Q. If 1 mole of a non-electrolyte solute is dissolved in 1 kg of water, what is the expected change in freezing point?
A.
0.0 °C
B.
-1.86 °C
C.
-3.72 °C
D.
-5.58 °C
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Solution
The freezing point depression for 1 mole of a non-electrolyte solute in 1 kg of water is -1.86 °C.
Correct Answer: B — -1.86 °C
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Q. If 1 mole of a non-volatile solute is dissolved in 1 kg of water, what is the expected change in boiling point? (Kb for water = 0.512 °C kg/mol)
A.
0.512 °C
B.
1.024 °C
C.
2.048 °C
D.
0.256 °C
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Solution
Boiling point elevation = i * Kb * m = 1 * 0.512 * 1 = 0.512 °C.
Correct Answer: B — 1.024 °C
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Q. If 1 mole of NaCl is dissolved in 1 kg of water, what is the expected van 't Hoff factor (i)?
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Solution
NaCl dissociates into 2 ions (Na+ and Cl-), so the van 't Hoff factor (i) is 2.
Correct Answer: B — 2
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Q. If 1 mole of solute is dissolved in 1 liter of solution, what is the concentration in terms of molarity?
A.
1 M
B.
2 M
C.
0.5 M
D.
0.25 M
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Solution
Molarity (M) = moles of solute / liters of solution = 1 mole / 1 L = 1 M.
Correct Answer: A — 1 M
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Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the mass/volume percent concentration?
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Solution
Mass/volume percent = (mass of solute / volume of solution) x 100 = (10 g / 500 mL) x 100 = 2%.
Correct Answer: B — 2%
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Q. If 10 grams of NaCl is dissolved in 500 mL of water, what is the molality of the solution? (Molar mass of NaCl = 58.5 g/mol)
A.
0.34 m
B.
0.17 m
C.
0.85 m
D.
0.50 m
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Solution
Molality (m) = moles of solute / kg of solvent. Moles of NaCl = 10 g / 58.5 g/mol = 0.171 moles. Mass of water = 0.5 kg. Molality = 0.171 moles / 0.5 kg = 0.342 m.
Correct Answer: A — 0.34 m
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Q. If 10 grams of NaCl is dissolved in enough water to make 500 mL of solution, what is the molality of the solution? (Molar mass of NaCl = 58.5 g/mol)
A.
0.34 m
B.
0.17 m
C.
0.85 m
D.
0.50 m
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Solution
Moles of NaCl = 10 g / 58.5 g/mol = 0.171 moles. Mass of solvent (water) = 0.5 kg. Molality (m) = moles of solute / kg of solvent = 0.171 moles / 0.5 kg = 0.34 m.
Correct Answer: A — 0.34 m
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Q. If 10 grams of NaOH is dissolved in 500 mL of solution, what is the molality of the solution? (Molar mass of NaOH = 40 g/mol)
A.
0.5 m
B.
1 m
C.
2 m
D.
0.25 m
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Solution
Moles of NaOH = 10 g / 40 g/mol = 0.25 moles. Mass of solvent (water) = 0.5 kg. Molality (m) = moles of solute / kg of solvent = 0.25 moles / 0.5 kg = 0.5 m.
Correct Answer: B — 1 m
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Q. If 10 grams of NaOH is dissolved in enough water to make 500 mL of solution, what is the molarity of the solution? (Molar mass of NaOH = 40 g/mol)
A.
0.5 M
B.
1 M
C.
2 M
D.
0.25 M
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Solution
Moles of NaOH = 10 g / 40 g/mol = 0.25 moles. Molarity = 0.25 moles / 0.5 L = 0.5 M.
Correct Answer: B — 1 M
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Q. If 100 g of glucose (C6H12O6) is dissolved in 1 L of solution, what is the molarity of the solution? (Molar mass of glucose = 180 g/mol)
A.
0.56 M
B.
1.0 M
C.
0.33 M
D.
0.75 M
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Solution
Moles of glucose = 100 g / 180 g/mol = 0.556 moles. Molarity = moles of solute / liters of solution = 0.556 moles / 1 L = 0.56 M.
Correct Answer: A — 0.56 M
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Q. If 15 grams of HCl is dissolved in 500 mL of solution, what is the molarity of the solution? (Molar mass of HCl = 36.5 g/mol)
A.
0.82 M
B.
1.0 M
C.
0.5 M
D.
1.5 M
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Solution
Moles of HCl = 15 g / 36.5 g/mol = 0.41096 moles. Molarity = 0.41096 moles / 0.5 L = 0.82192 M.
Correct Answer: A — 0.82 M
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Q. If 15 grams of sugar is dissolved in 250 mL of solution, what is the molarity of the solution? (Molar mass of sugar = 180 g/mol)
A.
0.33 M
B.
0.5 M
C.
0.25 M
D.
0.75 M
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Solution
Moles of sugar = 15 g / 180 g/mol = 0.0833 moles. Molarity = 0.0833 moles / 0.25 L = 0.333 M.
Correct Answer: A — 0.33 M
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Q. If 15 grams of sugar is dissolved in 250 mL of water, what is the molarity of the solution? (Molar mass of sugar = 180 g/mol)
A.
0.33 M
B.
0.5 M
C.
0.25 M
D.
0.75 M
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Solution
Moles of sugar = 15 g / 180 g/mol = 0.0833 moles. Molarity = 0.0833 moles / 0.25 L = 0.333 M.
Correct Answer: A — 0.33 M
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Q. If 2 moles of glucose are dissolved in 1 liter of water, what is the molarity of the solution?
A.
1 M
B.
2 M
C.
0.5 M
D.
3 M
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Solution
Molarity = moles of solute / liters of solution = 2 moles / 1 L = 2 M.
Correct Answer: B — 2 M
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Q. If 2 moles of KCl are dissolved in 1 liter of solution, what is the molarity of the solution?
A.
1 M
B.
2 M
C.
0.5 M
D.
3 M
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Solution
Molarity (M) = moles of solute / liters of solution = 2 moles / 1 L = 2 M.
Correct Answer: B — 2 M
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Q. If 2 moles of NaCl are dissolved in 1 kg of water, what is the van 't Hoff factor (i)?
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Solution
NaCl dissociates into 2 ions (Na⁺ and Cl⁻), so the van 't Hoff factor (i) is 2.
Correct Answer: C — 3
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Q. If 20 grams of glucose (C6H12O6) is dissolved in 200 mL of solution, what is the mass percent concentration? (Molar mass of glucose = 180 g/mol)
A.
10%
B.
5%
C.
20%
D.
15%
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Solution
Mass percent = (mass of solute / total mass of solution) x 100 = (20 g / (20 g + 200 g)) x 100 = 10%.
Correct Answer: A — 10%
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Q. If 4 moles of solute are dissolved in 2 kg of solvent, what is the molality of the solution?
A.
2 m
B.
4 m
C.
1 m
D.
0.5 m
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Solution
Molality (m) = moles of solute / kg of solvent = 4 moles / 2 kg = 2 m.
Correct Answer: A — 2 m
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Q. If 5 moles of KCl are dissolved in 1 kg of water, what is the molality of the solution?
A.
5 m
B.
2.5 m
C.
10 m
D.
1 m
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Solution
Molality (m) = moles of solute / kg of solvent = 5 moles / 1 kg = 5 m.
Correct Answer: A — 5 m
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Q. If 5 moles of KCl are dissolved in 3 kg of water, what is the molality of the solution?
A.
1.67 m
B.
2.5 m
C.
1.25 m
D.
0.5 m
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Solution
Molality (m) = moles of solute / kg of solvent = 5 moles / 3 kg = 1.67 m.
Correct Answer: A — 1.67 m
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Q. If 50 g of KCl is dissolved in 250 mL of solution, what is the molarity? (Molar mass of KCl = 74.5 g/mol)
A.
2.68 M
B.
1.34 M
C.
0.67 M
D.
0.25 M
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Solution
Moles of KCl = 50 g / 74.5 g/mol = 0.672 moles. Molarity = 0.672 moles / 0.25 L = 2.688 M.
Correct Answer: B — 1.34 M
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Q. If 50 grams of a solute is dissolved in 200 mL of solution, what is the mass/volume percent concentration?
A.
25%
B.
20%
C.
15%
D.
10%
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Solution
Mass/volume percent = (mass of solute / volume of solution) * 100 = (50 g / 200 mL) * 100 = 25%.
Correct Answer: A — 25%
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Q. If 50 grams of NaCl is dissolved in 1 liter of solution, what is the molarity? (Molar mass of NaCl = 58.5 g/mol)
A.
0.85 M
B.
1.0 M
C.
1.5 M
D.
2.0 M
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Solution
Moles of NaCl = 50 g / 58.5 g/mol = 0.854 moles. Molarity = 0.854 moles / 1 L = 0.854 M.
Correct Answer: B — 1.0 M
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Q. If 50 grams of NaOH is dissolved in 1 liter of solution, what is the molarity? (Molar mass of NaOH = 40 g/mol)
A.
1.25 M
B.
2.5 M
C.
0.5 M
D.
1 M
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Solution
Moles of NaOH = 50 g / 40 g/mol = 1.25 moles. Molarity = 1.25 moles / 1 L = 1.25 M.
Correct Answer: B — 2.5 M
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Q. If 50 mL of a 2 M HCl solution is diluted to 200 mL, what is the new molarity?
A.
0.25 M
B.
0.5 M
C.
1 M
D.
2 M
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Solution
Using the dilution formula M1V1 = M2V2, (2 M)(50 mL) = M2(200 mL) => M2 = 0.5 M.
Correct Answer: B — 0.5 M
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Q. If 7x - 3 = 4x + 6, what is the value of x?
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Solution
Subtracting 4x from both sides gives 3x - 3 = 6, then adding 3 gives 3x = 9, leading to x = 3.
Correct Answer: B — 2
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Q. If 7x = 21, what is the value of x?
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Solution
Dividing both sides by 7 gives x = 3.
Correct Answer: C — 3
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Q. If a solution has a vapor pressure of 80 mmHg and the pure solvent has a vapor pressure of 100 mmHg, what is the mole fraction of the solvent?
A.
0.8
B.
0.75
C.
0.6
D.
0.5
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Solution
Using Raoult's Law, the mole fraction of the solvent can be calculated as 80 mmHg / 100 mmHg = 0.8, which corresponds to a mole fraction of 0.75 for the solvent.
Correct Answer: B — 0.75
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Q. If the equation x^2 - 5x + k = 0 has equal roots, what is the value of k?
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Solution
For equal roots, the discriminant must be zero. Thus, (-5)^2 - 4*1*k = 0 => 25 - 4k = 0 => k = 25/4 = 6.25.
Correct Answer: A — 5
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Q. If the mole fraction of a solute in a solution is 0.2, what is the mole fraction of the solvent?
A.
0.8
B.
0.2
C.
0.5
D.
0.6
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Solution
Mole fraction of solvent = 1 - mole fraction of solute = 1 - 0.2 = 0.8.
Correct Answer: A — 0.8
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