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An aqueous solution is $1.00$ molal in $\text{KI}$. Which change will cause the vapour pressure of the solution to increase?
The freezing point depression constant ($K_f$) of benzene is $5.12 \text{ K kg mol}^{-1}$. The freezing point depression for the solution of molality $0.078 \text{ m}$ containing a non-electrolyte solute in benzene is:
One mole of sugar is dissolved in three moles of water at 298 K. The relative lowering of vapour pressure is:
A solution containing $10 \text{ g/dm}^3$ of urea (molecular mass $= 60 \text{ g mol}^{-1}$) is isotonic with a $5 \%$ solution of a non-volatile solute. The molecular mass of this non-volatile solute 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:
The correct option for the value of vapour pressure of a solution at 45 °C with benzene to octane in a molar ratio 3:2 is: [At 45 °C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume Ideal gas]
$K_H$ 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 $R=0.083 \text{ L bar mol}^{-1} \text{ K}^{-1}$)
Acidified $K_2Cr_2O_7$ solution turns green when $Na_2SO_3$ is added to it. This is due to the formation of:
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)
When neutral or faintly alkaline $KMnO_4$ is treated with potassium iodide, iodide ion is converted into 'X'. 'X' is:
The addition of water vapour does not change the density of:
Which of the following series of transitions in the spectrum of hydrogen atom fall in visible region?
In which case change in entropy is negative?
Identify the correct order of solubility in aqueous medium:
The vapour pressure of a solvent decreased by 10 mm of Hg when a non-volatile solute was added to the solvent. The mole fraction of the solute in solution is 0.2. What would be the mole fraction of the solvent if the decrease in vapour pressure is 20 mm of Hg?
Out of ‘X’ pairs of ribs in humans only 'Y' pairs are true ribs. Select the option that correctly represents values of X and Y and provides their explanation: