List of top Chemistry Questions on Types of Solutions asked in KEAM

Isotonic solutions have identical
Which of the following aqueous non-electrolyte solution will produce the highest freezing point if 20g of the solute is dissolved in 1000g of water?
The molarity of an aqueous solution containing 0.4g of NaOH (molar mass=40g/mol) in 250mL of a solution is
Hypertonic solution contains
Molal boiling point elevation is the least for the solvent
What is the mass of ethanoic acid required to prepare $0.5\,m$ solution containing $100\,g$ of water? (Molar mass of ethanoic acid = $60\,g\,mol^{-1}$)
What is the volume of methanol needed for making $2\,L$ of $0.4\,M$ solution? (Density of methanol $= 0.64\,kg\,L^{-1}$ and molar mass $= 32\,g\,mol^{-1}$)
3 g of benzoic acid is added to 25 g of benzene. \( \Delta T_f = 2.5\,\text{K} \) and \( K_f \) of benzene is 5. What is the experimental molecular mass of benzoic acid?
Find the mass of an organic compound of molar mass 84, required to prepare 250 ml solution of molarity 0.4
The osmotic pressure of \( 0.01\,M \) aqueous solution of urea at \( 300\,K \) is \((R = 0.082\,\text{lit atm mol}^{-1}\text{K}^{-1})\)
The binary liquid mixture that has positive deviation from Raoult's law is
Which of the following solvent has highest value of molal elevation constant \( K_b \)?
The density of \( 3\,M \) aqueous solution of a solute \( X \) is \( 1.86\,\text{g mL}^{-1} \). The molality of the solution is (Molar mass of solute \( X \) is \( 120\,\text{g mol}^{-1} \))
What is the mass of the substance 'X' required to prepare 250 mL of 0.5 molar aqueous solution? (Molar mass of 'X' is \(40 \mathrm{g} \mathrm{mol}^{- 1}\))
Which of the following gas has highest solubility in water at 298 K?
When the same amount of the solute \(P\) and \(Q\) are separately dissolved in 500 g water, the \(\Delta T_f\) values are 0.15 K and 0.30 K respectively. If the molecular weight of \(P\) is 80 g mol\(^{-1}\), then the molecular weight of \(Q\) is
A solution is prepared by dissolving 20 g NaOH in 1250 mL of a solvent of density 0.8 g/mL. Then the molality of the solution is
A solution of methanol in water is 20 % by volume. If the solution and pure methanol have densities of \( 0.964\text{ kg L}^{-1} \) and \( 0.793\text{ kg L}^{-1} \), respectively, find the per cent of methanol by weight?
The Henry's law constant for O\(_2\) dissolved in water is \( 4.34 \times 10^4\text{ atm} \) at certain temperature. If the partial pressure of O\(_2\) in a gas mixture that is in equilibrium with water is \( 0.434\text{ atm} \), what is the mole fraction of O\(_2\) in the solution?
Acetic acid dimerizes when dissolved in benzene. As a result boiling point of the solution rises by \( 0.36^\circ \text{C} \), when 100 g of benzene is mixed with "X" g of acetic acid. In this solution, if experimentally measured molecular weight of acetic acid is 117.8 and molar elevation constant of benzene is 2.57 K kg mol\(^{-1} \), what is the weight % and degree of dissociation (in %) of acetic acid in benzene?
The freezing point of equimolal aqueous solutions will be highest for
The molality of the 3M solution of methanol if the density of the solution is $0.9\ \text{g cm}^{-3}$ is}
Calculate the molality of a solution that contains 51.2 g of naphthalene (C$_{10}$H$_8$), in 500 mL of carbon tetrachloride. The density of CCl$_4$ is 1.60 g/mL.
31 g of ethylene glycol (C$_2$H$_6$O$_2$) is mixed with 500 g of solvent ($K_f = 2$ K kg mol$^{-1}$). What is the freezing point of the solution in K? (Freezing point of solvent = 273 K)
18 g of glucose is dissolved in 178.2 g of water. The vapour pressure of the solution at 100$^\circ$C is (vapour pressure of pure water at 100$^\circ$C is 760 mm Hg)