$${\mathrm{CaCO}}_3(\mathrm{s})+2\mathrm{HCl}(\mathrm{aq})\to {\mathrm{CaCl}}_2(\mathrm{aq})+{\mathrm{CO}}_2(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{l})$$ Consider the above reaction, what mass of ${\mathrm{CaCl}}_2$ will be formed if 250 mL of 0.76 M HCl reacts with 1000 g of ${\mathrm{CaCO}}_3$ ? (Given : Molar mass of $\mathrm{Ca},\mathrm{C},\mathrm{O},\mathrm{H}$ and Cl are $40,12,16,1$ and $35.5\mathrm{g}{\mathrm{mol}}^{-1}$, respectively)

On complete combustion 1.0 g of an organic compound $(\mathrm{X})$ gave 1.46 g of ${\mathrm{CO}}_2$ and 0.567 g of ${\mathrm{H}}_2\mathrm{O}$. The empirical formula mass of compound $(\mathrm{X})$ is __________ g. (Given molar mass in $\mathrm{g}{\mathrm{mol}}^{-1}\mathrm{C}:12,\mathrm{H}:1,\mathrm{O}:16$ )

Among $10^{-9}\mathrm{g}$ (each) of the following elements, which one will have the highest number of atoms? Element: $\mathrm{Pb},\mathrm{Po},\mathrm{Pr}$ and Pt

Mass of magnesium required to produce 220 mL of hydrogen gas at STP on reaction with excess of dil. HCl is Given: Molar mass of Mg is $24\mathrm{g}{\mathrm{mol}}^{-1}$.

10 mL of 2 M NaOH solution is added to 20 mL of 1 M HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and made the volume upto the mark with distilled water. The solution in this flask is :

In Dumas' method for estimation of nitrogen 0.4 g of an organic compound gave 60 mL of nitrogen collected at 300 K temperature and 715 mm Hg pressure. The percentage composition of nitrogen in the compound is (Given : Aqueous tension at $300\mathrm{K}=15\mathrm{mm}\mathrm{Hg}$ )

The purification method based on the following physical transformation is :$\underset{(X)}{\mathrm{Solid}}\stackrel{\text{ Heat }}{\to }\underset{(X)}{\mathrm{Vapour}}\stackrel{\text{ Cool }}{\to }\underset{(X)}{\mathrm{Solid}}$

Given below are two statements : Statement (I): NaCl is added to the ice at 0°C, present in the ice cream box to prevent the melting of ice cream. Statement (II): On addition of NaCl to ice at 0°C, there is a depression in freezing point. In the light of the above statements, choose the correct answer from the options given below :

1.24 g of AX2 (molar mass 124 g mol−1) is dissolved in 1 kg of water to form a solution with boiling point of 100.015°C, while 25.4 g of AY2 (molar mass 250 g mol−1) in 2 kg of water constitutes a solution with a boiling point of 100.0260°C.Kb(H2O) = 0.52 kg mol−1Which of the following is correct?

Arrange the following solutions in order of their increasing boiling points. (i) $10^{-4}\mathrm{M}\mathrm{NaCl}$ (ii) $10^{-4}\mathrm{M}$ Urea (iii) $10^{-3}\mathrm{M}\mathrm{NaCl}$ (iv) $10^{-2}\mathrm{M}\mathrm{NaCl}$

When a non-volatile solute is added to the solvent, the vapour pressure of the solvent decreases by 10 mm of Hg . The mole fraction of the solute in the solution is 0.2 . What would be the mole fraction of the solvent if decrease in vapour pressure is 20 mm of Hg ?

Consider a binary solution of two volatile liquid components 1 and $2.x_1$ and $y_1$ are the mole fractions of component 1 in liquid and vapour phase, respectively. The slope and intercept of the linear plot of $\frac{1}{x_1}$ vs $\frac{1}{y_1}$ are given respectively as :

Consider the given plots of vapour pressure (VP) vs temperature(T/K). Which amongst the following options is correct graphical representation showing $\Delta {\mathrm{T}}_{\mathrm{f}}$, depression in the freezing point of a solvent in a solution?

What is the freezing point depression constant of a solvent, 50 g of which contain 1 g non volatile solute (molar mass $256\mathrm{g}{\mathrm{mol}}^{-1}$ ) and the decrease in freezing point is 0.40 K ?

$\mathrm{HA}(aq)\rightleftharpoons {\mathrm{H}}^{+}(aq)+{\mathrm{A}}^{-}(aq)$The freezing point depression of a 0.1 m aqueous solution of a monobasic weak acid HA is 0.20 °C. The dissociation constant for the acid isGiven: $K_f$(H2O) = 1.8 K kg mol−1, molality ≡ molarity

Which of the following binary mixture does not show the behaviour of minimum boiling azeotropes?

A solution is made by mixing one mole of volatile liquid $A$ with 3 moles of volatile liquid $B$. The vapour pressure of pure A is 200 mm Hg and that of the solution is 500 mm Hg . The vapour pressure of pure B and the least volatile component of the solution, respectively, are:

Which of the following graph correctly represents the plots of ${\mathrm{K}}_{\mathrm{H}}$ at 1 bar for gases in water versus temperature?

' $x$ ' g of NaCl is added to water in a beaker with a lid. The temperature of the system is raised from $1^{\circ }\mathrm{C}$ to $25^{\circ }\mathrm{C}$. Which out of the following plots, is best suited for the change in the molarity $(\mathrm{M})$ of the solution with respect to temperature ? [Consider the solubility of NaCl remains unchanged over the temperature range]

2 moles each of ethylene glycol and glucose are dissolved in 500 g of water. The boiling point of the resulting solution is: (Given : Ebullioscopic constant of water $=0.52\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1}$ )