SOLID STATE PRESS
← Back to catalog
Brønsted-Lowry Acids and Bases cover
Coming soon
Coming soon to Amazon
This title is in our publishing queue.
Browse available titles
Chemistry

Brønsted-Lowry Acids and Bases

A High School & College Chemistry Primer on Proton Transfer, Conjugate Pairs, and pH

Acids and bases show up on nearly every chemistry exam — and for most students, the confusion starts the moment a teacher mentions proton donors, conjugate pairs, or Ka without slowing down to explain what any of it actually means.

This TLDR guide cuts straight to what you need. In about 15 focused pages, it walks you through the Brønsted-Lowry definition of acids and bases, explains how conjugate acid-base pairs work, and builds up Ka, Kb, and pKa from scratch. You'll see exactly how to use ICE tables and the small-x approximation to calculate pH for strong and weak acids and bases — the calculations that appear most often on AP Chemistry exams and college general chemistry tests. The final section connects everything to buffers and blood pH, so you're ready for what comes next in the course.

This guide is written for high school students in AP or honors chemistry and college freshmen in general chemistry who need a clear, efficient reference — not a 900-page textbook. It's also useful for parents and tutors who want to get up to speed fast before a study session.

If you need a high school chemistry acid base primer that respects your time and actually explains the math, this is it.

Pick it up, read it once before your next exam, and walk in knowing exactly what you're doing.

What you'll learn
  • Define Brønsted-Lowry acids and bases as proton donors and acceptors, and contrast with the older Arrhenius definition
  • Identify conjugate acid-base pairs in any proton-transfer reaction
  • Relate acid strength to Ka, base strength to Kb, and use pKa to predict reaction direction
  • Recognize amphoteric species and the special role of water in autoionization
  • Calculate pH and pOH for strong and weak acid/base solutions using Ka, Kb, and Kw
What's inside
  1. 1. From Arrhenius to Brønsted-Lowry: What Counts as an Acid
    Introduces the Brønsted-Lowry definition as proton donor/acceptor and shows why it is broader and more useful than the Arrhenius definition.
  2. 2. Conjugate Acid-Base Pairs
    Shows how every Brønsted-Lowry reaction produces a conjugate acid and conjugate base, with rules for identifying pairs.
  3. 3. Acid and Base Strength: Ka, Kb, and pKa
    Covers strong vs. weak acids and bases, the equilibrium constants Ka and Kb, and the inverse relationship between an acid's strength and its conjugate base's strength.
  4. 4. Water, Kw, and the pH Scale
    Introduces autoionization of water, the ion-product Kw, and how pH and pOH connect to hydronium concentration.
  5. 5. Calculating pH for Strong and Weak Acids and Bases
    Walks through pH calculations for strong acids, strong bases, and weak acids/bases using ICE tables and the small-x approximation.
  6. 6. Why It Matters: Buffers, Biology, and What Comes Next
    Briefly connects Brønsted-Lowry chemistry to buffers, blood pH, and the upcoming topics of titrations and Lewis acids.
Published by Solid State Press
Brønsted-Lowry Acids and Bases cover
TLDR STUDY GUIDES

Brønsted-Lowry Acids and Bases

A High School & College Chemistry Primer on Proton Transfer, Conjugate Pairs, and pH
Solid State Press

Brønsted-Lowry Acids and Bases

A High School & College Chemistry Primer on Proton Transfer, Conjugate Pairs, and pH

Copyright © 2026 Solid State Press.

Published by Solid State Press.

All rights reserved. No part of this book may be reproduced or transmitted in any form without prior written permission, except for brief quotations in critical reviews and educational use.

Part of the TLDR Study Guides series.

Who This Book Is For

If you're sitting in AP Chemistry and acids and bases feel like a blur of formulas and definitions, or you're a college freshman hitting your first general chemistry unit on proton transfer reactions, this book was written for you. It also works for high school students who want a focused acid-base primer before a unit test or midterm.

This Brønsted-Lowry acids and bases study guide covers everything that actually shows up on exams: how conjugate acid-base pairs work — explained simply and with real examples — plus Ka, Kb, and pKa explained for beginners, the pH scale, and exactly how to calculate pH for a weak acid using an ICE table. About 15 pages, zero filler.

Read it straight through once — the sections build on each other. Work every example as you go, pausing to do the arithmetic yourself. Then hit the problem set at the end. That cycle is the fastest path from confused to confident, whether you need a quick AP Chemistry acids-and-bases review or a short chemistry guide for your first college course.

Contents

  1. 1 From Arrhenius to Brønsted-Lowry: What Counts as an Acid
  2. 2 Conjugate Acid-Base Pairs
  3. 3 Acid and Base Strength: Ka, Kb, and pKa
  4. 4 Water, Kw, and the pH Scale
  5. 5 Calculating pH for Strong and Weak Acids and Bases
  6. 6 Why It Matters: Buffers, Biology, and What Comes Next
Chapter 1

From Arrhenius to Brønsted-Lowry: What Counts as an Acid

Chemistry gives you several ways to define an acid, and which definition you use determines how many substances qualify. The oldest useful framework is the Arrhenius definition, proposed by Svante Arrhenius in the 1880s. An Arrhenius acid is any substance that releases hydrogen ions ($\text{H}^+$) when dissolved in water. An Arrhenius base is any substance that releases hydroxide ions ($\text{OH}^-$) in water. Hydrochloric acid ($\text{HCl}$) dissolves to give $\text{H}^+$ and $\text{Cl}^-$, so it is an Arrhenius acid. Sodium hydroxide ($\text{NaOH}$) dissolves to give $\text{Na}^+$ and $\text{OH}^-$, so it is an Arrhenius base. Clean, simple, and useful — as far as it goes.

The problem is the phrase "in water." The Arrhenius definition only works in aqueous solution. Worse, it can't handle bases that contain no $\text{OH}^-$ at all. Ammonia ($\text{NH}_3$) makes a perfectly good base — it neutralizes acids, turns litmus blue, and has a bitter taste — yet it has no hydroxide ion to release. Arrhenius can't explain why. A better framework was needed.

The Brønsted-Lowry upgrade

In 1923, Johannes Brønsted and Thomas Lowry independently proposed a definition centered on a single particle: the proton. A bare hydrogen ion ($\text{H}^+$) is just a proton — one positively charged particle with no electrons. The Brønsted-Lowry definition says: an acid is any species that donates a proton, and a base is any species that accepts a proton. The reaction between them is a proton transfer.

That shift — from "releases $\text{OH}^-$" to "accepts $\text{H}^+$" — is what rescues ammonia. When $\text{NH}_3$ reacts with water, it grabs a proton from $\text{H}_2\text{O}$:

$\text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons \text{NH}_4^+ + \text{OH}^-$

Keep reading

You've read the first half of Chapter 1. The complete book covers 6 chapters in roughly fifteen pages — readable in one sitting.

Coming soon to Amazon