Solutions
128 JEE Chemistry previous year questions on Solutions — options free on every question; 13 include the answer & explanation free, the rest unlock with PYQ Pass.
What is the freezing point depression constant of a solvent 50 g of which contain 1 g of non-volatile solute(M.W: 256 g/mol and depression in freezing point is 0.4 K.
Memory Based Question 28/Jan/25 Morning shift
\(5.12\mathrm{K}\mathrm{Kg}{\mathrm{mol}}^{-1}\)
\(\mathrm{Depression}\mathrm{in}\mathrm{freezing}\mathrm{point}∆{\mathrm{T}}_{\mathrm{b}}={\mathrm{K}}_{\mathrm{f}}.\mathrm{m}\\ \mathrm{molality}\mathrm{m}=\frac{1}{256}\times \frac{1000}{50}=0.0781\\ {\mathrm{K}}_{\mathrm{f}}=\frac{∆{\mathrm{T}}_{\mathrm{b}}}{\mathrm{m}}=0.4/0.0781=5.12\mathrm{KKg}/\mathrm{mol}\)
Molality \(( m )\) of \(3 M\) aqueous solution of \(NaCl\) is
(Given : Density of solution \(=1.25 ~g mL ^{-1}\), Molar mass in \(g mol ^{-1}\) : \(\mathrm{Na}:23,\mathrm{Cl}:35.5\))
[JEE Main 2024, 6 Apr (Shift 2)]
\(2.79\) m
Molality \((m)\) is given as
\(m=\frac{{n}_{\text{solute }}}{k{g}_{\text{solvent }}}\)
To calculate no. of moles of solute we take the help of molarity and to determine mass of solvent we take the help of density of solution. \(3 M\) solution of \(N a C l\) implies that there are 3 moles of \(N a C l\) in every 1 litre of solution. Considering \(1 L\) of solution, we have
\({n}_{\mathrm{NaCl}}=3\mathrm{mol}\)
Mass of \(1 L\) solution of \(\mathrm{NaCl}=(\) volume \()(\) density )
\(\begin{matrix} & =(1000\mathrm{mL})(1.25{\mathrm{gmol}}^{−1}) \\ & =1250\mathrm{g}\end{matrix}\)
Mass of NaCl in 1L of solution \(\begin{matrix} & =({n}_{\mathrm{NaCl}})({\mathrm{mm}}_{\mathrm{NaCl}})\end{matrix}\)
\(\begin{matrix} & =(3\mathrm{mol})(58.5{\mathrm{gmol}}^{−1}) \\ & =175.5\mathrm{g}\end{matrix}\)
Mass of solvent \(\left({\mathrm{H}}_{2}\mathrm{O}\right)=\) Mass of solution - Mass of solute \(=(1250\mathrm{g})-(175.5\mathrm{g})\)
\(=1074.5g\)
Thus
\(\begin{matrix} & m=\frac{{n}_{\text{solute}}}{{g}_{\text{solv}}}\frac{1000g}{kg} \\ & =\frac{3\mathrm{mol}}{1074.5g}\times \frac{1000g}{\mathrm{kg}} \\ & 2.79molk{g}^{-1}\end{matrix}\\\)
Alternatively \(m=\frac{{M}_{\text{soln }}}{1000d−{M}_{\text{soln }m{m}_{\text{solute }}}}\times 1000\)
\(\begin{matrix} & =\frac{3}{(1000)(1.25)−(3)(58.5)}\times 1000 \\ & =2.79{\mathrm{molkg}}^{−1}\end{matrix}\)
In a 3M aqueous solution of NaCl, having density 1.25 g/ml, what will be the molality of the solution?
2.79
\(molality(m)=\frac{1000M}{1000d-M\times {M}_{0}}(whereM=molarity,{M}_{0}=molarmass)\\ m=\frac{3000}{1250-58.5\times 3}=2.79\)
What is the freezing point depression constant of a solvent 50 g of which contain 1 g of non-volatile solute(M.W: 256 g/mol and depression in freezing point is 0.4 K.
Memory Based Question 28/Jan/25 Morning shift
\(5.12\mathrm{K}\mathrm{Kg}{\mathrm{mol}}^{-1}\)
\(\mathrm{Depression}\mathrm{in}\mathrm{freezing}\mathrm{point}∆{\mathrm{T}}_{\mathrm{b}}={\mathrm{K}}_{\mathrm{f}}.\mathrm{m}\\ \mathrm{molality}\mathrm{m}=\frac{1}{256}\times \frac{1000}{50}=0.0781\\ {\mathrm{K}}_{\mathrm{f}}=\frac{∆{\mathrm{T}}_{\mathrm{b}}}{\mathrm{m}}=0.4/0.0781=5.12\mathrm{KKg}/\mathrm{mol}\)
Molality \(( m )\) of \(3 M\) aqueous solution of \(NaCl\) is
(Given : Density of solution \(=1.25 ~g mL ^{-1}\), Molar mass in \(g mol ^{-1}\) : \(\mathrm{Na}:23,\mathrm{Cl}:35.5\))
[JEE Main 2024, 6 Apr (Shift 2)]
\(2.79\) m
Molality \((m)\) is given as
\(m=\frac{{n}_{\text{solute }}}{k{g}_{\text{solvent }}}\)To calculate no. of moles of solute we take the help of molarity and to determine mass of solvent we take the help of density of solution. \(3 M\) solution of \(N a C l\) implies that there are 3 moles of \(N a C l\) in every 1 litre of solution. Considering \(1 L\) of solution, we have
\({n}_{\mathrm{NaCl}}=3\mathrm{mol}\)
Mass of \(1 L\) solution of \(\mathrm{NaCl}=(\) volume \()(\) density )
\(\begin{matrix} & =(1000\mathrm{mL})(1.25{\mathrm{gmol}}^{−1}) \\ & =1250\mathrm{g}\end{matrix}\)
Mass of NaCl in 1L of solution \(\begin{matrix} & =({n}_{\mathrm{NaCl}})({\mathrm{mm}}_{\mathrm{NaCl}})\end{matrix}\)
\(\begin{matrix} & =(3\mathrm{mol})(58.5{\mathrm{gmol}}^{−1}) \\ & =175.5\mathrm{g}\end{matrix}\)
Mass of solvent \(\left({\mathrm{H}}_{2}\mathrm{O}\right)=\) Mass of solution - Mass of solute \(=(1250\mathrm{g})-(175.5\mathrm{g})\)
\(=1074.5g\)
Thus
\(\begin{matrix} & m=\frac{{n}_{\text{solute}}}{{g}_{\text{solv}}}\frac{1000g}{kg} \\ & =\frac{3\mathrm{mol}}{1074.5g}\times \frac{1000g}{\mathrm{kg}} \\ & =2.79molk{g}^{-1}\end{matrix}\\\)
Alternatively \(m=\frac{{M}_{\text{soln }}}{1000d−{M}_{\text{soln }m{m}_{\text{solute }}}}\times 1000\)
\(\begin{matrix} & =\frac{3}{(1000)(1.25)−(3)(58.5)}\times 1000 \\ & =2.79{\mathrm{molkg}}^{−1}\end{matrix}\)
Liquid A and B form an ideal solution. The vapour pressure of pure liquids A and B are \(350\) and\(750\)mm Hg respectively at the same temperature. If \({\mathrm{x}}_{\mathrm{A}}\) and \({x}_{B}\) are the mole fraction of A and B in solution while \({\mathrm{y}}_{\mathrm{A}}\) and \({y}_{B}\) are the mole fraction of A and B in vapour phase then
[JEE Main 2025, 7 Apr (Shift 2)]
\(\frac{{x}_{A}}{{x}_{B}}>\frac{{y}_{A}}{{y}_{B}}\)
\({P}_{A}^{∘}<{P}_{B}^{∘}\Rightarrow \frac{{P}_{A}^{∘}}{{P}_{B}^{∘}}<1\)
\(\frac{{y}_{A}}{{y}_{B}}=\frac{{P}_{A}^{∘}{x}_{A}}{{P}_{B}^{∘}{x}_{B}}\)
\(\Rightarrow \frac{{y}_{A}}{{y}_{B}}<\frac{{x}_{A}}{{x}_{B}}\)
\(\mathrm{HA}(\mathrm{aq})⇌{\mathrm{H}}^{+}(\mathrm{aq})+{\mathrm{A}}^{-}(\mathrm{aq})\)
The freezing point depression of a \(0.1\mathrm{m}\)aqueous solution of a monobasic weak acid HA is \(0.20^\circ \mathrm{C}\). The dissociation constant for the acid is
Given : \({\mathrm{K}}_{\mathrm{f}}\left({\mathrm{H}}_{2}\mathrm{O}\right)=1.8\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1},\mathrm{molality}\equiv \mathrm{molarity}\)
[JEE Main 2025, 8 Apr (Shift 1)]
\(1.38\times {10}^{-3}\)
ΔTf = ikfm
0.2 = i × 1.8 × 0.1
\(i=\frac{20}{18}=\frac{10}{9}\)
\(\begin{matrix}For & H{A}_{(aq)} & ⇌ & {H}_{(aq)}^{+} & + & {A}_{(aq)}^{−} \\ t=0 & 1 \\ t={t}_{eq} & 1−\alpha & & \alpha & & \alpha \end{matrix}\)
i = 1 + α
\(\frac{10}{9}=1+\alpha\)
\(\alpha =\frac{1}{9}\)
\({K}_{eq}=\frac{[{H}^{+}][{A}^{−}]}{[HA]}=\frac{C{\alpha }^{2}}{1−\alpha }\)
\(=\frac{0.1{(\frac{1}{9})}^{2}}{1−\frac{1}{9}}=\frac{1}{720}\)
\({K}_{eq.}=1.38\times {10}^{−3}\)
The plots of \(\frac{1}{{\mathrm{X}}_{\mathrm{A}}}and\frac{1}{{Y}_{A}}(where{\mathrm{X}}_{\mathrm{A}}\mathrm{and}{\mathrm{Y}}_{\mathrm{A}}\mathrm{are}\mathrm{the}\mathrm{mole}\mathrm{fraction}\mathrm{of}\mathrm{liquid}\mathrm{A}\mathrm{in}\mathrm{liquid}\mathrm{and}\mathrm{vapour}\mathrm{phase}\mathrm{respectively})\) is linear with slope and intercepts respectively
(Memory Based JEE Mains 23/01/2025 ,Shift -2)
\({{\mathrm{P}}_{\mathrm{A}}}^{0}/{{\mathrm{P}}_{\mathrm{B}}}^{0}\mathrm{and}\frac{{{\mathrm{P}}_{\mathrm{B}}}^{0}-{{\mathrm{P}}_{\mathrm{A}}}^{0}}{{{\mathrm{P}}_{\mathrm{B}}}^{0}}\)
By the Rault's law
\({\mathrm{P}}_{\mathrm{A}}={\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}{\mathrm{X}}_{\mathrm{A}}....(1)\\ {\mathrm{P}}_{\mathrm{B}}={\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}{\mathrm{X}}_{\mathrm{B}}.....(2)\\ \mathrm{Now}\\ {\mathrm{P}}_{\mathrm{A}}={\mathrm{Y}}_{\mathrm{A}}{\mathrm{P}}_{\mathrm{T}}\Rightarrow {\mathrm{P}}_{\mathrm{T}}=\frac{{\mathrm{P}}_{\mathrm{A}}}{{\mathrm{Y}}_{\mathrm{A}}}\\ {\mathrm{P}}_{\mathrm{B}}={\mathrm{Y}}_{\mathrm{B}}{\mathrm{P}}_{\mathrm{T}}\Rightarrow {\mathrm{P}}_{\mathrm{T}}=\frac{{\mathrm{P}}_{\mathrm{B}}}{{\mathrm{Y}}_{\mathrm{B}}}\\ \frac{{\mathrm{P}}_{\mathrm{A}}}{{\mathrm{Y}}_{\mathrm{A}}}=\frac{{\mathrm{P}}_{\mathrm{B}}}{{\mathrm{Y}}_{\mathrm{B}}}\\ \frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}{\mathrm{X}}_{\mathrm{A}}}{{\mathrm{Y}}_{\mathrm{A}}}=\frac{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}{\mathrm{X}}_{\mathrm{B}}}{{\mathrm{Y}}_{\mathrm{B}}}\left(\mathrm{From}\left(1\right)\mathrm{and}\left(2\right)\right)\\ \frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}{\mathrm{X}}_{\mathrm{A}}}{{\mathrm{Y}}_{\mathrm{A}}}=\frac{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}\left(1-{\mathrm{X}}_{\mathrm{A}}\right)}{1-{\mathrm{Y}}_{\mathrm{A}}}\\ \frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}\left(1-{\mathrm{Y}}_{\mathrm{A}}\right)}{{\mathrm{Y}}_{\mathrm{A}}}=\frac{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}\left(1-{\mathrm{X}}_{\mathrm{A}}\right)}{{\mathrm{X}}_{\mathrm{A}}}\\ \frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}}{{\mathrm{Y}}_{\mathrm{A}}}-\frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}{\mathrm{Y}}_{\mathrm{A}}}{{\mathrm{Y}}_{\mathrm{A}}}=\frac{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}}{{\mathrm{X}}_{\mathrm{A}}}-\frac{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}{\mathrm{X}}_{\mathrm{A}}}{{\mathrm{X}}_{\mathrm{A}}}\\ \frac{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}}{{\mathrm{X}}_{\mathrm{A}}}=\frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}}{{\mathrm{Y}}_{\mathrm{A}}}+\left({\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}-{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}\right)\\ \frac{1}{{\mathrm{X}}_{\mathrm{A}}}=\frac{1}{{\mathrm{Y}}_{\mathrm{A}}}\left(\frac{{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}}{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}}\right)+\frac{\left({\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}-{\mathrm{P}}_{\mathrm{A}}^{\mathrm{o}}\right)}{{\mathrm{P}}_{\mathrm{B}}^{\mathrm{o}}}\\ \mathrm{Compare}\mathrm{with}\mathrm{y}=\mathrm{mx}+\mathrm{c}\)
58.5 g of NaCl and 180 g of glucose were separately dissolved in 1000 mL of water.Identify the correct statement regarding the elevation of boiling point of the resulting solution.
NaCl solution will show higher elevation of boiling point.
Boiling point elevation depends on molality × van’t Hoff factor (i). NaCl (i = 2) dissociates, while glucose (i = 1) does not. Thus, NaCl solution shows higher elevation.
Which of the following binary mixture does not show the behaviour of minimum boiling azeotropes?
[JEE Main 2025, 8 Apr (Shift 1)]
\({\mathrm{C}}_{6}{\mathrm{H}}_{5}\mathrm{OH}+{\mathrm{C}}_{6}{\mathrm{H}}_{5}{\mathrm{NH}}_{2}\)
Binary mixture of C6H5OH and C6H5NH2 shows negative deviation from Raoult's law. So, vapour pressure of solution is less than V.P of pure C6H5OH and C6H5NH2. So, B.P. of solution is greater than boiling point of pure C6H5OH and C6H5NH2. So mixture shows maximum Boiling azeotrope
Considering acetic acid dissociates in water, its dissociation constant is \(6.25\times {10}^{-5}\) . If \(5\mathrm{ml}\) of acetic acid is dissolved in 1 litre water, the solution will freeze at \(-\mathrm{x}\times {10}^{-2}^\circ \mathrm{C}\), provided pure water freezes at \(0^\circ C\). \(x=\)________
Given: \({\left({K}_{f}\right)}_{\text{water }}=1.86Kkgmo{l}^{-1}\text{. }\)
Density of acetic acid is 1.2 g mL–1.
molar mass of water = 18 g mol–1.
molar mass of acetic acid = 60 g mol–1.
density of water = 1 g cm–3
Acetic acid dissociates as
\({\mathrm{CH}}_{3}\mathrm{COOH}⇌{\mathrm{CH}}_{3}{\mathrm{COO}}^{-}+{\mathrm{H}}^{+}\)
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Considering acetic acid dissociates in water, its dissociation constant is \(6.25\times {10}^{-5}\) . If \(5\mathrm{ml}\) of acetic acid is dissolved in 1 litre water, the solution will freeze at \(-\mathrm{x}\times {10}^{-2}^\circ \mathrm{C}\), provided pure water freezes at \(0^\circ C\). \(x=\)________
Given: \({\left({K}_{f}\right)}_{\text{water }}=1.86Kkgmo{l}^{-1}\text{. }\)
Density of acetic acid is 1.2 g mL–1.
molar mass of water = 18 g mol–1.
molar mass of acetic acid = 60 g mol–1.
density of water = 1 g cm–3
Acetic acid dissociates as
\({\mathrm{CH}}_{3}\mathrm{COOH}⇌{\mathrm{CH}}_{3}{\mathrm{COO}}^{-}+{\mathrm{H}}^{+}\)
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If a substance ' \(A\) ' dissolves in solution of a mixture of ' \(B\) ' and ' \(C\) ' with their respective number of moles as \(n _{ A }, n _{ B }\) and \(n _{ C }\). Mole fraction of \(C\) in the solution is
[JEE Main 2024, 30 Jan (Shift 2)]
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If a substance ' \(A\) ' dissolves in solution of a mixture of ' \(B\) ' and ' \(C\) ' with their respective number of moles as \(n _{ A }, n _{ B }\) and \(n _{ C }\). Mole fraction of \(C\) in the solution is
[JEE Main 2024, 30 Jan (Shift 2)]
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What is the freezing point depression constant of a solvent, 50 g of which contain 1 g non volatile solute (molar mass \(256gmo{l}^{-1}\) ) and the decrease in freezing point is 0.40 K ?
[JEE Main 2025, 28 Jan (Shift 1)]
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Arrange the following aqueous solutions in order of their increasing boiling points
\(\left(\mathrm{i}\right){10}^{-4}\mathrm{M}\mathrm{NaCl}\\ \left(\mathrm{ii}\right){10}^{-4}\mathrm{M}\mathrm{Urea}\\ \left(\mathrm{iii}\right){10}^{-3}\mathrm{M}\mathrm{NaCl}\\ \left(\mathrm{iv}\right){10}^{-2}\mathrm{M}\mathrm{NaCl}\)
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The quantity which changes with temperature is:
[JEE Main 2024, 27 Jan (Shift 2)]
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The quantity which changes with temperature is:
[JEE Main 2024, 27 Jan (Shift 2)]
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Assume a living cell with \(0.9\%(\omega /\omega )\) of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water.
(Consider the data upto first decimal place only)
The cell will
[JEE Main 2025, 28 Jan (Shift 2)]
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The Molarity (M) of an aqueous solution containing \(5.85\mathrm{g}\) of \(\mathrm{NaCl}\) in \(500\mathrm{mL}\) water is (Given : Molar Mass \(\mathrm{Na}\): \(23\) and \(Cl:35.5gmo{l}^{-1}\))
[JEE Main 2024, 4 Apr (Shift 1)]
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What is the value of van't Hoff Factor for \({\mathrm{A}}_{2}\mathrm{B}\) if 30% of \({\mathrm{A}}_{2}\mathrm{B}\) is dissociated?
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The molarity of \(1\mathrm{L}\) orthophosphoric acid \(\left({\mathrm{H}}_{3}{\mathrm{PO}}_{4}\right)\) having 70 % purity by weight (specific gravity \(1.54\mathrm{g}{\mathrm{cm}}^{-3}\)) is _____ \(\mathrm{M}\)
(Molar mass of \({\mathrm{H}}_{3}{\mathrm{PO}}_{4}=98\mathrm{g}{\mathrm{mol}}^{-1}\) )
[JEE Main 2024, 31 Jan (Shift 2)]
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Given below are two statements :
Statement (I) : NaCl is added to the ice at \(0^\circ C\), present in the ice cream box to prevent the melting of ice cream.
Statement (II) : On addition of NaCl to ice at \(0^\circ C\), there is a depression in freezing point.
In the light of the above statements, choose the correct answer from the options given below
[JEE Main 2025, 29 Jan (Shift 2)]
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Arrange the following solutions in order of their increasing boiling points
\(\left(\mathrm{i}\right){10}^{-4}\mathrm{M}\mathrm{NaCl}\\ \left(\mathrm{ii}\right){10}^{-4}\mathrm{M}\mathrm{Urea}\\ \left(\mathrm{iii}\right){10}^{-3}\mathrm{M}\mathrm{NaCl}\\ \left(\mathrm{iv}\right){10}^{-2}\mathrm{M}\mathrm{NaCl}\)
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The plots of \(\frac{1}{{\mathrm{X}}_{\mathrm{A}}}and\frac{1}{{Y}_{A}}(where{\mathrm{X}}_{\mathrm{A}}\mathrm{and}{\mathrm{Y}}_{\mathrm{A}}\mathrm{are}\mathrm{the}\mathrm{mole}\mathrm{fraction}\mathrm{of}\mathrm{liquid}\mathrm{A}\mathrm{in}\mathrm{liquid}\mathrm{and}\mathrm{vapour}\mathrm{phase}\mathrm{respectively})\) is linear with slope and intercepts respectively
(Memory Based JEE Mains 23/01/2025 ,Shift -2)
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A solution containing 10 g of an electrolyte in 100 g of water boils at \(100.52{}^{\mathrm{o}}\mathrm{C}\). The degree of ionization of the electrolyte is \(x\times {10}^{-1}\) (nearest integer)
[Given : Molar mass of \(AB _2=200 ~g mol ^{-1}, K _{ b }\) (molal boiling point elevation const. of water) \(=0.52 ~K kg mol ^{-1}\), boiling point of water \(=100^{\circ} C ; AB _2\) ionises as \(\left.AB _2 \rightarrow A ^{2+}+2 B ^{-}\right]\)
[JEE Main 2024, 08 Apr (Shift 1)]
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A solution containing 10 g of an electrolyte in 100 g of water boils at \(100.52{}^{\mathrm{o}}\mathrm{C}\). The degree of ionization of the electrolyte is \(x\times {10}^{-1}\) (nearest integer)
[Given : Molar mass of \(AB _2=200 ~g mol ^{-1}, K _{ b }\) (molal boiling point elevation const. of water) \(=0.52 ~K kg mol ^{-1}\), boiling point of water \(=100^{\circ} C ; AB _2\) ionises as \(\left.AB _2 \rightarrow A ^{2+}+2 B ^{-}\right]\)
[JEE Main 2024, 08 Apr (Shift 1)]
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Molality of an aqueous solution of urea is \(4.44 ~m\). Mole fraction of urea in solution is \(x \times 10^{-3}\). Value of \(x\) is (Integer answer)
[JEE Main 2024, 08 Apr (Shift 2)]
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Molality of an aqueous solution of urea is \(4.44 ~m\). Mole fraction of urea in solution is \(x \times 10^{-3}\). Value of \(x\) is (Integer answer)
[JEE Main 2024, 08 Apr (Shift 2)]
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Molality of an aqueous solution of urea is \(4.44 ~m\). Mole fraction of urea in solution is \(x \times 10^{-3}\). Value of \(x\) is (Integer answer)
[JEE Main 2024, 08 Apr (Shift 2)]
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What happens to freezing point of benzene when small quantity of napthalene is added to benzene?
[JEE Main 2024, 30 Jan (Shift 1)]
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What happens to freezing point of benzene when small quantity of napthalene is added to benzene?
[JEE Main 2024, 30 Jan (Shift 1)]
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Proceess in non spontaneous at freezing point but spontaneous at boiling point, find ΔH and ΔS ?
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An artificial cell is made by encapsulating \(0.2\mathrm{M}\) glucose solution within a semipermeable membrane. The osmotic pressure developed when the artificial cell is placed within a \(0.05\mathrm{M}\) solution of \(\mathrm{NaCl}\) at \(300\mathrm{K}\) is _______ \(\times {10}^{-1}\) bar. (nearest integer).
[Given : \(R=0.083Lbarmo{l}^{-1}{K}^{-1}\)]
Assume complete dissociation of \(\mathrm{NaCl}\)
[JEE Main 2024, 5 Apr (Shift 1)]
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Which of the following binary mixture does not show the behaviour of minimum boiling azeotropes?
[JEE Main 2025, 8 Apr (Shift 1)]
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30gm \({\mathrm{HNO}}_{3}\)is added to a solution to prepare 75 % w/ w solution having density 1.25 g / mL. Volume of solution is?
Memory Based Question 28/Jan/25 Evening shift
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Molarity (M) of an aqueous solution containing \(x \mathrm{~g}\) of anhyd. \(\mathrm{CuSO}_4\) in \(500 \mathrm{~mL}\) solution at \(32^{\circ} \mathrm{C}\) is \(2 \times 10^{-1} \mathrm{M}\). Its molality will be_____ \(\times 10^{-3} \mathrm{~m}\). (nearest integer). [Given density of the solution \(=1.25 \mathrm{~g} / \mathrm{mL}\) ]
[JEE Main 2024, 9 Apr (Shift 1)]
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\(\mathrm{HA}(\mathrm{aq})⇌{\mathrm{H}}^{+}(\mathrm{aq})+{\mathrm{A}}^{-}(\mathrm{aq})\)
The freezing point depression of a \(0.1\mathrm{m}\)aqueous solution of a monobasic weak acid HA is \(0.20^\circ \mathrm{C}\). The dissociation constant for the acid is
Given : \({\mathrm{K}}_{\mathrm{f}}\left({\mathrm{H}}_{2}\mathrm{O}\right)=1.8\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1},\mathrm{molality}\equiv \mathrm{molarity}\)
[JEE Main 2025, 8 Apr (Shift 1)]
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The Henry's law constant \(\left({\mathrm{K}}_{\mathrm{H}}\right)\) values of three gases (A, B, C) in water are \(145,2\times {10}^{-5}\) and \(35\mathrm{kbar}\), respectively. The solubility of these gases in water follow the order
[NEET 2024]
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Mass of ethylene glycol (antifreeze) to be added to \(18.6 ~kg\) of water to protect the freezing point at \(-24^\circ C\) is____________ \(kgmo{l}^{-1}\) (Round off to nearest integer) (Molar mass in \(gmo{l}^{-1}\) for ethylene glycol \(=62) ( K _f\) of water \(=1.86Kkgmo{l}^{-1}\)
[JEE Main 2024, 1 Feb (Shift 2)]
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58.5 g of NaCl and 180 g of glucose were separately dissolved in 1000 mL of water.Identify the correct statement regarding the elevation of boiling point of the resulting solution.
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200 ml of 0.2 M NaOH is mixed with 400 ml of 0.5 M NaOH solution. Molarity of mixture is:
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In which mode of expression, the concentration of a solution remains independent of temperature?
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What is the value of van't Hoff Factor for \({\mathrm{A}}_{2}\mathrm{B}\) if 30% of \({\mathrm{A}}_{2}\mathrm{B}\) is dissociated?
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When a non-volatile solute is added to the solvent, the vapour pressure of the solvent decreases by 10 mm Hg. The mole fraction of the solute in the solution is 0.2. What would be the mole fraction of the solvent if decrease in vapour pressure is 20 mm Hg?
[JEE Main 2025, 23 Jan (Shift 2)]
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2 moles each of ethylene glycol and glucose are dissolved in 500 g of water. The boiling point of the resulting solution is
(Given : Ebullioscopic constant of water \(=0.52\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}\))
[JEE Main 2025, 3 Apr (Shift 1)]
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When a non-volatile solute is added to the solvent, the vapour pressure of the solvent decreases by 10 mm Hg. The mole fraction of the solute in the solution is 0.2. What would be the mole fraction of the solvent if decrease in vapour pressure is 20 mm Hg?
[JEE Main 2025, 23 Jan (Shift 2)]
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1.24 g of \(A{X}_{2}\) (molar mass \(124gmo{l}^{-1}\)) is dissolved in 1 kg of water to form a solution with boiling point of \(100.0156^\circ C\), while 25.4 g of \(A{Y}_{2}\) (molar mass \(250gmo{l}^{-1}\)) in 2 kg of water constitutes a solution with a boiling point of \(100.0260^\circ C\).
\({K}_{b}\left({H}_{2}O\right)=0.52Kkgmo{l}^{-1}\)
Which of the following is correct ?
[JEE Main 2025, 29 Jan (Shift 1)]
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In which mode of expression, the concentration of a solution remains independent of temperature?
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The density of ' \(x\) ' \(\mathrm{M}\) solution (' \(x\) ' molar) of \(\mathrm{NaOH}\) is \(1.12\mathrm{g}{\mathrm{mL}}^{-1}\), while in molality, the concentration of the solution is \(3\mathrm{m}(3\mathrm{molal})\). Then \(x\) is
(Given : Molar mass of \(\mathrm{NaOH}\) is \(40\mathrm{g}/\mathrm{mol}\) )
[JEE Main 2024, 6 Apr (Shift 1)]
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Arrange the following solutions in order of their increasing boiling points
\(\left(\mathrm{i}\right){10}^{-4}\mathrm{M}\mathrm{NaCl}\\ \left(\mathrm{ii}\right){10}^{-4}\mathrm{M}\mathrm{Urea}\\ \left(\mathrm{iii}\right){10}^{-3}\mathrm{M}\mathrm{NaCl}\\ \left(\mathrm{iv}\right){10}^{-2}\mathrm{M}\mathrm{NaCl}\)
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Which of the following binary mixture does not show the behaviour of minimum boiling azeotropes?
[JEE Main 2025, 8 Apr (Shift 1)]
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What is the freezing point depression constant of a solvent, 50 g of which contain 1 g non volatile solute (molar mass \(256gmo{l}^{-1}\) ) and the decrease in freezing point is 0.40 K ?
[JEE Main 2025, 28 Jan (Shift 1)]
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What is the freezing point depression constant of a solvent, 50 g of which contain 1 g non volatile solute (molar mass \(256gmo{l}^{-1}\) ) and the decrease in freezing point is 0.40 K ?
[JEE Main 2025, 28 Jan (Shift 1)]
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Consider the dissociation of the weak acid \(\mathrm{HX}\) as given below
\(\mathrm{HX}(\mathrm{aq})⇌{\mathrm{H}}^{+}(\mathrm{aq})+{\mathrm{X}}^{-}(\mathrm{aq}),\mathrm{Ka}=1.2\times {10}^{-5}\)
\(\left[{\mathrm{K}}_{\mathrm{a}}\right.\) : dissociation constant]
The osmotic pressure of \(0.03\mathrm{M}\) aqueous solution of \(\mathrm{HX}\) at \(300\mathrm{K}\) is ___ \(\times {10}^{-2}\) bar (nearest integer)
[Given : \(\mathrm{R}=0.083{\mathrm{Lbarmol}}^{-1}{\mathrm{K}}^{-1}\) ]
[JEE Main 2024, 6 Apr (Shift 1)]
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Given below are two statements :
Statement (I) : NaCl is added to the ice at \(0^\circ C\), present in the ice cream box to prevent the melting of ice cream.
Statement (II) : On addition of NaCl to ice at \(0^\circ C\), there is a depression in freezing point.
In the light of the above statements, choose the correct answer from the options given below
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A solution is made by mixing one mole of volatile liquid A with \(3\) moles of volatile liquid B. The vapour pressure of pure A is 200 mm Hg and that of the solution is \(500\) mm Hg . The vapour pressure of pure B and the least volatile component of the solution, respectively, are
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Compare boiling point of given solutions:
(Memory Based JEE Mains 22/01/2025 Shift-1)
\((\mathrm{i}){10}^{-4}\mathrm{M}\mathrm{NaCl}\\ (\mathrm{ii}){10}^{-3}\mathrm{M}\mathrm{NaCl}\\ (\mathrm{iii}){10}^{-2}\mathrm{M}\mathrm{NaCl}\\ (\mathrm{iv}){10}^{-4}\mathrm{M}\mathrm{Urea}\)
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2 moles each of ethylene glycol and glucose are dissolved in 500 g of water. The boiling point of the resulting solution is
(Given : Ebullioscopic constant of water \(=0.52\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}\))
[JEE Main 2025, 3 Apr (Shift 1)]
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The solution from the following with highest depression in freezing point/lowest freezing point is
[JEE Main 2024, 30 Jan (Shift 2)]
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Proceess in non spontaneous at freezing point but spontaneous at boiling point, find ΔH and ΔS ?
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The Molarity (M) of an aqueous solution containing \(5.85\mathrm{g}\) of \(\mathrm{NaCl}\) in \(500\mathrm{mL}\) water is (Given : Molar Mass \(\mathrm{Na}\): \(23\) and \(Cl:35.5gmo{l}^{-1}\))
[JEE Main 2024, 4 Apr (Shift 1)]
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A solution is prepared by adding 1 mole ethyl alcohol in 9 mole water. The mass percent of solute in the solution is ....... (Integer answer) (Given : Molar mass in \(g mol ^{-1}\) Ethyl alcohol : \(46\) water: \(18\)\()\)
[JEE Main 2024, 08 Apr (Shift 2)]
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A solution is prepared by adding 1 mole ethyl alcohol in 9 mole water. The mass percent of solute in the solution is ....... (Integer answer) (Given : Molar mass in \(g mol ^{-1}\) Ethyl alcohol : \(46\) water: \(18\)\()\)
[JEE Main 2024, 08 Apr (Shift 2)]
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Molality of \(0.8 M ~H _2 SO _4\) solution (density \(1.06{\mathrm{gcm}}^{-3}\)) is ______ \(\times 10^{-3} m\). (Nearest Integer)
[JEE Main 2024, 29 Jan (Shift 2)]
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1.24 g of \(A{X}_{2}\) (molar mass \(124gmo{l}^{-1}\)) is dissolved in 1 kg of water to form a solution with boiling point of \(100.0156^\circ C\), while 25.4 g of \(A{Y}_{2}\) (molar mass \(250gmo{l}^{-1}\)) in 2 kg of water constitutes a solution with a boiling point of \(100.0260^\circ C\).
\({K}_{b}\left({H}_{2}O\right)=0.52Kkgmo{l}^{-1}\)
Which of the following is correct ?
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30gm \({\mathrm{HNO}}_{3}\)is added to a solution to prepare 75 % w/ w solution having density 1.25 g / mL. Volume of solution is?
Memory Based Question 28/Jan/25 Evening shift
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The density of ' \(x\) ' \(\mathrm{M}\) solution (' \(x\) ' molar) of \(\mathrm{NaOH}\) is \(1.12\mathrm{g}{\mathrm{mL}}^{-1}\), while in molality, the concentration of the solution is \(3\mathrm{m}(3\mathrm{molal})\). Then \(x\) is
(Given : Molar mass of \(\mathrm{NaOH}\) is \(40\mathrm{g}/\mathrm{mol}\) )
[JEE Main 2024, 6 Apr (Shift 1)]
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What is the freezing point depression constant of a solvent 50 g of which contain 1 g of non-volatile solute(M.W: 256 g/mol and depression in freezing point is 0.4 K.
Memory Based Question 28/Jan/25 Morning shift
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A solution is made by mixing one mole of volatile liquid A with \(3\) moles of volatile liquid B. The vapour pressure of pure A is 200 mm Hg and that of the solution is \(500\) mm Hg . The vapour pressure of pure B and the least volatile component of the solution, respectively, are
[JEE Main 2025, 2 Apr (Shift 1)]
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The quantity which changes with temperature is:
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Liquid A and B form an ideal solution. The vapour pressure of pure liquids A and B are \(350\) and\(750\)mm Hg respectively at the same temperature. If \({\mathrm{x}}_{\mathrm{A}}\) and \({x}_{B}\) are the mole fraction of A and B in solution while \({\mathrm{y}}_{\mathrm{A}}\) and \({y}_{B}\) are the mole fraction of A and B in vapour phase then
[JEE Main 2025, 7 Apr (Shift 2)]
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The density of ' \(x\) ' \(\mathrm{M}\) solution (' \(x\) ' molar) of \(\mathrm{NaOH}\) is \(1.12\mathrm{g}{\mathrm{mL}}^{-1}\), while in molality, the concentration of the solution is \(3\mathrm{m}(3\mathrm{molal})\). Then \(x\) is
(Given : Molar mass of \(\mathrm{NaOH}\) is \(40\mathrm{g}/\mathrm{mol}\) )
[JEE Main 2024, 6 Apr (Shift 1)]
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Identify the mixture that shows positive deviations from Raoult's Law
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Lead storage battery contains \(38 \%\) by weight solution of \(H _2 SO _4\). The van't Hoff factor is 2.67 at this concentration. The temperature in Kelvin at which the solution in the battery will freeze is
Given \(K _{ f }=1.8 ~K kg mol ^{-1}\)
[JEE Main 2023, 30 Jan (Shift 2)]
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The number of units, which are used to express concentration of solutions from the following is________
Mass percent, Mole, Mole fraction, Molarity, ppm, Molality.
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How much ethyl alcohol must be added to 1 litre of water so that the solution will freeze at –14°C?
(Kf for water = 1.86 C° /molal)
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A \(6.50\) molal solution of \(\mathrm{KOH}(\mathrm{aq}.)\) has a density of \(1.89\mathrm{g}{\mathrm{cm}}^{-3}\). The molarity of the solution is ......... mol \({\mathrm{dm}}^{-3}\).(Round off to the Nearest Integer).
[Atomic masses: \(\mathrm{K}:39.0\mathrm{u};\mathrm{O}:16.0\mathrm{u};\mathrm{H}:1.0\mathrm{u}\) ]
[JEE Main 2021, 16 Mar (Shift 1)]
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The molality of a \(10 \%( V / V )\) solution of di-bromine solution in \(CCl _4\) (carbon tetrachloride) is ' \(x\) '. \(x =\)________ \(\times 10^{-2} m\). (Nearest Integer)
[Given: molar mass of \(Br _2= 160 g mol ^{-1}\)
atomic mass of \(C =12 ~g mol ^{-1}\)
atomic mass of \(Cl =35.5 ~g mol ^{-1}\)
density of dibromine \(3.2 ~g cm ^{-3}\)
density of \(\left.CCl _4=1.6 ~g cm ^{-3}\right]\)
[JEE Main 2023, 1 Feb (Shift 2)]
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A solution is prepared by adding \(2 g\) of " \(X\) " in 1 mole of water. Mass percent of " \(X\) " in the solution is
[JEE Main 2023, 11 Apr (Shift 2)]
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A solution is prepared by adding \(2 g\) of " \(X\) " in 1 mole of water. Mass percent of " \(X\) " in the solution is
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If \( 8 \mathrm{~g} \) of a non-electrolyte solute is dissolved in \( 114 \mathrm{~g} \) of \( \mathrm{n} \)-octane to reduce its vapour pressure to \( 80 \% \), the molar mass ( \(\mathrm{in}\) \( \mathrm{g} \mathrm{mol}^{-1} \) ) of the solute is [Given that molar mass of \( \mathrm{n} \)-octane is \( 114 \mathrm{~g} \mathrm{~mol}^{-1} \) ]
[Re-NEET 2020]
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If the degree of dissociation of aqueous solution of weak monobasic acid is determined to be 0.3 , then the observed freezing point will be_______\(\%\) higher than the expected/ theoretical freezing point. (Nearest Integer)
[JEE Main 2023, 10 Apr (Shift 1)]
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Mass of Urea \(\left( NH _2 CONH _2\right)\) required to be dissolved in \(1000 g\) of water to reduce the vapour pressure of water by \(25 \%\) is________ g. (Nearest Integer)
(Given: Molar mass of \(\mathrm{N},\mathrm{C},\mathrm{O}\mathrm{and}\mathrm{H}\) are \(14,12,16,1\mathrm{g}/\mathrm{mol}\) respectively)
[JEE Main 2023, 6 Apr (Shift 1)]
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80 mole percent of \(MgCl _2\) is dissociated in aqueous solution. The vapour pressure of 1.0 molal aqueous solution of \(MgCl _2\) at \(38^{\circ} C\) is________ \(mm Hg\). (Nearest Integer)
Given : Vapour pressure of water at \(38^{\circ} C\) is \(50 ~mmHg\)
[JEE Main 2023, 12 Apr (Shift 1)]
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\(10.30 \mathrm{~mg}\) of \(\mathrm{O}_2\) dissolved into a liter of sea water of density \(1.03 \mathrm{~g} / \mathrm{mL}\). The concentration of \(\mathrm{O}_2\) in ppm is...........
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\( 6.023 \times 10^{22} \) molecules are present in \( 10 \mathrm{~g} \) of a substance X. The molarity of a solution containing \( 5 \mathrm{~g} \) of substance X in \( 2 \mathrm{~L} \) solution is ____\( \times 10^{-3} \) M
[JEE Main 2020, 3 Sep (Shift 2)]
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An open beaker of water in equilibrium with water vapour is in a sealed container. When a few grams of glucose are added to the beaker of water, the rate at which water molecules
[JEE Main 2020, 2 Sep (Shift 1)]
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Henry's constant (in kbar) for four gases \(\alpha, \beta, \gamma\) and \(\delta\) in water at \(298 K\) is given below:
\[\begin{array}{c|c|c|c|c} & \alpha & \beta & \gamma & \delta \\\hline K _{ H } & 50 & 2 & 2 \times 10^{-5} & 0.5\end{array}\]
(density of water \(=10^3 kg m ^{-3}\) at \(298 K\))
Choose the correct statements
(A) \(\alpha\) has the highest solubility in water at a given pressure
(B) Solubility of \(\gamma\) at 308 K is lower than at 290 K
(C) The pressure of \(\delta\) a 55.5 molal solution of is 250 bar
(D) The pressure of a 55.5 molal solution of \(\gamma\) is 1 bar
[JEE Main 2020, 3 Sep (Shift 1)]
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The freezing point of equimolal aqueous solutions will be highest for
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The following solutions were prepared by dissolving \( 10 \mathrm{~g} \) of glucose \( \left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right) \) in \( 250 \mathrm{~ml} \) of water \( \left(\mathrm{P}_{1}\right), 10 \mathrm{~g} \) of urea \( \left(\mathrm{CH}_{4}\mathrm{~N}_{2} \mathrm{O}\right) \) in \( 250 \mathrm{~ml} \) of water \( \left(\mathrm{P}_{2}\right) \) and \( 10 \mathrm{~g} \) of sucrose \( \left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) \) in \( 250 \mathrm{~ml} \) of water \( \left(\mathrm{P}_{3}\right) \). The right option for the decreasing order of osmotic pressure of these solutions is
[NEET 2021]
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The freezing point depression constant \( \left(\mathrm{K}_{f}\right) \) of benzene is \( 5.12 \) \( \mathrm{K} \mathrm{kg} \mathrm{mol}{ }^{-1} \). The freezing point depression for the solution of molality \( 0.078 \mathrm{~m} \) containing a non-electrolyte solute in benzene is (rounded off upto two decimal places) :
[NEET 2020]
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\(50 ~mL\) of 0.2 molal urea solution (density \(=1.012 ~g mL ^{-1}\) at \(300 K\) ) is mixed with \(250 ~mL\) of a solution containing \(0.06~g\) of urea. Both the solutions were prepared in the same solvent. The osmotic pressure (in Torr) of the resulting solution at \(300 K\) is______
[Use : Molar mass of urea \(=60 ~g mol ^{-1}\); gas constant, \(R =62 ~L Torr K ^{-1} mol ^{-1}\); Assume, \(\left.\Delta_{\text {mix }} H =0, \Delta_{\text {mix }} V =0\right]\)
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Solution of \(12 g\) of non- electrolyte (A) prepared by dissolving it in \(1000~mL\) of water exerts the same osmotic pressure as that of \(0.05 M\) glucose solution at the same temperature. The empirical formula of \(A\) is \(CH _2 O\). The molecular mass of \(A\) is________g. (Nearest Integer)
[JEE Main 2023, 13 Apr (Shift 1)]
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Which one of the following \( 0.06 \mathrm{~M} \) aqueous solutions has lowest freezing point?
[JEE Main 2021, 22 Jul (Shift 2)]
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If 80 g of copper sulphate CuSO4⋅5H2O is dissolved in deionised water to make 5 L of solution. The concentration of the copper sulphate solution is \(\mathrm{x}\times {10}^{-3}\mathrm{mol}/\mathrm{L}\). The value of x is [Atomic masses Cu : 63.54u, S:32u, O:16u, H:1u]
[JEE Main 2021, 1 Sep (Shift 2)]
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\(4.5 g\) of compound \(A(M W=90)\) was used to make \(250 ~mL\) of its aqueous solution. The molarity of the solution in \(M\) is \(x \times 10^{-1}\). The value of \(x\) is (Rounded off to the nearest integer)
[JEE Main 2021, 24 Feb (Shift 1)]
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Liquids A and B form an ideal solution in the entire composition range. At 350 K , the vapor pressures of pure A and pure B are \(7\times {10}^{3}\mathrm{Pa}\mathrm{and}12\times {10}^{3}\mathrm{Pa}\), respectively. The composition of the vapour is in equilibrium with a solution containing 40 mole percent of at this temperature is:
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A solute A dimerizes in water. The boiling point of a 2 molal solution of \( \mathrm{A} \) is \( 100.52^{\circ} \mathrm{C} \). The percentage association of \( A \) is ____ (Round off to the Nearest Integer). [Use: \( \mathrm{K}_{\mathrm{b}} \) for water \( =0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} \)
Boiling point of water \( \left.=100^{\circ} \mathrm{C}\right] \)
[JEE Main 2021, 18 Mar (Shift 2)]
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\(\begin{array}{|c|c|c|}\hline \begin{array}{l}\text { Match List-I with List-II. } \\\text { List-I }\end{array} & & \begin{array}{l}\text { List-II }\end{array} \hline \text { (A) Van't Hoff Factor, i } & \text { (I) } & \text { Cryoscopic constant } \hline \text { (B) } k _{ f } & \text { (II) } & \text { Isotonic solutions } \hline \text { C) Solutions with same } & \text { (III) } & \text { Normal molar mass } \hline & & \overline{\text { Abnormal molar mass }} \hline \text { D) Azeotropes } & \text { (IV) } & \begin{array}{l}\text { Solutions with same } \\\text { composition of vapour } \\\text { above it }\end{array} \hline\end{array}\)
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If the concentration of glucose \(\left({\mathrm{C}}_{6}{\mathrm{H}}_{12}{\mathrm{O}}_{6}\right)\) in blood is 0.72 gL–1, the molarity of glucose in blood is_______ ×10–3M. (Nearest Integer)
(Given: Atomic mass of C = 12u, H = 1u, O = 16u)
[JEE Main 2021, 22 Jul (Shift 2)]
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\(100 ~mL\) of \(Na _3 PO _4\) solution contains \(3.45 g\) of sodium. The molarity of the solution is__________ \(\times 10^{-2} mol L ^{-1}\), (Nearest Integer)
[Atomic Masses - \(Na : 23.0 ~u , O : 16.0 ~u , P : 31.0 ~u\) ]
[JEE Main 2021, 26 Aug (Shift 2)]
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\( 224 \mathrm{~mL} \) of \( \mathrm{SO}_{2(\mathrm{~g})} \) at \( 298 \mathrm{~K} \) and \( 1 \mathrm{~atm} \) is passed through \( 100 \mathrm{~mL} \) of \( 0.1 \mathrm{~M} \mathrm{~NaOH} \) solution. The non-volatile solute produced is dissolved in \( 36 \mathrm{~g} \) of water. The lowering of vapour pressure of solution (assuming the solution is dilute) \( \left(\mathrm{P}_{\left(\mathrm{H}_{2} \mathrm{O}\right)}^{\mathrm{O}}=24 \mathrm{~mm}\right. \) of \( \left.\mathrm{Hg}\right) \) is \( \mathrm{x} \times 10^{-2} \mathrm{~mm} \) of \( \mathrm{Hg} \), the value of \( \mathrm{x} \) is ...... (Integer answer)
[JEE Main 2021, 26 Feb (Shift 1)]
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A 1 molal \( \mathrm{K}_{4} \mathrm{Fe}(\mathrm{CN})_{6} \) solution has a degree of dissociation of 0.4 . Its boiling point is equal to that of another solution which contains 18.1 weight percent of a non electrolytic solute \( \mathrm{A} \). The molar mass of \( \mathrm{A} \) is ___u. (Round off to the Nearest Integer). [Density of water \( =1.0 \mathrm{~g} \mathrm{~cm}^{-3} \) ]
[JEE Main 2021, 17 Mar (Shift 2)]
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If the boiling points of two solvents \(X\) and \(Y\) (having same molecular weights) are in the ratio \(2: 1\) and their enthalpy of vaporizations are in the ratio \(1: 2\), then the boiling point elevation constant of \(X\) is \(m\) times the boiling point elevation constant of \(Y\). The value of \(m\) is_______(Nearest Integer)
[JEE Main 2023, 8 Apr (Shift 2)]
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The molarity of the solution prepared by dissolving \( 6.3 \mathrm{~g} \) of oxalic acid \( \left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}\right) \) in \( 250 \mathrm{~mL} \) of water in \( \mathrm{molL}^{-1} \) is \( \mathrm{x} \times 10^{-2} \). The value of \( \mathrm{x} \) is (Nearest integer) [Atomic mass: \( \mathrm{H}: 1.0, \mathrm{C}: 12.0,0: 16.0 \) ]
[JEE Main 2021, 31 Aug (Shift 1)]
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The water having more dissolved \({\mathrm{O}}_{2}\) is:
[JEE Main 2021, 22 Jul (Shift 2)]
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\( \mathrm{AB}_{2} \) is \( 10 \% \) dissociated in water to \( \mathrm{A}^{2+} \) and \( \mathrm{B}^{-} \). The boiling point of a 10.0 molal aqueous solution of \( \mathrm{AB}_{2} \) is _____\( { }^{\circ} \mathrm{C} \). (Round off to the Nearest Integer)
[Given: Molal elevation constant of water, \({\mathrm{K}}_{\mathrm{b}}=0.5\mathrm{K}{\mathrm{Kgmol}}^{-1}\), boiling point of pure water \( \left.=100^{\circ} \mathrm{C}\right] \)
[JEE Main 2021, 16 Mar (Shift 1)]
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An aqueous solution of volume \(300 \mathrm{~cm}^3\) contains \(0.63 \mathrm{~g}\) of protein. The osmotic pressure of the solution at \(300 \mathrm{~K}\) is 1.29 mbar. The molar mass of the protein is ______\(\mathrm{g} \mathrm{mol}^{-1}\)
Given : \(\mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{K}^{-1} \mathrm{~mol}^{-1}\)
[JEE Main 2023, 10 Apr (Shift 2)]
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What weight of glucose must be dissolved in \(100 g\) of water to lower the vapour pressure by \(0.20 ~mm Hg\) ?
(Assume dilute solution is being formed)
Given: Vapour pressure of pure water is \(54.2 ~mm Hg\) at room temperature. Molar mass of glucose is \(180 ~g mol ^{-1}\)
[JEE Main 2023, 11 Apr (Shift 2)]
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Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R)
Assertion A: \(3.1500 ~g\) of hydrated oxalic acid dissolved in water to make \(250.0 ~mL\) solution will result in \(0.1 ~M\) oxalic acid solution.
Reason R: Molar mass of hydrated oxalic acid is \(126 ~g mol ^{-1}\).
In the light of the above statements, choose the correct answer from the options given below
[JEE Main 2023, 10 Apr (Shift 2)]
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The number of units, which are used to express concentration of solutions from the following is
Mass percent, Mole, Mole fraction, Molarity, ppm, Molality
[JEE Main 2023, 24 Jan (Shift 2)]
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\( 1.22 \mathrm{~g} \) of an organic acid is separately dissolved in \( 100 \mathrm{~g} \) of benzene \( \left(\mathrm{K}_{\mathrm{b}}=2.6 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right) \) and \( 100 \mathrm{~g} \) of acetone \( \left(\mathrm{K}_{\mathrm{b}}=1.7 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right) \). The acid is known to dimerize in benzene but remain as a monomer in acetone. The boiling point of the solution in acetone increases by \( 0.17^{\circ} \mathrm{C} \). The increase in boiling point of solution in benzene in \( { }^{\circ} \mathrm{C} \) is \( \mathrm{x} \times 10^{-2} \). The value of \( \mathrm{x} \) is ........ (Nearest integer) [Atomic mass: \( \mathrm{C}=12.0, \mathrm{H}=1.0, \mathrm{O}=16.0 \) )
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A solution containing \(2 g\) of a non-volatile solute in \(20 g\) of water boils at \(373.52 K\). The molecular mass of the solute is ...................g/mol (Nearest Integer)
(Given, water boils at \(373\mathrm{K}\) and \({\mathrm{K}}_{\mathrm{b}}\) for water \(0.52\mathrm{K}\mathrm{Kg}{\mathrm{mol}}^{-1}\))
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Sea water contains 29.25% NaCl and 19% MgCl2 by weight of solution. The normal boiling point of the sea water is (in °C) (Nearest Integer) Assume 100 % ionization for both NaCl and MgCl2
Given: \(K _{ b }\left( H _2 O \right)=0.52 ~K kg mol ^{-1}\)
Molar mass of NaCl and MgCl2 is 58.5 and 95 g mol–1 respectively
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\(20 \%\) of acetic acid is dissociated when its \(5 g\) is added to \(500 ~mL\) of water. The depression in freezing point of such water is__________ \(\times 10^{-3}\) \({}^{\mathrm{o}}\mathrm{C}\). Atomic mass of \(C , H\) and \(O\) are \(12,1,16\mathrm{amu}\)
[Given: Molal depression constant and density of water are \(1.86 ~K kg mol ^{-1}\) and \(1 ~gcm ^{-3}\) respectively]
[JEE Main 2023, 1 Feb (Shift 2)]
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The enthalpy change for the adsorption process and micelle formation respectively are
[JEE Main 2023, 10 Apr (Shift 1)]
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In the depression of freezing point experiment
(A) Vapour pressure of the solution is less than that of pure solvent
(B) Vapour pressure of the solution is more than that of pure solvent
(C) Only solute molecules solidify at the freezing point
(D) Only solvent molecules solidify at the freezing point
[JEE Main 2023, 24 Jan (Shift 1)]
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1 molal aqueous solution of an electrolyte \( \mathrm{A}_{2} \mathrm{B}_{3} \) is \( 60 \% \) ionised. The boiling point of the solution at \( 1 \mathrm{~atm} \) is ....... K. (Rounded-off to the nearest integer) [Given: \( \mathrm{K}_{\mathrm{b}} \) for \( \left(\mathrm{H}_{2} \mathrm{O}\right)=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} \) ]
[JEE Main 2021, 25 Feb (Shift 1)]
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\(0.004 ~M ~K _2 SO _4\) solution is isotonic with \(0.01 ~M\) glucose solution. Percentage dissociation of \(K _2 SO _4\) is _________ (Nearest Integer)
[JEE Main 2023, 11 Apr (Shift 1)]
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The total pressure of a mixture of non-reacting gases \(X (0.6 g )\) and \(Y (0.45 g )\) in a vessel is \(740 mm\) of \(Hg\). The partial pressure of the gas \(X\) is______ \(mm\) of \(Hg\). (Nearest Integer)
(Given : molar mass \(X =20\) and \(Y =45 g mol ^{-1}\) )
[JEE Main 2023, 31 Jan (Shift 1)]
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Given below are two statements
Statement (I) : Molal depression constant \({\mathrm{K}}_{\mathrm{f}}\) is given by \(\frac{{M}_{1}R{T}_{f}}{\Delta {S}_{\text{fus }}}\), where symbols have their usual meaning.
Statement (II) : \({\mathrm{K}}_{\mathrm{f}}\) for benzene is less than the \({\mathrm{K}}_{\mathrm{f}}\) for water.
In the light of the above statements, choose the most appropriate answer from the options given below
[JEE Main 2025, 4 Apr (Shift 2)]
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At \( 35^{\circ} \mathrm{C} \), the vapour pressure of \( \mathrm{CS}_{2} \) is \( 512 \mathrm{~mm} \mathrm{Hg} \) and that of acetone is \( 344 \mathrm{~mm} \mathrm{Hg} \). A solution of \( \mathrm{CS}_{2} \) in acetone has a total vapour pressure of \( 600 \mathrm{~mm} \mathrm{Hg} \). The false statement amongst the following is:
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Consider the following pairs of solution which will be isotonic at the same temperature. The number of pairs of solutions is/are
(a) \(1 M\) aq. \(NaCl\) and \(2 M\) aq. Urea
(b) \(1 M\) aq. \(CaCl _2\) and \(1.5 M\) aq. \(KCl\)
(c) \(1.5 M\) aq. \(AlCl _3\) and \(2 M\) aq. \(Na _2 SO _4\)
(d) \(2.5 M\) aq. \(KCl\) and \(1 M\) aq. \(Al _2\left( SO _4\right)_3\)
[JEE Main 2023, 6 Apr (Shift 2)]
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When \( 12.2 \mathrm{~g} \) of benzoic acid is dissolved in \( 100 \mathrm{~g} \) of water, the freezing point of solution was found to be \( -0.93^{\circ} \mathrm{C} \) \( \left(\mathrm{K}_{\mathrm{f}}\left(\mathrm{H}_{2} \mathrm{O}\right)=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right) \). The number (n) of benzoic acid molecules associated (assuming 100 % association) is
[JEE Main 2021, 26 Feb (Shift 2)]
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