List of top Chemistry Questions on Solutions

At 293 K, HCl(g) is dissolved in cyclohexane. Identify the graph obtained for this solution (x-axis = mole fraction of HCl dissolved in cyclohexane; y-axis = partial pressure of HCl(g)).
If two liquids \(A\) and \(B\) have \[ P_A^\circ:P_B^\circ=1:2 \] and have mole fraction in solution as \(1:2\), then mole fraction of \(B\) in vapour phase is
The relative lowering of vapour pressure of an aqueous solution containing a non-volatile solute is 0.0125. The molality of the solution is
At $300\,\mathrm{K}$, a certain reaction has an equilibrium constant equal to 10. The value of $\Delta G^\circ$ for this reaction (in $\mathrm{kJ\,mol^{-1}}$) is:} \[ (R=8.314\,\mathrm{J\,K^{-1}mol^{-1}}) \]
When the bottle of soft drink is opened, what would take place from the following?
(A) Solubility of dissolved gas decreases.
(B) bottle released internal pressure.
(C) effervences evolved from the bottle.
(D) increase in external pressure.
Identify the correct choice.
Calculate the solubility of certain gas in solvent with pressure \(3\) atm at \(25^{\circ}\text{C}\) (Henry's law constant is \(3.0\times 10^{-2}\,\text{mol dm}^{-3}\,\text{atm}^{-1}\))
Which from following gases is least soluble in water under same conditions of temperature and pressure ?
Which of the following statements is NOT true about solubility?
Identify a pair of gases from following that does not obey Henry's law.
The partial pressure of a gas at \(25^{\circ}\)C is \(0.18\) atm, calculate the concentration of the gas dissolved at the same temperature,
If \(K_H\) is \(0.15 \text{mol dm}^{-3} \text{atm}^{-1}\)
The solubility of \(\text{N}_2\) gas in water at \(25^{\circ}\)C and \(1\) bar is \(6.85\times 10^{-4}\text{ mol L}^{-1}\). Calculate the solubility of \(\text{N}_2\) gas in water at the same temperature when the partial pressure of \(\text{N}_2\) is \(0.70\) bar
Which of the following aqueous solutions will show maximum vapour pressure at 300K?
Explain with the help of Henry's law: (i) Bends (ii) Anoxia
Define Molal depression constant. 48 g of ethylene glycol (C2H6O2) is dissolved in 600 g of water. Calculate (i) depression in freezing point and (ii) freezing point of the solution. [Given Kf(water) = 1.86 °C kg mol-1]
OR
Define molality and explain mole fraction. Calculate the mole fraction of solute and solvent of a 20% aqueous C2H6O2 solution.
0.32 g of a new compound was dissolved in 25 g of water. The freezing point of this solution was found to be \(-0.201\,^\circ\text{C}\). Determine the molecular weight of this new compound. For water \(K_f = 1.86\,^\circ\text{C}\;\text{kg mol}^{-1}\).
Which of the following solutions will have a maximum boiling point?
An aqueous solution of glucose is 10% (w/w). What would be the molality and mole fraction of each component in the solution? (Molar mass of glucose = 180 g mol⁻¹)
Define molal elevation constant. (2)
Explain reverse osmosis and write any one example of artificial semipermeable membrane. (1+1=2)
Read the following assertion and reason and choose the correct alternative.
Assertion: Elevation in boiling point for two isotonic solutions is same.
Reason: Boiling point depends upon the concentration of the solute.
(i) Explain Henry's law. (ii) 200 ml of an aqueous solution of a protein contains 1.26 g of protein. The osmotic pressure of such a solution at 300 K is found to be 2.57 × 10-3 bar. Calculate the molar mass of the protein. (1+2=3)
Define molality and molarity.
Aqueous solution of sodium chloride boils at higher temperature than water, but it freezes at lower temperature than water. Explain with reason.
Read the following assertion and reason and choose the correct alternative.
Assertion: Osmotic pressure is a colligative property.
Reason: Osmotic pressure is directly proportional to molarity at a given temperature.
If 2 g of benzoic acid is dissolved in 25 g of benzene, its depression in freezing point was found to be 1.62 K. Molal depression constant of benzene is 4.9 K kg mol-1. If benzoic acid forms a dimer in this solution, what will be the percentage association of benzoic acid? (5)
OR
A 200 cm3 aqueous solution of a protein contains 1.26 g of protein. The osmotic pressure of this solution at 300 K is \(2.57\times10^{-3}\) bar. Calculate the molar mass of this protein. (5)