastric juice in stomach is about 1.8 and that in small intestine is 7.8.
The pKa value of Aspirin is 3.5. Aspirin will be:
(a) completely ionised in small intestine and In the stomach
(b) unionised in small intestine as well as in stomach
(c) ionised in small intestine and almost unionised in stomach
(d) ionised in stomach and almost unionised in intestine
Q 31. Which one of the following mixtures will give a solution with pH greater than 7 ?
(a) 50 mL of 0.1 M HCl + 50 mL of 0.2 M NaCl
(b) 50 mL of 0.1 M HCl + 50 mL of 0.1 M CH3COONa
(c) 50 mL of 0.1 M CH3COONa + 50 mL of 0.1 M NaOH
(d) 50 mL of 0.2 M H2SO4 50 mL of 0.3 M NaOH
Q 32. Which of the following will suppress the ionization of phthalic acid in an aqueous
solution ?
(a) KCl
(b) KNO3
(c) HNO3
(d) NaOH
Q 33. The dissociation constants of monobasic acids A, B, C and D are 6 × 10-4 5 × 10-5 3.6 ×
10-6 and 7 × 10-10 respectively. The pH values of their 0.1 molar aqueous solutions are in
the order:
(a)A < B < C < D
(b) A > B > C > D
(c) A = B = C = D
(d) A > B < C > D
Q 34. Choose the incorrect statement:
(a) The pH of 10 M NaOH solution could not be greater than 14
(b) The pH of 0.01 M NaOH is 12
(c) AlCl3 is a Lewis acid as it can donate electron
(d) AgCl is more soluble in very conc. NaCl solution than in pure water
Q 35. In which of the following pairs of solutions is there no effect on the pH upon dilution ?
(a) 0.1 M HCl and 0.01 NaOH
(b) 0.1 MKCl and 0.1 M HCl
(c) 0.1 M Na2HPO4 and 0.1 M Na2HPO4
(d) All of the above
Answers
1.
8.
15.
22.
29.
b
a
b
a
b
2.
9.
16.
23.
30.
d
d
b
d
c
3.
10.
17.
24.
31.
c
b
a
b
c
4.
11.
18.
25.
32.
a
c
c
a
c
5.
12.
19.
26.
33.
a
a
b
a
a
6.
13.
20.
27.
34.
c
a
b
c
c
7.
14.
21
28
35.
a
c
b
d
c