Physical Chemistry Study Resources for Competitive Exams

Physical Chemistry

Atomic Structure Basic Concepts of Chemistry Chemical Bonding Chemical Kinetics Electrochemistry Equilibrium Redox Reactions Solutions States of Matter Surface Chemistry Thermodynamics

Q. What is the osmotic pressure of a solution containing 0.5 moles of glucose in 2 liters of solution? (R = 0.0821 L·atm/(K·mol), T = 298 K)

A. 6.14 atm
B. 12.28 atm
C. 3.07 atm
D. 1.54 atm

Solution

Osmotic pressure (π) = (n/V)RT = (0.5/2) * 0.0821 * 298 = 6.14 atm.

Correct Answer: A — 6.14 atm

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Q. What is the osmotic pressure of a solution containing 0.5 moles of solute in 2 liters of solution at 25 °C? (R = 0.0821 L·atm/(K·mol))

A. 10.25 atm
B. 5.12 atm
C. 2.03 atm
D. 1.23 atm

Solution

Osmotic pressure (π) = nRT/V = (0.5 moles * 0.0821 * 298) / 2 = 12.21 atm.

Correct Answer: B — 5.12 atm

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Q. What is the osmotic pressure of a solution containing 1 mole of glucose in 2 liters of solution at 25 °C? (R = 0.0821 L·atm/(K·mol))

A. 0.41 atm
B. 0.82 atm
C. 1.23 atm
D. 1.64 atm

Solution

Osmotic pressure (π) = nRT/V = (1 mol)(0.0821 L·atm/(K·mol))(298 K) / 2 L = 0.82 atm.

Correct Answer: B — 0.82 atm

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Q. What is the osmotic pressure of a solution directly proportional to?

A. Temperature
B. Concentration of solute
C. Volume of solvent
D. Both A and B

Solution

Osmotic pressure is directly proportional to both the temperature and the concentration of solute.

Correct Answer: D — Both A and B

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Q. What is the oxidation state of chlorine in NaClO3?

A. +1
B. +3
C. +5
D. +7

Solution

In NaClO3, chlorine has an oxidation state of +5.

Correct Answer: C — +5

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Q. What is the oxidation state of nitrogen in NH4+?

A. -3
B. +1
C. +3
D. +5

Solution

In NH4+, nitrogen has an oxidation state of -3.

Correct Answer: A — -3

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Q. What is the oxidation state of nitrogen in NO3^-?

A. +3
B. +5
C. 0
D. -1

Solution

In NO3^-, nitrogen has an oxidation state of +5.

Correct Answer: B — +5

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Q. What is the oxidation state of sulfur in H2SO4?

A. 0
B. +4
C. +6
D. -2

Solution

In H2SO4, the oxidation state of sulfur is +6.

Correct Answer: C — +6

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Q. What is the percentage by mass of a solution containing 20 grams of solute in 180 grams of solution?

A. 10%
B. 20%
C. 15%
D. 25%

Solution

Percentage by mass = (mass of solute / mass of solution) * 100 = (20 g / (20 g + 180 g)) * 100 = 20%.

Correct Answer: B — 20%

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Q. What is the percentage by mass of a solution containing 5 g of NaCl in 95 g of water?

A. 5%
B. 10%
C. 15%
D. 20%

Solution

Percentage by mass = (mass of solute / total mass) × 100 = (5 g / (5 g + 95 g)) × 100 = 5%.

Correct Answer: A — 5%

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Q. What is the percentage composition of carbon in glucose (C6H12O6)?

A. 40%
B. 50%
C. 60%
D. 30%

Solution

Molar mass of glucose = 6(12) + 12(1) + 6(16) = 180 g. Percentage of carbon = (72/180) x 100 = 40%.

Correct Answer: A — 40%

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Q. What is the pH of a 0.01 M HCl solution?

A. 1
B. 2
C. 3
D. 4

Solution

The pH of a 0.01 M HCl solution is 2, as HCl is a strong acid and fully dissociates.

Correct Answer: B — 2

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Q. What is the pH of a 0.01 M NaOH solution?

A. 12
B. 2
C. 10
D. 1

Solution

For NaOH, which is a strong base, pOH = -log[OH-]. [OH-] = 0.01 M, so pOH = 2. Therefore, pH = 14 - pOH = 14 - 2 = 12.

Correct Answer: A — 12

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Q. What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?

A. 4.76
B. 7.00
C. 9.24
D. 10.00

Solution

Sodium acetate is a salt of a weak acid (acetic acid) and a strong base (sodium hydroxide). The pH can be calculated using the formula pH = 7 + 0.5(pKa - log[C]), where pKa of acetic acid is 4.76.

Correct Answer: C — 9.24

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Q. What is the pH of a 0.01 M solution of sodium hydroxide (NaOH)?

A. 12
B. 2
C. 10
D. 14

Solution

pH = 14 - pOH; pOH = -log[OH-] = -log(0.01) = 2; pH = 14 - 2 = 12.

Correct Answer: A — 12

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Q. What is the pH of a 0.01 M solution of sulfuric acid (H2SO4)?

A. 1
B. 2
C. 3
D. 0.5

Solution

H2SO4 is a strong acid and dissociates completely, so pH = -log(0.01) = 2.

Correct Answer: A — 1

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Q. What is the pH of a 0.05 M solution of sulfuric acid (H2SO4)?

A. 1
B. 1.3
C. 1.7
D. 2

Solution

H2SO4 is a strong acid and dissociates completely; [H+] = 0.05 M, so pH = -log(0.05) ≈ 1.3

Correct Answer: B — 1.3

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Q. What is the pH of a 0.1 M NaOH solution?

A. 10
B. 11
C. 12
D. 13

Solution

pOH = -log[OH-] = -log(0.1) = 1; pH = 14 - pOH = 14 - 1 = 13

Correct Answer: C — 12

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Q. What is the pH of a 0.1 M solution of acetic acid (CH3COOH) given its Ka is 1.8 x 10^-5?

A. 2.87
B. 4.76
C. 3.87
D. 5.00

Solution

Using the formula for weak acids, pH = 0.5(pKa - log[C]) = 0.5(4.74 - log(0.1)) = 4.76.

Correct Answer: B — 4.76

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Q. What is the pH of a 0.1 M solution of ammonium chloride (NH4Cl)?

A. 5.1
B. 5.5
C. 6.1
D. 6.5

Solution

NH4Cl is a salt of a weak base and a strong acid; it hydrolyzes to give H+, resulting in a pH < 7.

Correct Answer: C — 6.1

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Q. What is the pH of a 0.1 M solution of hydrochloric acid (HCl)?

A. 1
B. 0.1
C. 10
D. 0

Solution

The pH of a strong acid like HCl is calculated using the formula pH = -log[H+]. For 0.1 M HCl, [H+] = 0.1 M, so pH = -log(0.1) = 1.

Correct Answer: A — 1

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Q. What is the pH of a 0.1 M solution of potassium hydrogen phthalate (KHP)?

A. 4.0
B. 5.0
C. 6.0
D. 7.0

Solution

KHP is a weak acid; its pKa is approximately 5.0, so the pH of a 0.1 M solution is around 5.0.

Correct Answer: B — 5.0

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Q. What is the pH of a 0.1 M solution of sodium acetate (CH3COONa)?

A. 4.76
B. 7
C. 9.24
D. 10

Solution

pH = 7 + 0.5(pKa + log[C]) = 7 + 0.5(4.76 + log(0.1)) = 9.24

Correct Answer: C — 9.24

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Q. What is the pH of a 0.1 M solution of sodium bicarbonate (NaHCO3)?

A. 7.5
B. 8.4
C. 9.0
D. 6.0

Solution

NaHCO3 is a weak base; its pH is around 8.4.

Correct Answer: B — 8.4

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Q. What is the pH of a buffer solution containing 0.1 M acetic acid and 0.1 M sodium acetate?

A. 4.74
B. 5.74
C. 6.74
D. 7.74

Solution

Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]). Here, pKa ≈ 4.74, so pH = 4.74 + log(1) = 4.74.

Correct Answer: A — 4.74

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Q. What is the pH of a buffer solution containing 0.2 M acetic acid and 0.1 M sodium acetate?

A. 4.76
B. 5.00
C. 5.74
D. 6.00

Solution

Using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) = 4.76 + log(0.1/0.2) = 5.74

Correct Answer: C — 5.74

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Q. What is the pH of a buffer solution made from 0.2 M acetic acid and 0.2 M sodium acetate?

A. 4.76
B. 5.76
C. 6.76
D. 7.76

Solution

Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]) = 4.76.

Correct Answer: A — 4.76

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Q. What is the pH of a neutral solution at 25°C?

A. 0
B. 7
C. 14
D. 1

Solution

At 25°C, the pH of a neutral solution is 7.

Correct Answer: B — 7

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Q. What is the pH of a solution formed by mixing equal volumes of 0.1 M HCl and 0.1 M NaOH?

A. 7
B. 1
C. 0
D. 14

Solution

HCl and NaOH neutralize each other completely, resulting in a neutral solution with a pH of 7.

Correct Answer: A — 7

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Q. What is the pH of a solution that has a hydrogen ion concentration of 1 x 10^-5 M?

A. 5
B. 7
C. 9
D. 10

Solution

pH is calculated as pH = -log[H+]. For [H+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5.

Correct Answer: A — 5

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Physical Chemistry

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