Ionic Equilibrium · Chemistry · NEET
MCQ (Single Correct Answer)
1
Which indicator is used in the titration of sodium hydroxide against oxalic acid and what is the colour change at the end point?
NEET 2024 (Re-Examination)
2
The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is:
(Given : Solubility product of AgCl = 10$$^{–10}$$)
NEET 2024 (Re-Examination)
3
An acidic buffer is prepared by mixing :
NEET 2023 Manipur
4
0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :
NEET 2022 Phase 2
5
The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is [Given pKa of CH3COOH = 4.57]
NEET 2022 Phase 1
6
The pKb of dimethyl amine and pKa of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethyl ammonium acetate solution is :
NEET 2021
7
Find out the solubility of Ni(OH)2 in 0.1M NaOH. Given that the ionic product of Ni(OH)2 is 2 $$ \times $$ 10-15.
NEET 2020 Phase 1
8
Conjugate base for Bronsted acids H2O and HF are :
NEET 2019
9
pH of a saturated solution of Ca(OH)2 is 9. The solubility product (Ksp) of Ca(OH)2 is :
NEET 2019
10
Which will make basic buffer?
NEET 2019
11
The solubility of BaSO4
in water is
2.42 × 10–3 g L–1 at 298 K. The value of its
solubility product (Ksp) will be (Given molar
mass of BaSO4
= 233 g mol–1)
NEET 2018
12
Following solutions were prepared by mixing
different volumes of NaOH and HCl of different
concentrations :
A. 60 mL $${M \over {10}}$$ HCl + 40 mL $${M \over {10}}$$ NaOH
B. 55 mL $${M \over {10}}$$ HCl + 45 mL $${M \over {10}}$$ NaOH
C. 75 mL $${M \over {5}}$$ HCl + 25 mL $${M \over {5}}$$ NaOH
D. 100 mL $${M \over {10}}$$ HCl + 100 mL $${M \over {10}}$$ NaOH
pH of which one of them will be equal to 1?
A. 60 mL $${M \over {10}}$$ HCl + 40 mL $${M \over {10}}$$ NaOH
B. 55 mL $${M \over {10}}$$ HCl + 45 mL $${M \over {10}}$$ NaOH
C. 75 mL $${M \over {5}}$$ HCl + 25 mL $${M \over {5}}$$ NaOH
D. 100 mL $${M \over {10}}$$ HCl + 100 mL $${M \over {10}}$$ NaOH
pH of which one of them will be equal to 1?
NEET 2018
13
Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.2 $$ \times $$ 10$$-$$4 mol L$$-$$1. Solubility product of Ag2C2O4 is
NEET 2017
14
The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5N+H) ina 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 $$ \times $$ 10$$-$$9) is
NEET 2016 Phase 2
15
The solubility of AgCl(s) with solubility product 1.6 $$ \times $$ 10$$-$$10 in 0.1 M NaCl solution would be
NEET 2016 Phase 2
16
Which of the following fluro-compounds is most likely to behave as a Lewis base ?
NEET 2016 Phase 2
17
MY and NY3, two nearly insoluble salts, have the same Ksp values of 6.2 $$ \times $$ 10$$-$$13 at room temperature. Which statement would be true in regard to MY and NY3?
NEET 2016 Phase 1
18
Which one of the following pairs of solution is not an acidic buffer ?
AIPMT 2015
19
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
AIPMT 2015
20
The Ksp of Ag2CrO4, AgCl, AgBr and Agl are respectively, 1.1 $$ \times $$ 10$$-$$12, 1.8 $$ \times $$ 10$$-$$10, 5.0 $$ \times $$ 10$$-$$13, 8.3 $$ \times $$ 10$$-$$17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na2CrO4?
AIPMT 2015 Cancelled Paper
21
Which of the following salts will give highest pH in water?
AIPMT 2014
22
The dissociation constant of weak acid is 1 $$ \times $$ 10$$-$$4. In order to prepare a buffer solution with a pH = 5, the [Salt]/[Acid] ratio should be
NEET 2013 (Karnataka)
23
The values of Ksp of CaCO3 and CaC2O4 are 4.7 $$ \times $$ 10$$-$$9 and 1.3 $$ \times $$ $$-$$9 respectively at 25oC. If the mixture of these two is washed with water, what is the concentration of Ca2+ ions in water ?
NEET 2013 (Karnataka)
24
At 100oC the Kw of water is 55 times its value at 25oC. What will be the pH of neutral solution? (log 55 = 1.74)
NEET 2013 (Karnataka)
25
Accumulation of lactic acid (HC3H5O3), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociates. The value of dissociation constant, Ka, for this acid will be
NEET 2013 (Karnataka)
26
KMnO4 can be prepared from K2MnO4 as per the reaction,
3MnO42$$-$$ + 2H2O $$\rightleftharpoons$$ 2MnO4$$-$$ + MnO2 + 4OH$$-$$
The reaction can go to completion by removing OH$$-$$ ions by adding
3MnO42$$-$$ + 2H2O $$\rightleftharpoons$$ 2MnO4$$-$$ + MnO2 + 4OH$$-$$
The reaction can go to completion by removing OH$$-$$ ions by adding
NEET 2013
27
Which of these is least likely to act as a lewis base ?
NEET 2013
28
Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value ?
AIPMT 2012 Prelims
29
Buffer solutions have constant acidity and alkalinity because
AIPMT 2012 Prelims
30
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is
AIPMT 2012 Prelims
31
In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl$$-$$ concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium ?
(Ksp for AgCl = 1.8 $$ \times $$ 10$$-$$10, Ksp for PbCl2 = 1.7 $$ \times $$ 10$$-$$5)
(Ksp for AgCl = 1.8 $$ \times $$ 10$$-$$10, Ksp for PbCl2 = 1.7 $$ \times $$ 10$$-$$5)
AIPMT 2011 Mains
32
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of NH+4 is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 $$ \times $$ 10$$-$$5, what is the pH of this solution? (log 2.7 = 0.43)
AIPMT 2011 Prelims
33
Which of the following is least likely to behave as Lewis base?
AIPMT 2011 Prelims
34
If pH of a saturated solution of Ba(OH)2 is 12, the value of its Ksp is
AIPMT 2010 Prelims
35
In a buffer solution containing equal concentration of B$$-$$ and HB, the Kb for B$$-$$ is 10$$-$$10. The pH of buffer solution is
AIPMT 2010 Prelims
36
What is [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.10 M in CH3COOH? Ka for CH3COOH = 1.8 $$ \times $$ 10$$-$$5
AIPMT 2010 Prelims
37
The ionization constant of ammonium hydroxide is 1.77 $$ \times $$ 10$$-$$5 at 298 K. Hydrolysis constant of ammonium chloride is
AIPMT 2009
38
What is the [OH$$-$$] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)2?
AIPMT 2009
39
Which of the following molecules acts as a Lewis acid?
AIPMT 2009
40
Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
AIPMT 2008
41
A weak acid, HA, has a Ka of 1.00 $$ \times $$ 10$$-$$5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to
AIPMT 2007
42
Calculate the pOH of a solution at 25oC that contains 1 $$ \times $$ 10$$-$$10 M of hydronium ions, i.e. H3O+.
AIPMT 2007
43
Which of the following pairs constitutes a buffer?
AIPMT 2006
44
The hydrogen ion concentration of a 10$$-$$8 M, HCl aqueous solution at 298 K (Kw = 10$$-$$14) is
AIPMT 2006
45
At 25oC, the dissociation constant of a base, BOH, is 1.0 $$ \times $$ 10$$-$$12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be
AIPMT 2005
46
H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
AIPMT 2005
47
The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In$$-$$) forms of the indicator by the expression
AIPMT 2004
48
The solubility product of a sparingly soluble salt AX2 is 3.2 $$ \times $$ 10$$-$$11. Its solubility (in moles/L) is
AIPMT 2004
49
The solubility product of AgI at 25oC is 1.0 $$ \times $$ 10$$-$$16 mol2 L$$-$$2. The solubility of AgI in 10$$-$$4 N solution of KI at 25oC is approximately (in mol L$$-$$1
AIPMT 2003
50
Which has highest pH?
AIPMT 2002
51
Solubility of MX2 type electrolytes is 0.5 $$ \times $$ 10$$-$$4 mole/lit., then find out Ksp of electrolytes.
AIPMT 2002
52
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. Then find out pKb of NH4OH
AIPMT 2002
53
Ionisation constant of CH3COOH is 1.7 $$ \times $$ 10$$-$$5 and concentration of H+ ions is 3.4 $$ \times $$ 10$$-$$4. Then find out initial concentration of CH3COOH molecules.
AIPMT 2001
54
In HS$$-$$, I$$-$$, R $$-$$ NH2, NH3 order of proton accepting tendency will be
AIPMT 2001
55
Solubility of M2S salt is 3.5 $$ \times $$ 10$$-$$6 then find out solubility product.
AIPMT 2001
56
Correct relation between dissociation constants of a dibasic acid is
AIPMT 2001
57
Which statement is wrong about pH and H+?
AIPMT 2000
58
Conjugate acid of NH2$$-$$ is
AIPMT 2000