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BCH 202University of IbadanOct 23, 2026

7. IONIZATION OF WATER

Structure

6 Concept Stages

Practice Exam

80+ Questions

Active Recall

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Executive Topic Summary

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High-Yield Exam Takeaways

  • Acids, Bases & Conjugate Pairs: The Proton Transfer Story
  • Water's Secret Double Life: Autoionization and the Kw Constant
  • pH, pKa, and the Henderson-Hasselbalch Equation
  • Acid Strength, Classification, and Dissociation Constants
  • The pH Scale: Measurement, Meaning, and Biological Relevance
  • Buffer Systems: Biological pH Protection

Study Tree Preview (Bite-Sized Concepts)

Previewing 3 stages

1Acids, Bases & Conjugate Pairs: The Proton Transfer Story

4 Micro-Bites
The Brønsted-Lowry Definition: It's All About Protons:Let's start with the simplest way to think about acids and bases that you'll use throughout biochemistry. Forget the old "acids taste sour" definition from grade school—here's what...
What Happens When an Acid Dissolves? Meet the Conjugate Base:When an acid drops into water, it doesn't just sit there—it ionizes. That means it splits apart, releasing its H+ and leaving behind whatever was attached to that proton. This left...

2Water's Secret Double Life: Autoionization and the Kw Constant

5 Micro-Bites
Water Ionizes Itself: The Autoionization Reaction:Even pure water isn't just sitting there—it's constantly reacting with itself. One water molecule can donate a proton to another water molecule, creating a <term def="hydronium ion...
The Equilibrium Expression and Why We Simplify:For any equilibrium, we can write an expression with products over reactants. For water autoionization, that would be: $$K_{eq} = \frac{[H_3O^+][OH^-]}{[H_2O]^2}$$ But here's the k...

3pH, pKa, and the Henderson-Hasselbalch Equation

5 Micro-Bites
Why Logarithms? Taming Enormous Concentration Ranges:Biological [H⁺] concentrations span fourteen orders of magnitude—from 1 M in strong acid to $10^{-14}$ M in strong base. Writing and comparing these tiny numbers is painful. Enter ...
Defining pH and pKa: The Same Mathematical Trick:The formal definition is clean: $$\text{pH} = -\log[H^+]$$ Similarly, we define <term def="the negative base-10 logarithm of the acid dissociation constant; pKa = -log(Ka)">pKa</te...

Sample Practice Questions (Active Recall)

Showing 3 of 80+

Q1.Which of the following best explains why buffer systems are essential for maintaining biological homeostasis?

AThey completely neutralize all added acids and bases, keeping pH at exactly 7.0
BThey shift the equilibrium of water ionization to favor complete dissociation
CThey increase the ionic strength of biological fluids to enhance enzyme activity
DThey resist drastic pH changes when small amounts of acid or base are added, protecting pH-sensitive biological reactions

Q2.The course BCH 202 focuses exclusively on inorganic acid-base chemistry without biological applications.

ATrue
BFalse

Q3.According to the Brønsted-Lowry definition presented in the lecture, which of the following best describes the relationship between an acid and its conjugate base?

AThe conjugate base is always electrically neutral regardless of the acid's charge
BThe conjugate base is formed by adding a proton to the acid
CThe conjugate base is the species formed when the acid donates a proton (H⁺)
DThe conjugate base and acid differ by two protons

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