#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:

  $$HCl \rightarrow H^+ + Cl^-$$

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

#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:

  $$2H_2O \rightleftharpoons H_3O^+ + OH^-$$

  • 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...