Equilibrium
112 JEE Chemistry previous year questions on Equilibrium — options free on every question; 11 include the answer & explanation free, the rest unlock with PYQ Pass.
A vessel at 1000 K contains carbon dioxide with a pressure of 0.5 atm. Some of carbon dioxide is converted into carbon monoxide on addition of graphite. If total pressure at equilibrium is 0.8 atm, then \({\mathrm{K}}_{\mathrm{p}}\) is
[JEE Main 2025, 22 Jan (Shift 1)]
1.8 atm
\({\mathrm{CO}}_{2}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{s}\right)⇌2\mathrm{CO}\left(\mathrm{g}\right)\\ 0.5-\\ 0.5-\mathrm{x}2\mathrm{x}\\ {\mathrm{P}}_{\mathrm{T}}=0.5+\mathrm{x}=0.8\\ \mathrm{x}=0.8-0.5=0.3\\ {\mathrm{K}}_{\mathrm{P}}=\frac{{(0.6)}^{2}}{0.2}=1.8\)
If equal volumes of \({\mathrm{AB}}_{2}\) and XY (both are salts) aqueous solutions are mixed, which of the following combination will give a precipitate of \({\mathrm{AY}}_{2}\) at \(300\) K ?
\((\mathrm{Given}{\mathrm{K}}_{\mathrm{sp}}(\mathrm{at}300\mathrm{K})\)\(\mathrm{for}{\mathrm{AY}}_{2}=5.2\times {10}^{-7})\)
[JEE Main 2025, 2 Apr (Shift 1)]
\(2.0\times {10}^{-2}\mathrm{M}{\mathrm{AB}}_{2},2.0\times {10}^{-2}\mathrm{M}\mathrm{XY}\)
For precipitation of AY₂:
Ksp = [A²⁺][Y⁻]² = 5.2 × 10⁻⁷
Check option C:
[A²⁺] = 2.0 × 10⁻²
[Y⁻] = 2.0 × 10⁻²
Ion product = 8.0 × 10⁻⁶ > Ksp
⇒ Precipitation occurs
A weak acid HA has degree of dissociation x. Which option gives the correct expression of (\(\mathrm{pH}-{\mathrm{pk}}_{\mathrm{b}}\))
(Memory-based Question 28/ Jan/25 morning shift )
\(\log \left(\frac{x}{1-x}\right)\)
\(\mathrm{HA}(\mathrm{aq})⇌{\mathrm{H}}^{+}(\mathrm{aq})+{\mathrm{A}}^{-}(\mathrm{aq})\\ \mathrm{C}--\\ \mathrm{C}-\mathrm{Cx}\mathrm{Cx}\mathrm{Cx}\\ {\mathrm{K}}_{\mathrm{a}}=\frac{\left[{\mathrm{H}}^{+}\right]\left[{\mathrm{A}}^{-}\right]}{\mathrm{HA}}=\frac{\mathrm{Cα}\times \mathrm{Cα}}{\mathrm{C}(1-\mathrm{x})}\\ \left[{\mathrm{H}}^{+}\right]=\mathrm{Cα}=\frac{{\mathrm{K}}_{\mathrm{a}}(1-\mathrm{x})}{\mathrm{x}}\\ \mathrm{pH}=-\log \left[{\mathrm{H}}^{+}\right]=-\log \frac{\left[{\mathrm{K}}_{\mathrm{a}}(1-\mathrm{x})\right]}{\mathrm{x}}\\ \mathrm{pH}={\mathrm{PK}}_{\mathrm{a}}-\log \frac{(1-\mathrm{x})}{\mathrm{x}}\\ \mathrm{pH}-{\mathrm{PK}}_{\mathrm{a}}=\log \frac{\mathrm{x}}{1-\mathrm{x}}\)
An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would
(Given log 2 = 0.30)
[JEE Main 2025, 7 Apr (Shift 1)]
increase to 1.3
Initial pH = 1
[H⁺] = 10⁻¹ M
After adding equal volume of water → concentration becomes half
New [H⁺] = (10⁻¹) / 2
pH = −log(10⁻¹ / 2)
pH = −[log(10⁻¹) − log(2)]
pH = −[−1 − 0.30]
pH = 1 + 0.30
pH = 1.30
The pH of a \(0.01\) M weak acid \(\mathrm{HX}\left({\mathrm{K}}_{\mathrm{a}}=4\times {10}^{-10}\right)\) is found to be 5 . Now the acid solution is diluted with excess of water so that the pH of the solution changes to \(6\) . The new concentration of the diluted weak acid is given as \(x\times {10}^{-4}\mathrm{M}\). The value of x is ______ (nearest integer)
25
\(pH=6\ [{H}^{+}]={10}^{−6}\)
\([{H}^{+}]={10}^{−6}=\sqrt{{K}_{a}C}\)
\({10}^{−6}=\sqrt{4\times {10}^{−10}\times C}\)
\(\frac{{10}^{−12}}{4\times {10}^{−10}}=C\)
\(0.25\times {10}^{−2}=C\)
\(25\times {10}^{−4}=C\ ∴x=25\)
What will be the effect on pH of water when it is heated
Decrease
As water is heated degree of ionisation increases
[H+] ion concentration increases pH decreases.
\({\mathrm{CO}}_{2}(\mathrm{g})+\mathrm{C}(\mathrm{s})⇌2\mathrm{CO}(\mathrm{g})\)
If initial pressure of \({\mathrm{CO}}_{2}\)is 0.6 atm and after equilibrium is established, total pressure is 0/8 atm. Then, find \({\mathrm{K}}_{\mathrm{p}}\).
(Memory Based JEE Mains 22/01/2025, Shift -1)
0.4
\({\mathrm{CO}}_{2}(\mathrm{g})+\mathrm{C}(\mathrm{s})⇌2\mathrm{CO}(\mathrm{g})\\ \mathrm{At}\mathrm{t}=0{\mathrm{p}}_{0}--\\ \mathrm{At}\mathrm{t}=\mathrm{teq}{\mathrm{p}}_{0}-\mathrm{p}2\mathrm{p}\\ {\mathrm{P}}_{\mathrm{T}}={\mathrm{P}}_{0}+\mathrm{P}\Rightarrow \mathrm{p}=(0.8-0.6)=0.2,{\mathrm{p}}_{\mathrm{CO}}=0.4\mathrm{and}{\mathrm{p}}_{{\mathrm{CO}}_{2}}=0.4\\ {\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{p}}_{{(\mathrm{CO})}^{2}}}{{\mathrm{p}}_{{\mathrm{CO}}_{2}}}=\frac{{(0.4)}^{2}}{0.4}=0.4\).
A weak acid HA has degree of dissociation x. Which option gives the correct expression of (\(\mathrm{pH}-{\mathrm{pk}}_{\mathrm{b}}\))
(Memory-based Question 28/ Jan/25 morning shift )
\(\log \left(\frac{x}{1-x}\right)\)
\(\mathrm{HA}(\mathrm{aq})⇌{\mathrm{H}}^{+}(\mathrm{aq})+{\mathrm{A}}^{-}(\mathrm{aq})\\ \mathrm{C}--\\ \mathrm{C}-\mathrm{Cx}\mathrm{Cx}\mathrm{Cx}\\ {\mathrm{K}}_{\mathrm{a}}=\frac{\left[{\mathrm{H}}^{+}\right]\left[{\mathrm{A}}^{-}\right]}{\mathrm{HA}}=\frac{\mathrm{Cα}\times \mathrm{Cα}}{\mathrm{C}(1-\mathrm{x})}\\ \left[{\mathrm{H}}^{+}\right]=\mathrm{Cα}=\frac{{\mathrm{K}}_{\mathrm{a}}(1-\mathrm{x})}{\mathrm{x}}\\ \mathrm{pH}=-\log \left[{\mathrm{H}}^{+}\right]=-\log \frac{\left[{\mathrm{K}}_{\mathrm{a}}(1-\mathrm{x})\right]}{\mathrm{x}}\\ \mathrm{pH}={\mathrm{PK}}_{\mathrm{a}}-\log \frac{(1-\mathrm{x})}{\mathrm{x}}\\ \mathrm{pH}-{\mathrm{PK}}_{\mathrm{a}}=\log \frac{\mathrm{x}}{1-\mathrm{x}}\)
For a reaction, \({N}_{2}{O}_{5(g)}\to 2N{O}_{2(g)}+\frac{1}{2}{O}_{2(g)}\) in a constant volume container, no products were present initially. The final pressure of the system when 50 % of reaction gets completed is
[JEE Main 2025, 24 Jan (Shift 1)]
7/4 times of initial pressure
\({N}_{2}{O}_{5}(g)\to 2N{O}_{2}(g)+\frac{1}{2}{O}_{2}(g)\)
Let the initial pressure of \({N}_{2}{O}_{5}\) be \({P}_{0}\).
Initial moles: Only \({N}_{2}{O}_{5}\) is present \(\to {n}_{0}\) \(={P}_{0}\) (as per ideal gas law).
Let x be the fraction of reaction completed.
For 1 mole of \({N}_{2}{O}_{5}\) decomposing:
2 moles of \(N{O}_{2}\) are formed.
0.5 moles of \({O}_{2}\) are formed.
Given that 50 % of the reaction is completed (x =0.5):
\({N}_{2}{O}_{5}\) decomposed: \(0.5{P}_{0}\)
\(N{O}_{2}\) formed: \(2\times 0.5{P}_{0}={P}_{0}\)
\({O}_{2}\) formed: \(0.5\times 0.5{P}_{0}=0.25{P}_{0}\)
Remaining \({N}_{2}{O}_{5}:{P}_{0}-0.5{P}_{0}=0.5{P}_{0}\)
\({P}_{\text{final }}={P}_{{N}_{2}{O}_{5}}+{P}_{N{O}_{2}}+{P}_{{O}_{2}}\)
\({P}_{\text{final }}=0.5{P}_{0}+{P}_{0}+0.25{P}_{0}\)\(=1.75{P}_{0}=\frac{7}{4}{P}_{0}\)
The solubility of barium iodate in an aqueous solution prepared by mixing 200 mL of 0.010 M barium nitrate with 100 mL of 0.10 M sodium iodate is \(X \times 10^{-6} mol dm ^{-3}\). The value of \(X\) is________ .
Use: Solubility product constant ( \(K_{ sp }\) ) of barium iodate \(=1.58 \times 10^{-9}\)
[JEE Advanced 2025, Paper-2]
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A vessel at 1000 K contains carbon dioxide with a pressure of 0.5 atm. Some of carbon dioxide is converted into carbon monoxide on addition of graphite. If total pressure at equilibrium is 0.8 atm, then \({\mathrm{K}}_{\mathrm{p}}\)is
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A weak acid HA has degree of dissociation x. Which option gives the correct expression of ( \(pH-\) \(\left.p{K}_{a}\right)\) ?
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Le-Chatelier’s principle is not applicable to
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The molar solubility(s) of zirconium phosphate with molecular formula \({\left(\mathrm{Zr}\right)}_{3}{\left(P{O}_{4}\right)}_{4}\) is given by relation
[JEE Main 2025, 22 Jan (Shift 2)]
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Given below are two statements :
Statement 1: On passing \({\mathrm{HCl}}_{(\mathrm{g})}\) through a saturated solution of \({\mathrm{BaCl}}_{2}\), at room temperature white turbidity appears
Statement II : When \(\mathrm{HCl}\) gas is passed through a saturated solution of \(\mathrm{NaCl}\), sodium chloride is precipitated due to common ion effect.
In the light of the above statements, choose the most appropriate answer from the options given below:
[JEE Main 2024, 05 Apr (Shift 2)]
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Given below are two statements :
Statement 1: On passing \({\mathrm{HCl}}_{(\mathrm{g})}\) through a saturated solution of \({\mathrm{BaCl}}_{2}\), at room temperature white turbidity appears
Statement II : When \(\mathrm{HCl}\) gas is passed through a saturated solution of \(\mathrm{NaCl}\), sodium chloride is precipitated due to common ion effect.
In the light of the above statements, choose the most appropriate answer from the options given below:
[JEE Main 2024, 05 Apr (Shift 2)]
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Consider the equilibrium
\(CO(g)+3{H}_{2}(g)⇌C{H}_{4}(g)+{H}_{2}O(g)\)
If the pressure applied over the system increases by two fold at constant temperature then
(A) Concentration of reactants and products increases.
(B) Equilibrium will shift in forward direction.
(C) Equilibrium constant increases since concentration of products increases.
(D) Equilibrium constant remains unchanged as concentration of reactants and products remain same.
Choose the correct answer from the options given below.
[JEE Main 2023, 24 Jan (Shift 1)]
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Ice and water are placed in a closed container at a pressure at 1 atm and temperature 273.15 K .
If the pressure of the container increases 2 times and the temperature is kept constant, than identify the correct observation from the following.
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\(x\mathrm{mg}\) of \(\mathrm{Mg}(\mathrm{OH}{)}_{2}\) (molar mass = 58) is required to be dissolved in 1.0 L of water to produce a pH of 10.0 at 298 K . The value of x is ______ mg. (Nearest integer)
(Given : \(\mathrm{Mg}(\mathrm{OH}{)}_{2}\) is assumed to dissociate completely in \({\mathrm{H}}_{2}\mathrm{O}\) )
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In the following system, \({\mathrm{PCl}}_{5}(\mathrm{g})⇌{\mathrm{PCl}}_{3}(\mathrm{g})+{\mathrm{Cl}}_{2}(\mathrm{g})\) at equilibrium, upon addition of xenon gas at constant T & P, the concentration of
[JEE Main 2025, 3 Apr (Shift 1)]
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What will be the effect on pH of water when it is heated
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In the following system, \({\mathrm{PCl}}_{5}(\mathrm{g})⇌{\mathrm{PCl}}_{3}(\mathrm{g})+{\mathrm{Cl}}_{2}(\mathrm{g})\) at equilibrium, upon addition of xenon gas at constant T & P, the concentration of
[JEE Main 2025, 3 Apr (Shift 1)]
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For a sparingly soluble salt \(A{B}_{2}\), the equilibrium concentrations of \({A}^{2+}\) ions and \({B}^{-}\)ions are \(1.2\times {10}^{-4}M\) and \(0.24\times {10}^{-3}M\), respectively. The solubility product of \(A{B}_{2}\) is :
[JEE Main 2024, 9 Apr (Shift 2)]
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pH of water is 7 at 25 degree celsius. If water is heated to 80 degree celsius, it's pH will:
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A weak acid HA has degree of dissociation x. Which option gives the correct expression of (\(\mathrm{pH}-{\mathrm{pk}}_{\mathrm{b}}\))
(Memory-based Question 28/ Jan/25 morning shift )
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If equal volumes of \({\mathrm{AB}}_{2}\) and XY (both are salts) aqueous solutions are mixed, which of the following combination will give a precipitate of \({\mathrm{AY}}_{2}\) at \(300\) K ?
\((\mathrm{Given}{\mathrm{K}}_{\mathrm{sp}}(\mathrm{at}300\mathrm{K})\)\(\mathrm{for}{\mathrm{AY}}_{2}=5.2\times {10}^{-7})\)
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\({K}_{sp}\) for \(Cr(OH{)}_{3}\) is \(1.6\times {10}^{-30}\). What is the molar solubility of this salt in water?
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\({K}_{sp}\) for \(Cr(OH{)}_{3}\) is \(1.6\times {10}^{-30}\). What is the molar solubility of this salt in water?
[JEE Main 2025, 24 Jan (Shift 1)]
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At temperature T, compound \(A{B}_{2(g)}\) dissociates as \(A{B}_{2(g)}⇌AB(g)+\frac{1}{2}{B}_{2(g)}\) having degree of dissociation x (small compared to unity). The correct expression for x in terms of \({K}_{p}\) and p is
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A weak acid HA has degree of dissociation x. Which option gives the correct expression of ( \(pH-\) \(\left.p{K}_{a}\right)\)?
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The equilibrium constant for the reaction
\(S{O}_{3}(g)⇌S{O}_{2}(g)+\frac{1}{2}{O}_{2}(g)\)
is \({K}_{c}=4.9\times {10}^{-2}\). The value of \({K}_{c}\) for the reaction given below is \(2S{O}_{2}(g)+{O}_{2}(g)⇌2S{O}_{3}(g)\) is :
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The pH of 1 N aqueous solutions of HCl, \(C{H}_{3}COOH\) and HCOOH follows the order:
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At \(25^\circ \mathrm{C}\), the concentration of \({\mathrm{H}}^{+}\) ions in \(1.00\times {10}^{-3}\mathrm{M}\) aqueous solution of a weak monobasic acid having acid dissociation constant \(\left({K}_{\mathrm{a}}\right)\) of \(4.00\times {10}^{-11}\) is \(X\times {10}^{-7}\mathrm{M}\). The value of \(X\) is (nearest integer)___________
Use: Ionic product of water \(\left({K}_{\mathrm{w}}\right)=1.00\times {10}^{-14}\) at \(25^\circ \mathrm{C}\)
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The molar solubility(s) of zirconium phosphate with molecular formula \({\left({\mathrm{Zr}}^{4+}\right)}_{3}{\left(P{{O}_{4}}^{-3}\right)}_{4}\) is given by relation
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Le-Chatelier’s principle is not applicable to
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Consider the given following reaction
\({\mathrm{X}}_{2}\mathrm{Y}(\mathrm{s})⇌{\mathrm{X}}_{2}(\mathrm{g})+1/2{\mathrm{Y}}_{2}(\mathrm{g}).\mathrm{If}\alpha\) is the degree of dissociation. Calculate \({\mathrm{K}}_{\mathrm{p}}\)in the terms of P total pressure. (Memory Based JEE Mains 23/01/2025 ,Shift -2)
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Arrange the following in increasing order of solubility product : \(Ca(OH{)}_{2},AgBr,PbS,HgS\)
[JEE Main 2025, 28 Jan (Shift 2)]
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At temperature T, compound \(A{B}_{2(g)}\) dissociates as \(A{B}_{2(g)}⇌AB(g)+\frac{1}{2}{B}_{2(g)}\) having degree of dissociation x (small compared to unity). The correct expression for x in terms of \({K}_{p}\) and p is
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Consider the following chemical equilibrium of the gas phase reaction at a constant temperature :
\(\mathrm{A}(\mathrm{g})⇌\mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})\)
If p being the total pressure, \({\mathrm{K}}_{\mathrm{p}}\) is the pressure equilibrium constant and \(\alpha\) is the degree of dissociation, then which of the following is true at equilibrium ?
[JEE Main 2025, 2 Apr (Shift 2)]
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Ice and water are placed in a closed container at a pressure at 1 atm and temperature 273.15 K .
If the pressure of the container increases 2 times and the temperature is kept constant, than identify the correct observation from the following.
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pH of water is 7 at 25 degree celsius. If water is heated to 80 degree celsius, it's pH will be :
[JEE Main 2025, 23 Jan (Shift 2)]
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The pH of 1 N aqueous solutions of HCl, \(C{H}_{3}COOH\) and HCOOH follows the order:
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For a reaction, \({N}_{2}{O}_{5(g)}\to 2N{O}_{2(g)}+\frac{1}{2}{O}_{2(g)}\) in a constant volume container, no products were present initially. The final pressure of the system when 50 % of reaction gets completed is
[JEE Main 2025, 24 Jan (Shift 1)]
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Which of the following is not correct?
[JEE Main 2024, 29 Jan (Shift 1)]
(A) \(\Delta \mathrm{G}\) is positive for a spontaneous reaction
(B) \(\Delta \mathrm{G}\) is positive for a non-spontaneous reaction
(C) \(\Delta \mathrm{G}\) is zero for a reversible reaction
(D) \(\Delta \mathrm{G}\) is equal to zero for a spontaneous reaction
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Only one litre buffer solution was prepared by adding \(0.10\) mol each of \({\mathrm{NH}}_{3}\) and \({\mathrm{NH}}_{4}\mathrm{Cl}\) in deionised water. The change in pH on addition of \(0.05\) mol of \(\mathrm{HCl}\) to the above solution is ____ \(\times {10}^{-2}\), (Nearest integer) (Given : \({\mathrm{pK}}_{\mathrm{b}}\)of \({\mathrm{NH}}_{3}=4.745\) and \({\log }_{10}3=0.477\) )
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Given below are two statements :
Statement I : When a system containing ice in equilibrium with water (liquid) is heated, heat is absorbed by the system and there is no change in the temperature of the system until whole ice gets melted.
Statement II : At melting point of ice, there is absorption of heat in order to overcome intermolecular forces of attraction within the molecules of water in ice and kinetic energy of molecules is not increased at melting point.
In the light of the above statements, choose the correct answer from the options given below:
[JEE Main 2025, 3 Apr (Shift 2)]
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For the given hypothetical reactions, the equilibrium constants are as follows :
\(\begin{aligned}& X \rightleftharpoons Y ; K _1=1.0 \\& Y \rightleftharpoons Z ; K _2=2.0 \\& Z \rightleftharpoons W ; K _3=4.0\end{aligned}\)
The equilibrium constant for the reaction \(X \rightleftharpoons W\) is
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For a sparingly soluble salt \(A{B}_{2}\), the equilibrium concentrations of \({A}^{2+}\) ions and \({B}^{-}\)ions are \(1.2\times {10}^{-4}M\) and \(0.24\times {10}^{-3}M\), respectively. The solubility product of \(A{B}_{2}\) is :
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An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would
(Given log 2 = 0.30)
[JEE Main 2025, 7 Apr (Shift 1)]
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Consider the equilibrium
\(CO(g)+3{H}_{2}(g)⇌C{H}_{4}(g)+{H}_{2}O(g)\)
If the pressure applied over the system increases by two fold at constant temperature then
(A) Concentration of reactants and products increases.
(B) Equilibrium will shift in forward direction.
(C) Equilibrium constant increases since concentration of products increases.
(D) Equilibrium constant remains unchanged as concentration of reactants and products remain same.
Choose the correct answer from the options given below
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Consider the following equilibrium, \(\mathrm{CO}(\mathrm{g})+2{\mathrm{H}}_{2}(\mathrm{g})⇌{\mathrm{CH}}_{3}\mathrm{OH}(\mathrm{g})\),\(0.1\)mol of \(\mathrm{CO}\)along with a catalyst is present in a \(2{\mathrm{dm}}^{3}\) flask maintained at \(500\) K . Hydrogen is introduced into the flask until the pressure is 5 bar and \(0.04\) mol of \({\mathrm{CH}}_{3}\mathrm{OH}\) is formed. The \({\mathrm{K}}_{\mathrm{p}}^{0}\) is _________ \(\times {10}^{-3}\) (nearest integer).
Given : \(\mathrm{R}=0.08{\mathrm{dm}}^{3}\mathrm{bar}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}\) bar \({\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}\)
Assume only methanol is formed as the product and the system follows ideal gas behaviour.
[JEE Main 2025, 2 Apr (Shift 1)]
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Consider the given following reaction
\({\mathrm{X}}_{2}\mathrm{Y}(\mathrm{s})⇌{\mathrm{X}}_{2}(\mathrm{g})+1/2{\mathrm{Y}}_{2}(\mathrm{g}).\mathrm{If}\alpha\) is the degree of dissociation. Calculate \({\mathrm{K}}_{\mathrm{p}}\)in the terms of P total pressure. (Memory Based JEE Mains 23/01/2025 ,Shift -2)
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Consider the following chemical equilibrium of the gas phase reaction at a constant temperature :
\(\mathrm{A}(\mathrm{g})⇌\mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})\)
If p being the total pressure, \({\mathrm{K}}_{\mathrm{p}}\) is the pressure equilibrium constant and \(\alpha\) is the degree of dissociation, then which of the following is true at equilibrium ?
[JEE Main 2025, 2 Apr (Shift 2)]
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Arrange the following in increasing order of solubility product : \(Ca(OH{)}_{2},AgBr,PbS,HgS\)
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Find the value of solubility of zirconium phosphate with formula \(\left[{\mathrm{Zr}}_{3}{\left({\mathrm{PO}}_{4}\right)}_{4}\right]\) in terms of solubility product Ksp
(memory based jee mains shift-2 22/01/2025)
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Ice and water are placed in a closed container at a pressure of 1 atm and temperature 273.15 K . If pressure of the system is increased 2 times, keeping temperature constant, then identify correct observation from following
[JEE Main 2025, 28 Jan (Shift 1)]
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Ice and water are placed in a closed container at a pressure of 1 atm and temperature 273.15 K. If pressure of the system is increased 2 times, keeping temperature constant, then identify correct observation from following
[JEE Main 2025, 28 Jan (Shift 1)]
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Consider the following reaction (memory based jee mains shift-1 29/01/2025)
\({\mathrm{A}}_{2}\mathrm{B}\left(\mathrm{g}\right)⇌{\mathrm{A}}_{2}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{B}}_{2}\left(\mathrm{g}\right)\)
If 'P' is the total pressure at equilibrium and K is the equilibrium constant, then \(\alpha\) in terms of K and P will be
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Which of the following compound CANNOT act as a Lewis base?
[JEE Main 2021, 17 Mar (Shift 1)]
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Arrange the following solutions in the decreasing order of \(\mathrm{pOH}\)
(1) \(0.01\text{M}\mathrm{HCl}\)
(2) \(0.01\text{M}\mathrm{NaOH}\)
(3) \(0.01\text{M}{\mathrm{CH}}_{3}\mathrm{COONa}\)
(4) \(0.01\text{M}\mathrm{NaCl}\)
[JEE Main 2020, 6 Sep (Shift 1)]
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On decreasing the pH from 7 to 2, the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from 10–4 mol L–1 to 10–3 mol L–1. The pKa of HX is
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For the following Assertion and Reason, the correct option is:
Assertion (A): The pH of water increase with increase in temperature.
Reason (R): The dissociation of water into \({\mathrm{H}}^{+}\)and \({\mathrm{OH}}^{-}\)is an exothermic reaction
[JEE Main 2020, 8 Jan (Shift 2)]
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Consider the reaction \( \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g}) \).
The temperature at which \( \mathrm{K}_{\mathrm{C}}=20.4 \) and \( \mathrm{K}_{\mathrm{P}}=600.0 \mathrm{~K} \). (Round off to the nearest integer) (Assume all gases are ideal and \( \mathrm{R}=0.0831 \mathrm{~L} \mathrm{bar} \mathrm{K}^{-1} \mathrm{~mol}^{-1} \))
[JEE Main 2021, 17 Mar (Shift 2)]
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The ratio \(\frac{{K}_{p}}{{K}_{c}}\) for the reaction
\(\mathrm{CO}(\mathrm{g})+1/2{\mathrm{O}}_{2}⇌\mathrm{CO}(\mathrm{g})\mathrm{is}\)
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On decreasing the \(\mathrm{pH}\) from 7 to 2 , the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from \({10}^{-4}\mathrm{mol}{\mathrm{L}}^{-1}\) to \({10}^{-3}\mathrm{mol}{\mathrm{L}}^{-1}\). The \({\mathrm{pK}}_{\mathrm{a}}\) of \(\mathrm{HX}\) is:
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At 298 K, for the equilibrium:
\({\mathrm{PCl}}_{3}\left(\mathrm{g}\right)+{\mathrm{Cl}}_{2}\left(\mathrm{g}\right)⇄{\mathrm{PCl}}_{5}\left(\mathrm{g}\right)\)
Initial equilibrium concentrations are:
\(\left[{\mathrm{PCl}}_{3}\right]=0.20mol{L}^{-1}\\ \left[C{l}_{2}\right]=0.10mol{L}^{-1}\\ [{\mathrm{PCl}}_{5}]=0.40mol{L}^{-1}\\ {K}_{c}=20\)
Now, 0.20 mol L⁻¹ \({\mathrm{Cl}}_{2}\) is added. Find the new equilibrium concentration of \({\mathrm{PCl}}_{3}\)
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The equilibrium constant \( \mathrm{K}_{c} \) at \( 298 \mathrm{~K} \) for the reaction \( \mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D} \) is 100. Starting with an equimolar solution with concentrations of \( \mathrm{A}, \mathrm{B}, \mathrm{C} \) and \( \mathrm{D} \) all equal to \( 1 \mathrm{M} \), the equilibrium concentration of \( \mathrm{D} \) is "c" M .The value of \(22\times c\) is _______.
[JEE Main 2021, 26 Aug (Shift 2)]
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Assuming that \( \mathrm{Ba}(\mathrm{OH})_{2} \) is completely ionised in aqueous solution under the given conditions, the concentration of \( \mathrm{H}_{3} \mathrm{O}^{+} \)ions in \( 0.005 \mathrm{~M} \) aqueous solution of \( \mathrm{Ba}(\mathrm{OH})_{2} \) at 298 \( \mathrm{K} \) is \( \mathrm{x} \times 10^{-12} \mathrm{~mol} \mathrm{~L}^{-1} \). Find the value of \( \mathrm{x} \).
[JEE Main 2021, 25 Jul (Shift 2)]
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(i) \(\mathrm{X}(\mathrm{g})⇌\mathrm{Y}(\mathrm{g})+\mathrm{Z}(\mathrm{g}){\mathrm{K}}_{{\mathrm{p}}_{1}}=3\)
(ii) \(\mathrm{A}(\mathrm{g})⇌2\mathrm{B}(\mathrm{g}){\mathrm{K}}_{{\mathrm{p}}_{2}}=1\)
If the degree of dissociation and initial concentration of both the reactants X(g) and A(g) are equal, then the ratio of the total pressure at equilibrium \(\left(\frac{{p}_{1}}{{p}_{2}}\right)\) is equal to x: 1. The value of x is (Nearest integer)
[JEE Main 2023, 1 Feb (Shift 1)]
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The \({\mathrm{OH}}^{-}\)concentration in a mixture of \(5.0\mathrm{mL}\) of \(0.0504\mathrm{M}\) \({\mathrm{NH}}_{4}\mathrm{Cl}\) and \(2\mathrm{mL}\) of \(0.0210M{\mathrm{NH}}_{3}\) solution is __________\(\mathrm{x}\times {10}^{-6}\mathrm{M}\). The value of \(\mathrm{x}\) is . (Nearest integer)
[Given \({\mathrm{K}}_{\mathrm{w}}=1\times {10}^{-14}\) and \({\mathrm{K}}_{\mathrm{b}}=1.8\times {10}^{-5}\) ]
[JEE Main 2021, 26 Aug (Shift 1)]
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The \({\mathrm{K}}_{\mathrm{sp}}\) for the following dissociation is \(1.6\times {10}^{-5}\)
\({\mathrm{PbCl}}_{2}(\mathrm{s})⇌{\mathrm{Pb}}^{2+}(\mathrm{aq})+2{\mathrm{Cl}}^{-}(\mathrm{aq})\)
Which of the following choices is correct for a mixture of \(300\mathrm{mL}0.134M\mathrm{Pb}{\left({\mathrm{NO}}_{3}\right)}_{2}\) and \(100\mathrm{mL}0.4M\mathrm{NaCl}\) ?
[JEE Main 2020, 9 Jan (Shift 1)]
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Which of the following statement(s) is/are correct?
(A) The pH of \(1\times {10}^{-8}\) solution is 8 .
(B) The conjugate base \({\mathrm{H}}_{2}{\mathrm{PO}}_{4}^{-}\) is \(\mathrm{H}{{\mathrm{PO}}_{4}}^{2-}\).
(C) \({\mathrm{K}}_{\mathrm{W}}\) increases with increase in temperature.
(D) When a solution of weak monoprotic acid is titrated against a strong base at half neutralisation point, \(\mathrm{pH}=\frac{1}{2}{\mathrm{pK}}_{\mathrm{a}}\)
Choose the correct answer from the option given below.
[JEE Main 2023, 15 Apr (Shift 1)]
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Amongst the given options which of the following molecules/ion acts as a Lewis acid?
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\[\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) ; \mathrm{K}_{\mathrm{C}}=1.844\]
3.0 moles of \( \mathrm{PCl}_{5} \) is introduced in a \( 1 \mathrm{~L} \) closed reaction vessel at \( 380 \mathrm{~K} \). The number of moles \( \mathrm{PCl}_{5} \) at equilibrium is _____ \( \times 10^{-3} \). (Round off to the nearest integer)
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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)
\([\log 2.5=0.3979]\)
[JEE Main 2021, 31 Aug (Shift 2)]
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Hydrolysis of sucrose is given by the following reaction.
Sucrose \( +\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \) Glucose \( + \) Fructose
If the equilibrium constant \( \left(\mathrm{K}_{\mathrm{c}}\right) \) is \( 2 \times 10^{13} \) at \( 300 \mathrm{~K} \), the value of \( \Delta_{r} \mathrm{G}^{\mathrm{o}} \) at the same temperature will be :
[NEET 2020]
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A homogeneous ideal gaseous reaction \( \mathrm{AB}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{A}(\mathrm{g})+2 \mathrm{~B}(\mathrm{~g}) \) is carried out in a 25 litre flask at \( 27^{\circ} \mathrm{C} \). The initial amount of \( \mathrm{AB}_{2} \) was 1 mole and the equilibrium pressure was \( 1.9 \mathrm{~atm} \). The value of \( \mathrm{K}_{P} \) is \( \mathrm{x} \times 10^{-2} \). The value of \( \mathrm{x} \) is _____________(Round off to nearest integer)\[
[JEE Main 2021, 26 Feb (Shift 1)]
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On decreasing the \(\mathrm{pH}\) from 7 to 2 , the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from \({10}^{-4}\mathrm{mol}{\mathrm{L}}^{-1}\) to \({10}^{-3}\mathrm{mol}{\mathrm{L}}^{-1}\). The \({\mathrm{pK}}_{\mathrm{a}}\) of \(\mathrm{HX}\) is:
[JEE Advanced 2023, Paper-1]
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Value of \( K_{P} \) for the equilibrium reaction, \( \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g}) \) at \( 288 \mathrm{~K} \) is 47.9 . The \( \mathrm{K}_{\mathrm{C}} \) for this reaction at same temperature is ___
(Nearest integer \( ) \quad\left(\mathrm{R}=0.083 \mathrm{~L}\right. \) bar \( \left.\mathrm{K}^{-1} \mathrm{~mol}^{-1}\right) \)
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A solution of \({\mathrm{NH}}_{4}\mathrm{Cl}\) and \({\mathrm{NH}}_{3}\) has pH = 8.0. Which of the following hydroxides may be precipitated when this solution is mixed with equal volume of 0.2 M of metal ion.
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The solubility product of \(\mathrm{Cr}(\mathrm{OH})_3\) at \(298 \mathrm{~K}\) is \(6.0 \times 10^{-31}\). The concentration of hydroxide ions in a saturated solution of \(\mathrm{Cr}(\mathrm{OH})_3\) will be:
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The density of a monobasic strong acid (Molar mass \(24.2\mathrm{g}\) ) is \(1.21\mathrm{kg}/L\). The volume of its solution required for the complete neutralization of \(25\mathrm{mL}\) of \(0.24\mathrm{M}\mathrm{NaOH}\) is .............\(\times {10}^{-2}\mathrm{mL}\) (Nearest integer)
[JEE Main 2023, 25 Jan (Shift 1)]
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Sulphurous acid \( \left(\mathrm{H}_{2} \mathrm{SO}_{3}\right) \) has
\( \mathrm{Ka}_{1}=1.7 \times 10^{-2} \) and \( \mathrm{Ka}_{2}=6.4 \) \( \times 10^{-8} \). The \( \mathrm{pH} \) of \( 0.588 \mathrm{~M} \mathrm{~H}_{2} \mathrm{SO}_{3} \) is........ (Round off to the nearest integer)
[JEE Main 2021, 16 Mar (Shift 2)]
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The \( \mathrm{pK}_{\mathrm{b}} \) of dimethylamine and \( \mathrm{pK}_{\mathrm{a}} \) of acetic acid are \( 3.27 \) and \( 4.77 \) respectively at \( \mathrm{T}(\mathrm{K}) \). The correct option for the \( \mathrm{pH} \) of dimethylammonium acetate solution is:
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For the reaction \( \mathrm{A}_{(\mathrm{g})} \rightleftharpoons \mathrm{B}_{(\mathrm{g})} \), the value of the equilibrium constant at \( 300 \mathrm{~K} \) and \( 1 \mathrm{~atm} \) is equal to 100.0 . The value of \( \Delta_{\mathrm{r}} \mathrm{G} \) for the reaction at \( 300 \mathrm{~K} \) and 1 atm in \( \mathrm{J} \mathrm{mol}^{-1} \) is \( -\mathrm{xR} \), where \( \mathrm{x} \) is
(Rounded off to the nearest integer)
\( \left(\mathrm{R}=8.31 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right. \) and \( \left.\ln 10=2.3\right) \)
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The reaction rate for the reaction
\[\left[\mathrm{PtCl}_{4}\right]^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{3}\right]^{-}+\mathrm{Cl}^{-}\]
was measured as a function of concentration of different species. It was observed that
\[\begin{array}{l}\frac{-\mathrm{d}\left[\left[\mathrm{PtCl}_{4}\right]^{2-}\right]}{\mathrm{dt}}=4.8 \times 10^{-5} \\ {\left[\left[\mathrm{PtCl}_{4}\right]^{2-}\right]-2.4 \times 10^{-3}\left[\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{3}\right]^{-}\right]\left[\mathrm{Cl}^{-}\right] \text {. }} \\\end{array}\]
where square brackets are used to denote molar concentration. The equilibrium constant \( \mathrm{K}_{\mathrm{C}}= \) _____\(\text{x}{10}^{-2}\). (Nearest integer)
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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 \( \mathrm{NaOH} \), phenolphthalein is not a suitable indicator.
- In the light of above statements, choose the most appropriate - answer from the options given below.
[JEE Main 2021, 26 Aug (Shift 1)]
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A mixture of 1 mole of \({\mathrm{H}}_{2}\mathrm{O}\) and 1 mole of CO is taken in a 10 litre container and heated to 725 K. At equilibrium 40% of water by mass reacts with carbon monoxide according to the equation :
\(\mathrm{CO}(\mathrm{g})+{\mathrm{H}}_{2}\mathrm{O}(\mathrm{g})\to {\mathrm{CO}}_{2}(\mathrm{g})+{\mathrm{H}}_{2}(\mathrm{g})\)
The value of \({\mathrm{K}}_{\mathrm{C}}\times {10}^{2}\) for the reaction is_______.
(KC - Equilibrium constant) (Nearest integer)
[JEE Main 2023, 11 Apr (Shift 1)]
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3g of acetic acid is added to 250mL of 0.1 M HCL and the solution made up to 500 mL. To 20 mL of this solution \(1/2\mathrm{mL}\) of 5 M NaOH is added.
The pH of the solution is___________(round off to the nearest integer)
[Given: pKa of acetic acid =4.75, molar mass of acetic acid =60 g/ mol, log 3=0.4771] Neglect any changes in volume.
[JEE Main 2020, 7 Jan (Shift 2)]
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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 \( \mathrm{NaOH} \), phenolphthalein is not a suitable indicator.
In the light of above statements, choose the most appropriate - answer from the options given below
[JEE Main 2021, 26 Aug (Shift 1)]
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An acidified solution of \(0.05 M Zn ^{2+}\) is saturated with \(0.1 M H _2 S\). What is the minimum molar concentration (M) of \(H ^{+}\)required to prevent the precipitation of \(ZnS\) ?
Use \(K _{ sp }( ZnS )=1.25 \times 10^{-22}\) and overall dissociation constant of \(H _2 S , K _{ NET }= K _1 K _2=1 \times 10^{-21}\)
[JEE Advanced 2020, Paper-2]
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The dissociation constant of acetic is \(x\times {10}^{-5}\). When \(25\mathrm{mL}\) of \(0.2\mathrm{M}{\mathrm{CH}}_{3}\mathrm{COONa}\) solution is mixed with \(25\mathrm{mL}\) of \(0.02\mathrm{M}{\mathrm{CH}}_{3}\mathrm{COOH}\) solution, the \(\mathrm{pH}\) of the resultant solution is found to be equal to 5 . The value of x is
[JEE Main 2023, 24 Jan (Shift 1)]
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Water decomposes at \(2300 \mathrm{~K}\)
\({\mathrm{H}}_{2}\mathrm{O}(\mathrm{g})\to {\mathrm{H}}_{2}(\mathrm{g})+\frac{1}{2}{\mathrm{O}}_{2}(\mathrm{g})\)
The percent of water decomposing at \(2300 \mathrm{~K}\) and \(1 \mathrm{bar}\) is......... (Nearest integer).
Equilibrium constant for the reaction is \(2 \times 10^{-3}\) at \(2300 \mathrm{~K}\).
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Which one of the following molecular hydrides acts as a Lewis acid?
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Millimoles of calcium hydroxide required to produce 100 mL of the aqueous solution of pH =12 is x \(\times {10}^{-1}\). The value of \(\mathrm{x}\) is ________(Nearest integer).
Assume complete dissociation.
[JEE Main 2023, 29 Jan (Shift 1)]
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\(\mathrm{A}(\mathrm{g})⇌2\mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})\)
For the given reaction, if the initial pressure is \(450\mathrm{mm}\) Hg and the pressure at time t is \(720\mathrm{mmHg}\) at a constant temperature T and constant volume V. The fraction of Ag decomposed under these conditions is \(\mathrm{x}\times {10}^{-1}\). The value of x is (nearest integer)
[JEE Main 2023, 10 Apr (Shift 2)]
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4.5 moles each of hydrogen and iodine is heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for
\({\mathrm{H}}_{2}(\mathrm{g})+{\mathrm{I}}_{2}(\mathrm{g})⇌2\mathrm{HI}(\mathrm{g})\) is _____
[JEE Main 2023, 11 Apr (Shift 2)]
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The effect of addition of helium gas to the following reaction in equilibrium state, is:
\({\mathrm{PCI}}_{5}(\mathrm{g})⇌{\mathrm{PCl}}_{3}(\mathrm{g})+{\mathrm{Cl}}_{2}(\mathrm{g})\)
[JEE Main 2023, 1 Feb (Shift 2)]
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The solubility of \(\mathrm{Ca}(\mathrm{OH}{)}_{2}\) in water is :
[Given : The solubility product of \(\mathrm{Ca}(\mathrm{OH}{)}_{2}\) in water \(=5.5\times {10}^{-6}\) ]
[JEE Main 2021, 25 Feb (Shift 2)]
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An acidic buffer is obtained on mixing
[JEE Main 2020, 3 Sep (Shift 1)]
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The gas phase reaction,
\[2 \mathrm{~A}(\mathrm{~g}) \rightleftharpoons \mathrm{A}_{2}(\mathrm{~g})\]
at \( 400 \mathrm{~K} \) has \( \Delta \mathrm{G}^{0}=+25.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \).
The equilibrium constant \( \mathrm{K}_{\mathrm{C}} \) for this reaction is ____ \( \times 10^{-2} \) (Round off to the nearest integer) (Use : \( \mathrm{R}=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}, \ln 10=2.3, \log _{10} 2=0.30,1 \mathrm{~atm} \) - \( =1 \) bar \( )(\operatorname{antilog}(-0.3)=0.501) \)
[JEE Main 2021, 18 Mar (Shift 2)]
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In order to prepare a buffer solution of \( \mathrm{pH} = ~5.74 \), sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is \( 1.0 \mathrm{~M} \), the concentration of sodium acetate in the buffer is _____M.
(Round off to the nearest integer).
[Given; \( \mathrm{pK}_{\mathrm{a}}( \) acetic acid \( )=4.74 \) ]
[JEE Main 2021, 18 Mar (Shift 1)]
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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 __________ \({10}^{-12}{\left(\mathrm{mol}/\mathrm{L}\right)}^{3}\).
Given molar mass: \( \mathrm{CaF}_{2}=78 \mathrm{~g} \mathrm{~mol}^{-1} \)
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The number of correct statements involving equilibria in physical process from the following is
(i) Equilibrium is possible only in a closed system at a given temperature.
(ii) Both the opposing processes occur at the same rate.
(iii) When equilibrium is attained at a given temperature, the value of all its parameters became equal.
(iv) For dissolution of solids in liquids, the solubility is constant at a given temperature
[JEE Main 2023, 10 Apr (Shift 1)]
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25.0 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 \(0.5\times {10}^{-6}\) at \(298\mathrm{K}\). The ratio of \(\left[{\mathrm{Ba}}^{2+}\right]{\left[{\mathrm{F}}^{-}\right]}^{2}\) and \({\mathrm{K}}_{\mathrm{sp}}\) is...................... (Nearest integer)
[JEE Main 2023, 13 Apr (Shift 1)]
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Two salts \( A_{2} X \) and \( M X \) have the same value of solubility product of \( 4.0 \times 10^{-12} \). The ratio of their molar solubilities i.e. \( \frac{S\left(A_{2} X\right)}{S(M X)}= \)___________
(Round off to the nearest integer).
[JEE Main 2021, 16 Mar (Shift 1)]
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Given below are two statements:
Statement I: Methyl orange is a weak acid.
Statement II: The benzenoid form of methyl orange is more intense / deeply coloured than the quinonoid form.
In the light of the above statements, choose the most appropriate answer from the options given below.
[JEE Main 2023, 08 Apr (Shift 2)]
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\(20\mathrm{mL}\) of 0.1 M NaOH is added to \(50\mathrm{mL}\) of 0.1 M acetic acid solution. The pH of the resulting solution is _________\(\times {10}^{-2}\) (Nearest integer)
Given : \({\mathrm{pK}}_{\mathrm{a}}\left({\mathrm{CH}}_{3}\mathrm{COOH}\right)=4.76\)
\(\log 2=0.30\)
\(\log 3=0.48\)
[JEE Main 2023, 13 Apr (Shift 2)]
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The molar solubility of \( \mathrm{Zn}(\mathrm{OH})_{2} \) in \( 0.1 \mathrm{~M} \mathrm{~NaOH} \) solution is \( x \times 10^{-18} \mathrm{M} \). The value of \( x \) is ___________. (Nearest integer)
(Given: The solubility product of \( \mathrm{Zn}(\mathrm{OH})_{2} \) is \( 2 \times 10^{-20} \) )
[JEE Main 2021, 1 Sep (Shift 2)]
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For reaction : \({\mathrm{SO}}_{2}(\mathrm{g})+\frac{1}{2}{\mathrm{O}}_{2}(\mathrm{g})⇌{\mathrm{SO}}_{3}(\mathrm{g})\)
KP = 2 × 1012 at 27°C and 1 atm pressure. The KC for the same reaction is …… × 1013. (Nearest integer)
(Given R = 0.082L atm K–1 mol–1)
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