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Introduction to Acids and Bases

Emily Wilson

Emily Wilson

6 min read

Next Topic - pH and pOH of Strong Acids and Bases

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Study Guide Overview

This study guide covers acid-base chemistry, focusing on Arrhenius and Brønsted-Lowry definitions, pH and pOH calculations, conjugate acid-base pairs, and the relationship between acid/base strength and conjugate strength. It also includes practice questions covering titration, net ionic equations, and indicator selection.

#Acids and Bases: Your Ultimate AP Chem Review 🧪

Hey, future AP Chem superstar! Let's break down acids and bases, making sure you're totally prepped for anything the exam throws your way. We'll go from the basics to the trickiest parts, and I'll throw in some memory aids and exam tips to make sure you're feeling confident.

#Acid-Base Definitions: Arrhenius vs. Brønsted-Lowry

#Arrhenius Definition

  • Arrhenius Acid: Increases the concentration of H+ ions in solution. Think of it as anything that spits out H+ in water.

  • Arrhenius Base: Increases the concentration of OH- ions in solution. It's all about releasing OH- into the water.

    Example: HCl (hydrochloric acid) in water:

    HCl→H++Cl−HCl \rightarrow H^+ + Cl^-HCl→H++Cl−

    • HCl is an Arrhenius acid because it releases H+ ions.
Key Concept

Remember: Arrhenius is all about what happens in water – H+ or OH- release.

#pH and pOH

  • pH = −log[H3O+]

  • pOH = −log[OH−]

    • These equations help us quantify the acidity or basicity of a solution.

#pH of Water

  • Water autoionizes:

    2H2O⇌H3O++OH−2H_2O \rightleftharpoons H_3O^+ + OH^-2H2​O⇌H3​O++OH−

    • Kw = [H3O+][OH−] = 1.0 × 10−14 at 25°C
    • In pure water at 25°C, pH = pOH = 7.0 (neutral).
    • 💡 Important: Kw is temperature-dependent, so neutral pH isn't always 7.0!

#Brønsted-Lowry Definition

  • Brønsted-Lowry Acid: A proton...
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Previous Topic - Acids and BasesNext Topic - pH and pOH of Strong Acids and Bases

Question 1 of 10

Ready to dive in? 🤿 Which of these compounds is an Arrhenius acid?

NaCl

KOH

HCl

H2O