Cheat Sheet Flashcards
Topic
Explanation / Examples
BASIC INTRO TO ACIDS & BASES
Acids: Donate H⁺ ions (protons); Bases: Accept H⁺ or donate OH⁻ ions
CONJUGATE ACID-BASE PAIRS
Acid ⇌ H⁺ + Conjugate Base; Base + H⁺ ⇌ Conjugate Acid
Example
NH₃ (base) ⇌ NH₄⁺ (conjugate acid)
LEWIS, ARRHENIUS, BRONSTED CONCEPTS
Arrhenius: Acid → H⁺, Base → OH⁻; Bronsted: Acid = H⁺ donor, Base = H⁺ acceptor; Lewis: Acid = e⁻ pair acceptor, Base = e⁻ pair donor
STRENGTH OF ACIDS AND BASES
Strong = Complete ionization; Weak = Partial ionization; Strength ∝ Conductivity ∝ Ka/Kb
IONIZATION OF WATER / pH CALCULATION
H₂O ⇌ H⁺ + OH⁻; Kw = 1×10⁻¹⁴; pH = -log[H⁺]; pH + pOH = 14
STRONG ACIDS
HCl, HNO₃, H₂SO₄, HBr, HI, HClO₄
WEAK ACIDS
HF, CH₃COOH, H₂CO₃, HCN
STRONG BASES
NaOH, KOH, Ca(OH)₂, Ba(OH)₂
WEAK BASES
NH₃, CH₃NH₂, Pyridine
CONJUGATE ACID-BASE COMPARISON
Strong Acid → Weak Base; Strong Base → Weak Acid; Weak Acid → Stronger Conjugate Base; Weak Base → Stronger Conjugate Acid
BUFFER SOLUTIONS
Resist pH changes; Weak acid/base + salt; pH = pKa + log([Salt]/[Acid]); Applications: Blood, Pharma, Labs
SALT HYDROLYSIS
Strong Acid + Strong Base → Neutral; Strong Acid + Weak Base → Acidic; Weak Acid + Strong Base → Basic
HYDROLYSIS DEFINITION
Reaction with water to form H⁺ or OH⁻
SOLUBILITY PRODUCT (Ksp)
Ksp = [A⁺][B⁻]; Use ICE table; Precipitation when Q > Ksp
COMMON ION EFFECT
Common ion suppresses ionization; Example: CH₃COOH + NaCH₃COO → Less H⁺
Q1
What is the conjugate base of H₂CO₃? → HCO₃⁻
Q2
Which of these is a weak acid? (a) HCl (b) HNO₃ (c) HF (d) H₂SO₄ → (c) HF
Q3
Define buffer solution with example. → A solution that resists pH change; e.g., CH₃COOH + CH₃COONa
Q4
Why is NH₄Cl acidic in solution? → NH₄⁺ hydrolyzes to give H⁺ ions.
Q5
State pH formula. → pH = -log[H⁺]
Q6
Why does common ion effect reduce ionization? → Extra ions shift equilibrium left
Q7
When does precipitation occur? → When ionic product (Q) > Ksp
