Q. No.If the density of lake water is 1.25 g mL–1 and contains 92 g of Na+ ions per kg of water, then the molality of Na+ ions will be-
| 1. | 3.24 molal | 2. | 4 molal |
| 3. | 5 molal | 4. | 3.5 molal |
The partial pressure of ethane over a solution containing 6.56 × 10–2 g of ethane is 1 bar. If the solution contains 5.00 × 10–2 g of ethane, the partial pressure of the gas will be -
1. 0.66 bar
2. 0.96 bar
3. 0.76 bar
4. 0.19 bar
If the solubility product of CuS is 6 × 10–16, the maximum molarity of CuS in an aqueous solution will be
| 1. | 1.45 × 10−8 mol L−1 | 2. | 3.45 × 10−8 mol L−1 |
| 3. | 2.45 × 10−8 mol L−1 | 4. | 4.25 × 10−8 mol L−1 |
The mass percentage of aspirin (C9H8O4) in acetonitrile (CH3CN) when 6.5 g of C9H8O4 is dissolved in 450 g of CH3CN will be:
| 1. | 1.424% | 2. | 4.424% |
| 3. | 5.124% | 4. | 2.124% |
Nalorphene (C19H21NO3), similar to morphine, is used to combat withdrawal symptoms in narcotic users. The dose of nalorphene generally given is 1.5 mg.
Calculate the mass of 1.5 × 10−3m aqueous solution required for the above dose.
| 1. | 13.22 g | 2. | 3.22 g |
| 3. | 11.22 g | 4. | 9.22 g |
The amount of benzoic acid (C6H5COOH) required for preparing 250 mL of 0.15 M solution in methanol is -
| 1. | 4.57 g | 2. | 3.57 g |
| 3. | 1.57 g | 4. | 12.57 g |
Henry’s law constant for the solution of methane in benzene at 298 K is 4.27 × 105 mm Hg. The mole fraction of methane in benzene at 298 K under 760 mm Hg will be:
1. 1.85 × 10–5
2. 192 × 10–4
3. 178 × 10–5
4. 18.7 × 10–5
The major component of air is nitrogen with approximately 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K. if the Henry’s law constant for nitrogen at 298 K is 6.51 × 107 mm respectively, then the composition of nitrogen in air will be :
1. 12.4 x 10−5
2. 9.22×10−5
3. 3.54 x 10−5
4. 4.96 x 10−5
To minimise 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 |
| 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. | \(\text{Mass percentage}=\frac{\text{mass of the component in the solution}}{\text{Total mass of the solution}}\times100 \) |
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