🔬 Acids and Bases — Definitions, Strength, and pH Strategy

Acids and bases appear throughout the DAT in general chemistry, biochemistry, and biology. Expect questions on pH calculations, conjugate pairs, strength, and molecular identification. This blog breaks it all down with rules, visuals, and DAT-focused strategies.

🔬 Acids and Bases — Definitions, Strength, and pH Strategy

🧪 Acid-Base Definitions

Definition Acid Base
Arrhenius Produces H⁺ in solution Produces OH⁻ in solution
Brønsted-Lowry Donates H⁺ Accepts H⁺
Lewis Electron pair acceptor Electron pair donor

📌 DAT Tip: Brønsted-Lowry is the most commonly tested on the exam.

💪 Strong vs. Weak Acids/Bases

Strong Acids (completely dissociate):

  • HCl, HBr, HI

  • HNO₃, HClO₄, H₂SO₄

Weak Acids (partial dissociation):

  • HF, CH₃COOH, HCN

Strong Bases:

  • Group 1 & 2 hydroxides (e.g., NaOH, Ca(OH)₂)

🧠 Conjugate Acid-Base Pairs

  • When an acid donates a proton → forms its conjugate base

  • When a base accepts a proton → forms its conjugate acid

Example:

NH₃ (base) + H⁺ → NH₄⁺ (conjugate acid)

📌 The stronger the acid, the weaker its conjugate base.

📊 pH, pOH, and [H⁺]/[OH⁻] Relationships

Quantity Formula
pH –log[H⁺]
pOH –log[OH⁻]
pH + pOH = 14 (at 25°C)
[H⁺] 10–pH
[OH⁻] 10–pOH

🧪 Ka and Kb (Acid/Base Strength Constants)

  • Ka: Measures acid strength

  • Kb: Measures base strength

  • pKa + pKb = 14

  • The larger the Ka/Kb → the stronger the acid/base

🧠 DAT Question Styles

  • “Which is the conjugate base of HF?”

  • “Which of the following is a Lewis base?”

  • “Calculate the pH of a 0.01 M HCl solution.”

  • “Rank acids from strongest to weakest.”

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