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An aqueous solution of a weak monobasic acid containing $0.1 \text{ g}$ in $21.7 \text{ g}$ of water freezes at $272.817 \text{ K}$. If the value of $K_f$ for water is $1.86 \text{ K kg mol}^{-1}$, the molecular mass of the acid is:
Which one of the following is incorrect for an ideal solution?
Which of the following statements about the composition of the vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume that the temperature is constant at $25^\circ\text{C}$. (Given, vapour pressure data at $25^\circ\text{C}$, benzene = $12.8 \text{ kPa}$, toluene = $3.85 \text{ kPa}$)
The depression in freezing point of 0.01 M aqueous solutions of urea, sodium chloride and sodium sulphate is in the ratio of:
A solution of acetone in ethanol:
One mole of sugar is dissolved in three moles of water at 298 K. The relative lowering of vapour pressure is:
The Henry's law constant for the solubility of $N_2$ gas in water at $298 \text{ K}$ is $1.0 \times 10^5 \text{ atm}$. The mole fraction of $N_2$ in air is $0.8$. The number of moles of $N_2$ formed from air dissolved in $10 \text{ moles}$ of water at $298 \text{ K}$ and $5 \text{ atm}$ pressure is:
$K_H$ values for some gases at the same temperature 'T' are given: Gas : $K_H$/k bar Ar : 40.3 $CO_2$ : 1.67 HCHO : $1.83 \times 10^{-5}$ $CH_4$ : 0.413 $K_H$ is Henry's Law constant in water. The order of their solubility in water is :
The Henry's law constant $K_H$ values of three gases (A, B, C) in water are 145, $2 \times 10^{-5}$, and 35 kbar, respectively. Determine the order of solubility of these gases in water from highest to lowest:
The plot of osmotic pressure ($\pi$) vs concentration ($\text{mol L}^{-1}$) for a solution gives a straight line with slope $25.73 \text{ L bar mol}^{-1}$. The temperature at which osmotic pressure measurement is done is: (Use $R=0.083 \text{ L bar mol}^{-1} \text{ K}^{-1}$)
An aqueous solution of $6.3 \text{ g}$ oxalic acid dihydrate is made up to $250 \text{ mL}$. The volume of $0.1 \text{ N NaOH}$ required to completely neutralize $10 \text{ mL}$ of this solution is
Camphor is often used in molecular mass determination because:
200 mL of an aqueous solution contains 1.26 g of protein. The osmotic pressure of this solution at 300 K is found to be 2.57 × 10⁻³ bar. The molar mass of protein will be: (Use: R = 0.083 L bar mol⁻¹ K⁻¹)
The addition of water vapour does not change the density of:
In which case change in entropy is negative?
Identify the correct order of solubility in aqueous medium:
Select the correct match
Which of the following is a secondary pollutant?
Natality refers to
The formation of an ideal solution from components A and B indicates: