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Q. No.A sodium chloride (NaCl) solution has a molarity of 3 M. Given that the density of the solution is 1.25 g/mL, its molality will be:
1.
2.90
2.
2.79
3.
1.85
4.
3.85
Subtopic: Concentration Terms & Henry's Law |
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If the density of an x M solution of NaOH is 1.12 g/mL and its molality is 3 m, determine the value of x.
1. 3.0
2. 2.3
3. 4.0
4. 5.2
1. 3.0
2. 2.3
3. 4.0
4. 5.2
Subtopic: Concentration Terms & Henry's Law |
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Consider the given dissociation reaction
\(\mathrm{HX}_{(\mathrm{aq})} \rightleftharpoons \mathrm{H}_{(\mathrm{aq})}^{+}+\mathrm{X}_{(\mathrm{aq})}^{-} \)
with an acid dissociation constant (\(K_a\)) of \(1.2 \times 10^{-5}\). What is the osmotic pressure (in atm) of a 0.03 M HX solution at 300 K?
\(\mathrm{HX}_{(\mathrm{aq})} \rightleftharpoons \mathrm{H}_{(\mathrm{aq})}^{+}+\mathrm{X}_{(\mathrm{aq})}^{-} \)
with an acid dissociation constant (\(K_a\)) of \(1.2 \times 10^{-5}\). What is the osmotic pressure (in atm) of a 0.03 M HX solution at 300 K?
| 1. | 4 atm | 2. | 2 atm |
| 3. | 1 atm | 4. | 6 atm |
Subtopic: Osmosis & Osmotic Pressure | Van’t Hoff Factor |
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3 g of acetic acid is dissolved in 500 g of water. The depression in the freezing point of the solution is given as \(\mathrm{x} \times 10^{-1} \mathrm{~K}.\) Calculate the value of x to the nearest integer.
[ Given : \(\mathrm{K}_{\mathrm{a}} \text { of } \mathrm{CH}_3 \mathrm{COOH}=1.8 \times 10^{-5}\) and \(K_f\) of water \(=1.86 \mathrm{~K} / \mathrm{molal}\)
Density of water \(=1 \mathrm{~g} / \mathrm{mL}\) ]
1. 4
2. 6
3. 2
4. 1
[ Given : \(\mathrm{K}_{\mathrm{a}} \text { of } \mathrm{CH}_3 \mathrm{COOH}=1.8 \times 10^{-5}\) and \(K_f\) of water \(=1.86 \mathrm{~K} / \mathrm{molal}\)
Density of water \(=1 \mathrm{~g} / \mathrm{mL}\) ]
1. 4
2. 6
3. 2
4. 1
Subtopic: Depression of Freezing Point |
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The boiling point of a \(\text { 2% }\)aqueous solution of a non-volatile solute A is equal to the boiling point of \(\text { 8% }\)aqueous solution of a non-volatile solute B. What is the correlation between the molecular weights of A and B?
| 1. | MA = 4MB | 2. | MB = 4MA |
| 3. | MA = 8MB | 4. | MB = 8MA |
Subtopic: Elevation of Boiling Point |
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The elevation in boiling point for 1 molal solution of a non-volatile solute A is 3 K. The depression in the freezing point for 2 molal solutions of A in the same solvent is 6 K. The ratio of \(K_b \text { and } K_f \text { i.e., } K_b / K_f~\text{is}~1:X.\)
The value of \(X\) is:
The value of \(X\) is:
| 1. | 7 | 2. | 3 |
| 3. | 1 | 4. | 2 |
Subtopic: Elevation of Boiling Point | Depression of Freezing Point |
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Which of the following has more relative lowering in vapour pressure at the same temperature
1. 0.1 M urea
2. 0.1 M NaCl
3. 0.1 M sucrose
4. 0.1 M CaCl2
1. 0.1 M urea
2. 0.1 M NaCl
3. 0.1 M sucrose
4. 0.1 M CaCl2
Subtopic: Relative Lowering of Vapour Pressure | Van’t Hoff Factor |
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A solution containing 2 g of a non-electrolyte solute dissolved in 20 g of water has a boiling point of 373.52 K. Calculate the molecular mass of the solute.
(Given that the ebullioscopic constant (Kb) is 0.52 K·kg/mol)
1. 140 g/mol
2. 80 g/mol
3. 120 g/mol
4. 100 g/mol
(Given that the ebullioscopic constant (Kb) is 0.52 K·kg/mol)
1. 140 g/mol
2. 80 g/mol
3. 120 g/mol
4. 100 g/mol
Subtopic: Depression of Freezing Point |
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The density of a 3 M NaCl solution is 1 g/mL. The molality of the solution is ‘x’. The value of 2x is:
(Round off to nearest integer)
1. 7
2. 10
3. 13
4. 5
(Round off to nearest integer)
1. 7
2. 10
3. 13
4. 5
Subtopic: Concentration Terms & Henry's Law |
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The molarity of CO2 in a soft drink is 0.01 M. The volume of soft drink is 300 mL. The mass of CO2 in soft drink is:
1. 0.132 g
2. 0.481 g
3. 0.312 g
4. 0.190 g
1. 0.132 g
2. 0.481 g
3. 0.312 g
4. 0.190 g
Subtopic: Concentration Terms & Henry's Law |
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