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Ionic Equilibrium PYQs - Last 10 Years

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ChemistryPhysical Chemistry2017-2026
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Practice 121 JEE Main Chemistry questions from Ionic Equilibrium. Use the year-wise and type-wise breakdown to prioritize recent PYQs, then continue into the question list below.

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2017-2026
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121
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Last 10 Years Ionic Equilibrium Questions

Showing 50 of 121 filtered questions.

1Ionic Equilibrium
\(25.0 \mathrm{~mL}\) of \(0.050 ~\mathrm{M} ~\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) is mixed with \(25.0 \mathrm{~mL}\) of \(0.020 ~\mathrm{M} ~\mathrm{NaF} . \mathrm{K}_{\mathrm{Sp}}\) of \(\mathrm{BaF}_{2}\) is $$0.5 \times 10^{-6...
INTEGER+4 / -12023
2Ionic Equilibrium
20 mL of \(0.1 ~\mathrm{M} ~\mathrm{NaOH}\) is added to \(50 \mathrm{~mL}\) of \(0.1 ~\mathrm{M}\) acetic acid solution. The \(\mathrm{pH}\) of the resulting solution is ___________ \(\times 10^{-2}\) (Nearest integer)
Given : $$\mathrm{pKa...
INTEGER+4 / -12023
3Ionic Equilibrium
An analyst wants to convert \(1 \mathrm{~L} \mathrm{~HCl}\) of \(\mathrm{pH}=1\) to a solution of \(\mathrm{HCl}\) of \(\mathrm{pH} ~2\). The volume of water needed to do this dilution is __________ \(\mathrm{mL}\). (Nearest integer)
INTEGER+4 / -12023
4Ionic Equilibrium
\(25 \mathrm{~mL}\) of silver nitrate solution (1M) is added dropwise to \(25 \mathrm{~mL}\) of potassium iodide \((1.05 \mathrm{M})\) solution. The ion(s) present in very small quantity in the solution is/are :
MCQ+4 / -12023
5Ionic Equilibrium
The solubility of AgCl will be maximum in which of the following?
MCQ+4 / -12022
6Ionic Equilibrium
If the solubility product of PbS is 8 \(\times\) 10\(-\)28, then the solubility of PbS in pure water at 298 K is x \(\times\) 10\(-\)16 mol L\(-\)1. The value of x is __________. (Nearest Integer)
[Given : \(\sqrt2\) = 1.41]
INTEGER+4 / -12022
7Ionic Equilibrium
\(200 \mathrm{~mL}\) of \(0.01 \,\mathrm{M} \,\mathrm{HCl}\) is mixed with \(400 \mathrm{~mL}\) of \(0.01 \,\mathrm{M} \,\mathrm{H}_{2} \mathrm{SO}_{4}\). The \(\mathrm{pH}\) of the mixture is _________.
Given: $$\log {2}=0.30, \log 3=0.48,...
MCQ+4 / -12022
8Ionic Equilibrium
The solubility product of a sparingly soluble salt A2X3 is 1.1 \(\times\) 10\(-\)23. If specific conductance of the solution is 3 \(\times\) 10\(-\)5 S m\(-\)1, the limiting molar conductivity of the solution is \(x \,\times\) 10\(-\)3 S m2...
INTEGER+4 / -12022
9Ionic Equilibrium
A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of \({{[C{H_3}C{H_2}CO{O^ - }]} \over {[C{H_3}C{H_2}COOH]}}\) required to make buffer is ___________.
Given : $${K_a}(C{H_3}C{H_2}COOH) ...
MCQ+4 / -12022
10Ionic Equilibrium
\(\mathrm{K}_{\mathrm{a}}\) for butyric acid \(\left(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{COOH}\right)\) is \(2 \times 10^{-5}\). The \(\mathrm{pH}\) of \(0.2 \,\mathrm{M}\) solution of butyric acid is __________ \(\times 10^{-1}\). (Neare...
INTEGER+4 / -12022
11Ionic Equilibrium
Given below are two statements : One is labelled as Assertion A and the other is labelled as Reason R
Assertion A : Permanganate titrations are not performed in presence of hydrochloric acid.
Reason R : Chlorine is formed as a consequence o...
MCQ+4 / -12022
12Ionic Equilibrium
pH value of 0.001 M NaOH solution is ____________.
INTEGER+4 / -12022
13Ionic Equilibrium
In the titration of \(\mathrm{KMnO}_{4}\) and oxalic acid in acidic medium, the change in oxidation number of carbon at the end point is ___________.
INTEGER+4 / -12022
14Ionic Equilibrium
At \(310 \mathrm{~K}\), the solubility of \(\mathrm{CaF}_{2}\) in water is \(2.34 \times 10^{-3} \mathrm{~g} / 100 \mathrm{~mL}\). The solubility product of \(\mathrm{CaF}_{2}\) is ____________ $$\times 10^{-8}(\mathrm{~mol} / \mathrm{L})^{...
INTEGER+4 / -12022
15Ionic Equilibrium
The plot of \(\mathrm{pH}\)-metric titration of weak base \(\mathrm{NH}_{4} \mathrm{OH}\) vs strong acid HCl looks like :
MCQ+4 / -12022
16Ionic Equilibrium
50 mL of 0.1 M CH3COOH is being titrated against 0.1 M NaOH. When 25 mL of NaOH has been added, the pH of the solution will be _____________ \(\times\) 10\(-\)2. (Nearest integer)
(Given : pKa (CH3COOH) = 4.76)
log 2 = 0.30
log 3 = 0.48
log...
INTEGER+4 / -12022
17Ionic Equilibrium
Class XII students were asked to prepare one litre of buffer solution of \(\mathrm{pH} \,8.26\) by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the student in \(0.2\, \mathrm{M}\) ammonia solution to make one ...
MCQ+4 / -12022
18Ionic Equilibrium
Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R :
Assertion A : The amphoteric nature of water is explained by using Lewis acid/base concept.
Reason R : Water acts as an acid with NH3 and ...
MCQ+4 / -12022
19Ionic Equilibrium
The Ksp for bismuth sulphide (Bi2S3) is 1.08 \(\times\) 10\(-\)73. The solubility of Bi2S3 in mol L\(-\)1 at 298 K is :
MCQ+4 / -12022
20Ionic Equilibrium
\(20 \mathrm{~mL}\) of \(0.1\, \mathrm{M} \,\mathrm{NH}_{4} \mathrm{OH}\) is mixed with \(40 \mathrm{~mL}\) of \(0.05 \mathrm{M} \mathrm{HCl}\). The \(\mathrm{pH}\) of the mixture is nearest to :
(Given : $$\mathrm{K}_{\mathrm{b}}\left(\mat...
MCQ+4 / -12022
21Ionic Equilibrium
\({K_{{a_1}}}\), \({K_{{a_2}}}\) and \({K_{{a_3}}}\) are the respective ionization constants for the following reactions (a), (b) and (c).
(a) $${H_2}{C_2}{O_4} \mathbin{\lower.3ex\hbox{$\buildrel\textstyle\rightarrow\over
{\smash{\leftarr...
MCQ+4 / -12022
22Ionic Equilibrium
A3B2 is a sparingly soluble salt of molar mass M (g mol\(-\)1) and solubility x g L\(-\)1. The solubility product satisfies \({K_{sp}} = a{\left( {{x \over M}} \right)^5}\). The value of a is _____________. (Integer answer)
INTEGER+4 / -12021
23Ionic Equilibrium
The pH of a solution obtained by mixing 50 mL of 1 M HCl and 30 mL of 1 M NaOH is x \(\times\) 10\(-\)4. The value of x is ____________. (Nearest integer) [log 2.5 = 0.3979]
INTEGER+4 / -12021
24Ionic Equilibrium
The pH of ammonium phosphate solution, if pka of phosphoric acid and pkb of ammonium hydroxide are 5.23 and 4.75 respectively, is ___________.
INTEGER+4 / -12021
25Ionic Equilibrium
Given below are two statements.Statement I : In the titration between strong acid and weak base methyl orange is suitable as an indicator.Statement II : For titration of acetic acid with NaOH phenolphthalein is not a suitable indicator.In t...
MCQ+4 / -12021
26Ionic Equilibrium
The solubility of AgCN in a buffer solution of pH = 3 is x. The value of x is : [Assume : No cyano complex is formed; Ksp(AgCN) = 2.2 \(\times\) 10\(-\)16 and Ka(HCN) = 6.2 \(\times\) 10\(-\)10]
MCQ+4 / -12021
27Ionic Equilibrium
The solubility of Ca(OH)2 in water is :[Given : The solubility product of Ca(OH)2 in water = 5.5 \(\times\) 10\(-\)6]
MCQ+4 / -12021
28Ionic Equilibrium
The solubility product of PbI2 is 8.0 \(\times\) 10\(-\)9. The solubility of lead iodide in 0.1 molar solution of lead nitrate is x \(\times\) 10\(-\)6. mol/L. The value of x is __________. (Rounded off to the nearest integer) [Given $$\sqr...
INTEGER+4 / -12021
29Ionic Equilibrium
A solution is 0.1 M in Cl\(-\) and 0.001 M in CrO\(_4^{2 - }\). Solid AgNO3 is gradually added to it. Assuming that the addition does not change in volume and Ksp(AgCl) = 1.7 \(\times\) 10\(-\)10 M2 and Ksp(Ag2CrO4) = 1.9 \(\times\) 10\(-\)...
MCQ+4 / -12021
30Ionic Equilibrium
The molar solubility of Zn(OH)2 in 0.1 M NaOH solution is x \(\times\) 10\(-\)18 M. The value of x is _________ (Nearest integer)(Given : The solubility product of Zn(OH)2 is 2 \(\times\) 10\(-\)20)
INTEGER+4 / -12021
31Ionic Equilibrium
In order to prepare a buffer solution of pH 5.74, sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is 1.0 M, the concentration of sodium acetate in the buffer is ___________ M. (Round off to the Near...
INTEGER+4 / -12021
32Ionic Equilibrium
Given below are two statements : One is labelled as Assertion A and the other labelled as reason RAssertion A : During the boiling of water having temporary hardness, Mg(HCO3)2 is converted to MgCO3.Reason R : The solubility product of Mg(O...
MCQ+4 / -12021
33Ionic Equilibrium
The solubility of CdSO4 in water is 8.0 \(\times\) 10\(-\)4 mol L\(-\)1. Its solubility in 0.01 M H2SO4 solution is __________ \(\times\) 10\(-\)6 mol L\(-\)1. (Round off to the Nearest Integer). (Assume that solubility is much less than 0....
INTEGER+4 / -12021
34Ionic Equilibrium
Which of the following compound CANNOT act as a Lewis base?
MCQ+4 / -12021
35Ionic Equilibrium
Two salts A2X and MX have the same value of solubility product of 4.0 \(\times\) 10\(-\)12. The ratio of their molar solubilities i.e. \({{S({A_2}X)} \over {S(MX)}}\) = __________. (Round off to the Nearest Integer)
INTEGER+4 / -12021
36Ionic Equilibrium
Sulphurous acid (H2SO3) has Ka1 = 1.7 \(\times\) 10\(-\)2 and Ka2 = 6.4 \(\times\) 10\(-\)8. The pH of 0.588 M H2SO3 is __________. (Round off to the Nearest Integer).
INTEGER+4 / -12021
37Ionic Equilibrium
The Ksp for the following dissociation is
1.6 × 10–5
\(PbC{l_{2(s)}} \leftrightharpoons Pb_{(aq)}^{2 + } + 2Cl_{(aq)}^ -\)
Which of the following choices is correct for
a mixture of 300 mL 0.134 M Pb(NO3)2 and
100 mL 0.4 M NaCl ?
MCQ+4 / -12020
38Ionic Equilibrium
The solubility product of Cr(OH)3 at 298 K is
6.0 × 10–31. The concentration of hydroxide ions
in a saturated solution of Cr(OH)3 will be :
MCQ+4 / -12020
39Ionic Equilibrium
The strength of an aqueous NaOH solution is most accurately determined by titrating : (Note : consider that
an appropriate indicator is used)
MCQ+4 / -12020
40Ionic Equilibrium
The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively :
MCQ+4 / -12020
41Ionic Equilibrium
For the following Assertion and Reason, the
correct option is :
Assertion : The pH of water increases with
increase in temperature.
Reason : The dissociation of water into H+ and
OH– is an exothermic reaction.
MCQ+4 / -12020
42Ionic Equilibrium
Two solutions, A and B, each of 100L was made by dissolving 4g of NaOH and 9.8 g of H2SO4 in water, respectively. The pH of the resultant solution obtained from mixing 40L of solution A and 10L of solution B is :
INTEGER+4 / -02020
43Ionic Equilibrium
3 g of acetic acid is added to 250 mL of 0.1 M HCL and the solution made up to 500 mL. To 20 mL
of this solutions \({1 \over 2}\) mL of 5 M NaOH is added. The pH of the solution is __________.
[Given : pKa of acetic acid = 4.75, molar mass ...
INTEGER+4 / -02020
44Ionic Equilibrium
Arrange the following solutions in the
decreasing order of pOH :
(A) 0.01 M HCl
(B) 0.01 M NaOH
(C) 0.01 M CH3COONa
(D) 0.01 M NaCl
MCQ+4 / -12020
45Ionic Equilibrium
If the solubility product of AB2 is 3.20 \(\times\) 10–11 M3,
then the solubility of AB2 in pure water is
_____ \(\times\) 10–4 mol L–1.
[Assuming that neither kind
of ion reacts with water]
INTEGER+4 / -02020
46Ionic Equilibrium
A soft drink was bottled with a partial pressure of CO2
of 3 bar over the liquid at room temperature.
The partial pressure of CO2
over the solution approaches a value of 30 bar when 44 g of CO2
is
dissolved in 1 kg of water at room tempe...
INTEGER+4 / -02020
47Ionic Equilibrium
An acidic buffer is obtained on mixing :
MCQ+4 / -12020
48Ionic Equilibrium
100 mL of 0.1 M HCl is taken in a beaker and
to it 100 mL of 0.1 M NaOH is added in steps
of 2 mL and the pH is continuously measured.
Which of the following graphs correctly depicts
the change in pH?
MCQ+4 / -12020
49Ionic Equilibrium
For the following Assertion and Reason, the
correct option is
Assertion (A): When Cu (II) and sulphide ions
are mixed, they react together
extremely quickly to give a
solid.
Reason (R): The equilibrium constant of
Cu2+(aq) + S2–(aq) ⇌ CuS(s...
MCQ+4 / -12020
50Ionic Equilibrium
20 mL of 0.1 M H2SO4 solution is added to 30 mL of of 0.2 M NH4OH solution. The pH of the resultant mixture is : [pkb of NH4OH = 4.7].
MCQ+4 / -12019