Acids and Bases
Acid–base reasoning begins with proton transfer and conserved charge, then separates strong-species stoichiometry from weak-equilibrium calculations.
- Exam weight
- 11–15%
- Topics
- 11
Introduction
Acid–base reasoning begins with proton transfer and conserved charge, then separates strong-species stoichiometry from weak-equilibrium calculations.
pH is logarithmic and temperature-dependent through water autoionization. Weak systems require composition, equilibrium constants, and physical-root checks.
Buffers and titrations are inventory problems first. Identify the major species after stoichiometry, then choose the equilibrium model for that region.
Introduction to Acids and Bases
How does proton transfer identify an acid, a base, and their conjugates?
A Brønsted–Lowry acid donates a proton and a base accepts one; each conjugate pair differs by exactly one hydrogen and one positive charge.
Acid–base models track electron pairs or protons
Compare Brønsted proton transfer with Lewis electron-pair donation and identify conjugates.
H₂O donates H⁺; NH₃ accepts H⁺. The products are their conjugates.
NH₃ donates an electron pair into the empty orbital on electron-deficient boron.
Read this figure without the graphic
Acid–base models track electron pairs or protons. The figure connects proton transfer, electron-pair donation, conjugate pair so the relationship can be read without relying on color alone.
| Representation | What to read |
|---|---|
| proton transfer | starting evidence or quantity |
| electron-pair donation | intermediate relationship |
| conjugate pair | result or conclusion |