Acids and Bases Test Study Guide

By: Kareem Ibrahim

Arrhenius Acid

Produces H⁺ ions in water

Arrhenius Base

Produces OH⁻ ions in water

Properties of Acids

Sour, pH<7, turn blue litmus red, react with metals, conduct electricity

Properties of Bases

Bitter, slippery, pH>7, turn red litmus blue, conduct electricity

Acid Naming

Binary: hydro + root + ic acid; Oxyacids: -ate→-ic, -ite→-ous

Base Naming

Metal + hydroxide

Strong Acids

Completely ionize in water (HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄)

Weak Acids

Partially ionize in water (HF, CH₃COOH, H₂CO₃)

Strong Bases

Completely dissociate (Group 1 OH⁻ and Ca(OH)₂, Sr(OH)₂, Ba(OH)₂)

Weak Bases

Partially dissociate (NH₃ and amines)

Brønsted-Lowry Acid

Proton (H⁺) donor

Brønsted-Lowry Base

Proton (H⁺) acceptor

Conjugate Acid

Formed when a base gains H⁺

Conjugate Base

Formed when an acid loses H⁺

Conjugate Acid-Base Pair

Two substances differing by one H⁺

Lewis Acid

Electron pair acceptor

Lewis Base

Electron pair donor

pH Scale

Measures acidity/basicity from 0-14; 7 neutral

Acidic Solution

pH<7

Neutral Solution

pH=7

Basic Solution

pH>7

H⁺ Concentration

[H⁺]=10⁻ᵖᴴ

OH⁻ Concentration

[OH⁻]=10⁻ᵖᴼᴴ

pH Formula

pH=-log[H⁺]

pOH Formula

pOH=-log[OH⁻]

pH and pOH Relationship

pH+pOH=14

Water Ion Product

Kw=[H⁺][OH⁻]=1.0×10⁻¹⁴ at 25°C

Self-Ionization of Water

2H₂O ⇌ H₃O⁺ + OH⁻

Amphoteric Substance

Can act as both an acid and a base

Water

Is amphoteric

Indicator

Changes color based on pH

Litmus

Blue→red in acid, red→blue in base

Phenolphthalein

Colorless in acid, pink in base

Bromothymol Blue

Yellow in acid, blue in base, green near neutral

Universal Indicator

Shows a range of pH colors

Neutralization Reaction

Acid + Base → Salt + Water

Net Ionic Neutralization

H⁺ + OH⁻ → H₂O

Titration

Uses a known concentration to find an unknown concentration

Titration Formula

M₁V₁=M₂V₂ (for 1:1 reactions)

Equivalence Point

Moles of acid = moles of base

Endpoint

Point where indicator changes color

Ka

Acid dissociation constant

Stronger Acid

Larger Ka and smaller pKa

Weaker Acid

Smaller Ka and larger pKa

Acidic Salt Solution

Formed from strong acid + weak base

Basic Salt Solution

Formed from weak acid + strong base

Neutral Salt Solution

Formed from strong acid + strong base

Common Strong Acids

HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄

Common Strong Bases

LiOH, NaOH, KOH, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂