Chemistry II - Exam 2 & 3 Equations/Memorization Things

general equilibrium constant expression K

K = [products]/[reactants]

hydronium ion

H₃O⁺

hydroxide ion

OH⁻

general equation for an acid-base reaction

acid + base ⇌ salt + water

general equation for an acid-base reaction with a weak acid

HA + H₂O ⇌ H₃O⁺ + A⁻ 

general equation for an acid-base reaction with a weak base

B + H₂O ⇌ BH⁺ + OH⁻ 

acid-ionization constant Kₐ equation

Kₐ = [H₃O⁺][A⁻]/[HA]

acid-ionization constant Kb equation

Kb = [BH⁺][OH⁻]/[B]

ion-product constant for water Kw

Kw = 1.0 × 10⁻¹⁴

pH equation

pH = -log[H₃O⁺]

pOH equation

pOH = -log[OH⁻]

hydronium ion concentration equation

[H₃O⁺] = 10^-pH

hydroxide ion concentration equation

[OH⁻] = 10^-pOH

ion-product constant for water Kw equation

Kw = [H₃O⁺][OH⁻]

ion-product constant for water in relation to the acid-ionization constant and base-ionization constant as an equation

Kw = Ka × Kb

pK general equation

pK = -log(K)

acid or base ionization constant expression in relation to pK

K = 10^-pK

Henderson-Hasselbalch equation

pH = pKa + log [A⁻]/[HA]

hydrochloric acid formula

HCl

hydrobromic acid formula

HBr

hydroiodic acid formula

HI

nitric acid formula

HNO₃

perchloric acid

HClO₄

sulfuric acid

H₂SO₄

lithium hydroxide formula

LiOH

sodium hydroxide formula

NaOH

potassium hydroxide formula

KOH

strontium hydroxide formula

Sr(OH)₂

calcium hydroxide formula

Ca(OH)₂

barium hydroxide formula

Ba(OH)₂