It is given that: Volume of water $(\mathrm{V})=450 \mathrm{~mL}=0.45 \mathrm{~L}$ Temperature (T) $=37+273=310 \mathrm{~K}$ moles of the polymer, $\mathrm{n}=\frac{1}{185000} \mathrm{~mol}$ We know...
How much of sucrose is to be added to 500 g of water such that it boils at 100°C if the molar elevation constant for water is 0.52 K kg mol-1 and the boiling point of water at 750 mm Hg is 99.63°C?
Elevation in boiling point $\Delta T_{b}=(100+273)-(99.63+273)$ $=0.37 \mathrm{~K}$ Mass of water, $w_{1}=500 \mathrm{~g}$ Molar mass of sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22}...
Find the vapor pressure of water and its relative lowering in the solution which is 50 g of urea (NH2CONH2) dissolved in 850 g of water. (Vapor pressure of pure water at 298 K is 23.8 mm Hg)
As we know that vapour pressure of water, $P_{1}^{\infty}=23.8 \mathrm{~mm}$ of $\mathrm{Hg}$ Weight of water, $w_{1}=850 \mathrm{~g}$ Weight of urea, $w_{2}=50 \mathrm{~g}$ Molecular weight of...
The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K. Find out the composition of the liquid mixture if total vapour pressure is 600 mm Hg. Also find the composition of the vapour phase.
As we know that: $P_{A}^{\circ}=450 \mathrm{~mm} \text { of } \mathrm{Hg}$ $P_{B}^{\circ}=700 \mathrm{~mm}$ of $\mathrm{Hg}$ $P_{\text {total }}=600 \mathrm{~mm} \text { of } \mathrm{Hg}$ As...
Calculate Henry’s law constant when the solubility of H2S (a toxic gas with rotten egg like smell) in water at STP is 0.195 m
It is assumed that the solubility of $\mathrm{H}_{2} \mathrm{~S}$ in water at STP is $0.195 \mathrm{~m}$, which means that $0.195 \mathrm{~mol}$ of $\mathrm{H}_{2} \mathrm{~S}$ dissolves in $1000...
If 1.202 g mL^{-1}mL−1 is the density of 20% aqueous KI, determine the following:
(a) Molality of KI (b) Molarity of KI (c) Mole fraction of KI (a) Molar mass of $\mathrm{Kl}=39+127=166 \mathrm{~g} \mathrm{~mol}^{-1}$ $20 \%$ aqueous solution of KI shows that $20 \mathrm{~g}$ of...
To make 2.5 kg of 0.25 molar aqueous solution, determine the mass of urea (NH2CONH2) that is required.
Urea’s molar mass (NH2CONH2) = $2(1 \times 14+2 \times 1)+1 \times 12+1 \times 16=60 \mathrm{~g} \mathrm{~mol}^{-1}$ 0.25 urea in a molar aqueous solution denotes: $1000 \mathrm{~g}$ of water...
Determine the molarity of each of the solutions given below:
(a) 30 g of Co(NO)3. 6H2O in 4.3 L of solution (b) 30 mL of 0.5 M H2SO4 diluted to 500 mL. We are aware of this., Molarity $=\frac{\text { Moles of Solute }}{\text { Volume of solution in litre...
If benzene in solution containing 30% by mass in carbon tetrachloride, calculate the mole fraction of benzene.
Assume benzene has a mass of $30 \mathrm{~g}$ in a solution with a total mass of $100 \mathrm{~g}$. Mass of $\mathrm{CCl}_{4}=(100-30) \mathrm{g}$ $=70 \mathrm{~g}$ benzene’s molar mass...
If 22 g of benzene is dissolved in 122 g of carbon tetrachloride, determine the mass percentage of carbon tetrachloride (CCl4) and benzene (C6H6).
Benzene's mass percent $\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)=\frac{\text { Mass of } C_{6} H_{6}}{\text { Total mass of the solution }} v \times 100$ $=\frac{\text { Mass of } C_{6}...