Ionic Equilibrium PYQs - Last 10 Years
NEET / Chemistry / Physical Chemistry / 19 recent questions
ChemistryPhysical Chemistry2017-2026
Practice 19 NEET 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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Last 10 Years Ionic Equilibrium Questions
Showing 19 of 19 filtered questions.
1Ionic Equilibrum
\(\text { The correct order of solubility of the given salts in water at } 298 \mathrm{~K} \text { is }\)
$$ \begin{array}{|l|l|} \hline \text { Salt } & \mathbf{K}_{\text {sp }} \text { at } \mathbf{2 9 8} \text { K } \\ \hline \mathrm{A...
$$ \begin{array}{|l|l|} \hline \text { Salt } & \mathbf{K}_{\text {sp }} \text { at } \mathbf{2 9 8} \text { K } \\ \hline \mathrm{A...
MCQ+4 / -12026
2Ionic Equilibrum
Phenolphthalein is used as an indicator for the titration of sodium hydroxide solution against a standard solution of oxalic acid. The colour change that is observed at an alkaline pH close to the equivalence point during this titration is:...
MCQ+4 / -12026
3Ionic Equilibrum
At 298 K , a certain buffer solution contains equal concentrations of $\mathrm{X}^{-}$and $\mathrm{HX}, \mathrm{K}_{\mathrm{b}}$ for $\mathrm{X}^{-}$is $10^{-10}$. What is the pH of this buffer solution?
MCQ+4 / -12026
4Ionic Equilibrum
In a qualitative analysis, $\mathrm{Bi}^{3+}$ is detected by appearance of precipitate of $\mathrm{BiO}(\mathrm{OH})(\mathrm{s})$. Calculate pH when the following equilibrium exists at 298 K .
$$ \mathrm{BiO}(\mathrm{OH})(\mathrm{s}) \right...
$$ \mathrm{BiO}(\mathrm{OH})(\mathrm{s}) \right...
MCQ+4 / -12026
5Ionic Equilibrum
Phosphoric acid ionizes in three steps with their ionization constant values $K_{a_1}, K_{a_2}$ and $K_{a_3}$, respectively, while $K$ is the overall ionization constant. Which of the following statements are true?
A. $\quad \log \mathrm{K}...
A. $\quad \log \mathrm{K}...
MCQ+4 / -12025
6Ionic Equilibrum
If the molar conductivity $\left(\Lambda_{\mathrm{m}}\right)$ of a $0.050 \mathrm{~mol} \mathrm{~L}^{-1}$ solution of a monobasic weak acid is $90 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, its extent (degree) of dissociation will be
[...
[...
MCQ+4 / -12025
7Ionic Equilibrum
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\(^{–10}\))
(Given : Solubility product of AgCl = 10\(^{–10}\))
MCQ+4 / -12024
8Ionic Equilibrum
Which indicator is used in the titration of sodium hydroxide against oxalic acid and what is the colour change at the end point?
MCQ+4 / -12024
9Ionic Equilibrum
An acidic buffer is prepared by mixing :
MCQ+4 / -12023
10Ionic Equilibrum
0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :
MCQ+4 / -12022
11Ionic Equilibrum
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]
MCQ+4 / -12022
12Ionic Equilibrum
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 :
MCQ+4 / -12021
13Ionic Equilibrum
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.
MCQ+4 / -12020
14Ionic Equilibrum
pH of a saturated solution of Ca(OH)2 is 9. The solubility product (Ksp) of Ca(OH)2 is :
MCQ+4 / -12019
15Ionic Equilibrum
Which will make basic buffer?
MCQ+4 / -12019
16Ionic Equilibrum
Conjugate base for Bronsted acids H2O and HF are :
MCQ+4 / -12019
17Ionic Equilibrum
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. 7...
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. 7...
MCQ+4 / -12018
18Ionic Equilibrum
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)
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)
MCQ+4 / -12018
19Ionic Equilibrum
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
MCQ+4 / -12017