CHEM✦
✦
General Chemistry 210
2 MAXE
210 pH · Buffers · Intermolecular Forces · Thermodynamics
A C I D - B A S E · H Y D R O G E N B O N D I N G · W AT E R C H E M I S T R Y
SCIENCE
chem 210 exam 2
P H C A LCU L AT I O N S · A C I D - B A S E ST R E N GT H · I N T E R M O L E CU L A R F O R C E S · B U F F E R S · W AT E R
P R O P E RT I E S · T H E R M O DY N A M I CS
COURSE Chemistry 210 · General Chemistry II EXAM TYPE Unit Examination 2
ACADEMIC YEAR TOTAL QUESTIONS 25 Questions
SUBJECT AREAS pH/pOH · Ka/pKa · Buffers · IMFs · FORMAT Multiple Choice — Select the Single Best
Hydrogen Bonding · Water · ΔG/ΔH/ΔS Answer
EXAMINATION INSTRUCTIONS
▸ Select the single best answer for each question.
▸ Content covers: pH/pOH calculations, Ka/pKa relationships, acid-base strength, buffers, intermolecular forces, hydrogen
bonding, water properties, and thermodynamic concepts (ΔG, ΔH, ΔS).
▸ Each question includes the correct answer with a detailed rationale.
SECTION I — COMPREHENSIVE EXAM 2 Questions 1 – 25
1. The pH of a solution of 8.9 × 10⁻¹² M NaOH is:
A. 8.9
B. 8.9 × 10⁻¹²
C. 4.8
D. 11
E. 2.9
CORRECT ANSWER E — 2.9
RATIONALE NaOH is a STRONG base — it completely dissociates. [OH⁻] = 8.9 × 10⁻¹² M is extremely dilute — actually LESS
than the [OH⁻] from water autoionization (1.0 × 10⁻⁷ M). In such dilute solutions, the contribution from water
itself dominates. pH ≈ −log[H⁺] = 2.9 (the solution is slightly acidic due to water's autoionization dominating).
For a more concentrated strong base like 0.0010 M NaOH: [OH⁻] = 10⁻³, pOH = 3, pH = 14 − 3 = 11. The ion
product of water: Kw = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴. In equilibrium constant expressions, brackets [ ] indicate
concentration in MOLARITY.
✦
General Chemistry 210
2 MAXE
210 pH · Buffers · Intermolecular Forces · Thermodynamics
A C I D - B A S E · H Y D R O G E N B O N D I N G · W AT E R C H E M I S T R Y
SCIENCE
chem 210 exam 2
P H C A LCU L AT I O N S · A C I D - B A S E ST R E N GT H · I N T E R M O L E CU L A R F O R C E S · B U F F E R S · W AT E R
P R O P E RT I E S · T H E R M O DY N A M I CS
COURSE Chemistry 210 · General Chemistry II EXAM TYPE Unit Examination 2
ACADEMIC YEAR TOTAL QUESTIONS 25 Questions
SUBJECT AREAS pH/pOH · Ka/pKa · Buffers · IMFs · FORMAT Multiple Choice — Select the Single Best
Hydrogen Bonding · Water · ΔG/ΔH/ΔS Answer
EXAMINATION INSTRUCTIONS
▸ Select the single best answer for each question.
▸ Content covers: pH/pOH calculations, Ka/pKa relationships, acid-base strength, buffers, intermolecular forces, hydrogen
bonding, water properties, and thermodynamic concepts (ΔG, ΔH, ΔS).
▸ Each question includes the correct answer with a detailed rationale.
SECTION I — COMPREHENSIVE EXAM 2 Questions 1 – 25
1. The pH of a solution of 8.9 × 10⁻¹² M NaOH is:
A. 8.9
B. 8.9 × 10⁻¹²
C. 4.8
D. 11
E. 2.9
CORRECT ANSWER E — 2.9
RATIONALE NaOH is a STRONG base — it completely dissociates. [OH⁻] = 8.9 × 10⁻¹² M is extremely dilute — actually LESS
than the [OH⁻] from water autoionization (1.0 × 10⁻⁷ M). In such dilute solutions, the contribution from water
itself dominates. pH ≈ −log[H⁺] = 2.9 (the solution is slightly acidic due to water's autoionization dominating).
For a more concentrated strong base like 0.0010 M NaOH: [OH⁻] = 10⁻³, pOH = 3, pH = 14 − 3 = 11. The ion
product of water: Kw = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴. In equilibrium constant expressions, brackets [ ] indicate
concentration in MOLARITY.
