List of top Chemistry Questions on Solutions asked in JEE Advanced

Vessel-1 contains w₂ g of a non-volatile solute X dissolved in w₁ g of water. Vessel-2 contains w₂ g of another non-volatile solute Y dissolved in w₁ g of water. Both the vessels are at the same temperature and pressure. The molar mass of X is 80% of that of Y. The van’t Hoff factor for X is 1.2 times of that of Y for their respective concentrations.
The elevation of boiling point for solution in Vessel-1 is _____ % of the solution in Vessel-2.

For He⁺, a transition takes place from the orbit of radius 105.8 pm to the orbit of radius 26.45 pm. The wavelength (in nm) of the emitted photon during the transition is ___. 
[Use: Bohr radius, a = 52.9 pm, Rydberg constant, 𝑅H = 2.2 × 10⁻¹⁸ J, Planck’s constant, h = 6.6 × 10⁻³⁴ J s, Speed of light, c = 3 × 10⁸ m s⁻¹]

For He⁺, a transition takes place from the orbit of radius 105.8 pm to the orbit of radius 26.45 pm. The wavelength (in nm) of the emitted photon during the transition is ___. 
[Use: Bohr radius, a = 52.9 pm, Rydberg constant, 𝑅H = 2.2 × 10⁻¹⁸ J, Planck’s constant, h = 6.6 × 10⁻³⁴ J s, Speed of light, c = 3 × 10⁸ m s⁻¹]

Concentration of $H _2 SO _4$ and $Na _2 SO _4$ in a solution is $1 M$ and $1.8 \times 10^{-2} M$, respectively. Molar solubility of $PbSO _4$ in the same solution is $X \times 10^{- Y } M$ (expressed in scientific notation). The value of $Y$ is ________. [Given: Solubility product of $PbSO _4\left(K_{s p}\right)=1.6 \times 10^{-8}$ For $H _2 SO _4, K_{a l}$ is very large and $\left[K_{a 2}=1.2 \times 10^{-2}\right]$

The correct statement(s) related to colloids is(are)

The boiling point of water in a $01$ molal silver nitrate solution (solution $A$ ) is $x ^{\circ} C$ To this solution $A$, an equal volume of $01$ molal aqueous barium chloride solution is added to make a new solution $B$ The difference in the boiling points of water in the two solutions $A$ and $B$ is $y \times 10^{-2}{ }^{\circ} C$ (Assume: Densities of the solutions $A$ and $B$ are the same as that of water and the soluble salts dissociate completely Use: Molal elevation constant (Ebullioscopic Constant), $K _{ b }=05 \,K \,kg\, mol ^{-1}$; Boiling point of pure water as $100^{\circ} C$)
The value of $x$ is ______$^{\circ}C$

At 298 K, the limiting molar conductivity of a weak monobasic acid is 4 × 10² S cm² mol^–1. At 298 K, for an aqueous solution of the acid, the degree of dissociation is a and the molar conductivity is y × 10² S cm² mol^–1. At 298 K, upon 20 times dilution with water, the molar conductivity of the solution becomes 3y × 10² S cm² mol^–1.

The boiling point of water in a $0.1$ molal silver nitrate solution (solution $A$ ) is $x ^{\circ} C$. To this solution $A$, an equal volume of $0.1$ molal aqueous barium chloride solution is added to make a new solution $B$. The difference in the boiling points of water in the two solutions $A$ and $B$ is $y \times 10^{-2}{ }^{\circ} C$
(Assume: Densities of the solutions $A$ and $B$ are the same as that of water and the soluble salts dissociate completely
Use: Molal elevation constant (Ebullioscopic Constant), $K _{ b }=0.5 \,K \,kg\, mol ^{-1}$; Boiling point of pure water as $100^{\circ} C$)

A colorless aqueous solution contains nitrates of two metals, $X$ and $Y$. When it was added to an aqueous solution of $NaCl$, a white precipitate was formed. This precipitate was found to be partly soluble in hot water to give a residue $P$ and a solution $Q$. The residue $P$ was soluble in aq $NH _{3}$ and also in excess sodium thiosulfate. The hot solution $Q$ gave a yellow precipitate with $KI$. The metals $X$ and $Y$, respectively, are

$5.00\, mL$ of $0.10 \,M$ oxalic acid solution taken in a conical flask is titrated against $NaOH$ from a burette using phenolphthalein indicator. The volume of $NaOH$ required for the appearance of permanent faint pink color is tabulated below for five experiments. What is the concentration, in molarity, of the $NaOH$ solution? 
 

Exp. No.	Vol. of NaOH (mL)
1	12.5
2	10.5
3	9.0
4	9.0
5	9.0

Liquid $A$ and $B$ form ideal solution for all compositions of $A$ and $B$ at $25^{\circ} C$. Two such solutions with $025$ and $050$ mole fractions of $A$ have the total vapour pressures of $03$ and $04$ bar, respectively. What is the vapour pressure of pure liquid $B$ in bar?

For a solution formed by mixing liquids $L$ and $M$, the vapour pressure of $L$ plotted against the mole fraction of $M$ in solution is shown in the following figure. Here $x _{ L }$ and $x _{ M }$ represent mole fractions of $L$ and $M$, respectively, in the solution. The correct statement $(s)$ applicable to this system is (are)

Benzene and naphthalene form an ideal solution at room temperature. For this process, the true statement(s) is (are)

For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in 100g of water, the elevation in boiling point at 1 atm pressure is 2$^{\circ}$C. Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is (take $K_b = 0.76 K kg mol^{-1}).$

The species which by definition has zero standard molar enthalpy of formation at $298 \,K$ is

0.004 MNa$_2SO_4$ is isotonic with 0.01 M glucose. Degree of dissociation of Na$_2SO_4$ is

During depression of freezing point in a solution the following are in equilibrium

In the depression of freezing point experiment, it is found that the

When mercuric iodide is added to the aqueous solution of potassium iodide

A molal solution is one that contains one mole of a solute in

An azeotropic solution of two liquids has boiling point lower than either of them when it