Solutions

What is the molal elevation constant of solvent ?

If a solution is prepared by dissolving solute in 0.3 L of water having osmotic pressure 164.1 atm at 300 K, what will be the number of moles of solute in solution? (R = 0.08205 L atm K$^{-1}$mol$^{-1}$)

What is the molality of an aqueous solution containing 6 % glucose by mass ? (Molar mass of glucose = 180 g/mol)

The molal elevation constant for water is $0.52$ $^\circ$C kg mol$^{-1}$. Find out the boiling point of solution when $6.0$ g of urea is dissolved in $200$ g of water. (molar mass of urea $= 60$ g/mol)

What is the osmotic pressure of $0.25$ M urea solution at $27^\circ$C ($R = 0.0821\ \text{L atm mol}^{-1}\text{K}^{-1}$)?

A solution contains 50 g of common salt in 500 gm of water. Find the concentration of the solution in terms of percentage?

Calculate relative lowering of vapor pressure of 1 molal glucose solution in water at room temperature. (molar mass of water $=18$)

Calculate the pressure at which solubility of a certain gas in water is 0.165 mol L$^{-1}$ at $25\ ^\circ$C. (Henry's law constant for this gas in water is 0.034 mol L$^{-1}$bar$^{-1}$ at $25\ ^\circ$C.)

Which of the following laws describes the relationship between solubility of gas in a liquid and the pressure of the gas over the solution at a given temperature?

The maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does NOT depend upon

For a solution containing a non-volatile solute in a volatile solvent, which of the following relationships is correctly represented?

Which of the following statements is NOT true about 0.05 M urea solution & 0.1 M glucose solution?