A student mixes 300 g of an aqueous solution containing 25% solute by mass with 400 g of another aqueous solution of the same solute, which is 40% by mass. What is the approximate mass percentage of the solvent in the resulting mixture?
1.
66.43 %
2.
36.54 %
3.
12.45 %
4.
33.97 %
At 350 K, the vapour pressures of two volatile pure liquids, A and B, are 450 mm Hg and 700 mm Hg, respectively. If these liquids are mixed to form an ideal solution with a total equilibrium vapour pressure of 600 mm Hg, what are the respective mole fractions of A and B in the liquid phase?
| 1. | \(x_{A} = 0 . 2 ; x_{B } = 0 . 8\) | 2. | \(x_{A} = 0 . 8 ; x_{B} = 0 . 2\) |
| 3. | \(x_{A } = 0 . 4 ; x_{B} = 0 . 6\) | 4. | \(x_{A } = 0 . 6 ; x_{B } = 0 . 4\) |
The vapour pressure of water in the solution having 50 g of urea dissolved in 850 g of water is:
(Vapor pressure of pure water at 298 K is 23.8 mm Hg)
1. 23.40 mm of Hg
2. 33.46 mm of Hg
3. 12.76 mm of Hg
4. 87.12 mm of Hg
The amount of sucrose is to be added to 500 g of water such that it boils at 100°C is:
( Given: The boiling point of water at 750 mm Hg is 99.63°C ; Kb = 0.52 K kg mol-1)
1. 145.76 g
2. 213.54 g
3. 121.67 g
4. 195.36 g
The solubility of gases in liquids generally decreases as temperature increases.
The primary reason for this behavior is:
| 1. | Dissolution of a gas in a liquid is an endothermic process. |
| 2. | Dissolution of a gas in a liquid is an exothermic process. |
| 3. | Gases are highly compressible. |
| 4. |
All of the above statements are correct. |
To minimize the painful effects accompanying deep sea diving, oxygen diluted with less soluble helium gas is used as breathing gas by the divers. This is an example of the application of:
| 1. | Raoult's law | 2. | Henry's law |
| 3. | Ideal gas Equation | 4. | All of the above |
| Type of solution | Example | ||
| a. | Solid in gas | i. | Aerated water |
| b. | Gas in liquid | ii. | Smoke |
| c. | Liquid in solid | iii. | Solution of hydrogen in palladium |
| d. | Gas in solid | iv. | Amalgams |
| a | b | c | d | |
| 1. | i | iii | iv | ii |
| 2. | ii | i | iv | iii |
| 3. | iii | i | iv | ii |
| 4. | iv | i | ii | iii |
An example of a gas in a solid-type solution is:
1. Solution of hydrogen in palladium
2. Ethanol dissolved in water
3. Camphor vapours in N2 gas
4. Amalgams
| 1. | \(\text X_{\text{mole fraction}}=\frac{\text n_{\text{solute}}}{\text n_{\text{solution}}}\) |
| 2. | \(\text{Molarity}=\frac{\text{amount of solute (g)}}{\text{volume of solution (mL)}}\) |
| 3. | \(\text{Molality}=\frac{\text{Number of mole of solute}}{\text{amount of solvent (kg)}}\) |
| 4. | \(\text{Mass percentage}=\frac{\text{mass of the component in the solution}}{\text{Total mass of the solution}}\times100 \) |
The density of 68 % nitric acid by mass in an aqueous solution is 1.504 g mL–1. The molarity of the acid solution would be:
1. 15.24 M
2. 16.23 M
3. 14.52 M
4. 13.45 M
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