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Understanding Acids, Bases, and the Ionization of Water: A Comprehensive Guide

This guide explores the concepts of acids, bases, and the ionization of water, emphasizing the relationship between hydronium ions (H3O+), hydroxide ions (OH-), and pH. It explains the ionization constant (Kw) of water, the definitions of acidic and basic solutions, and provides example calculations for various scenarios. Learn how to determine the acidity or basicity of solutions, calculate pH and pOH, and understand the implications of concentration on these properties. This resource is essential for anyone studying chemistry and seeking to master the foundational aspects of acid-base chemistry.

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Understanding Acids, Bases, and the Ionization of Water: A Comprehensive Guide

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  1. Acids & Bases pH

  2. H2O + H2O H3O+ + OH- Ionization of Water Kw = [H3O+][OH-] = 1.0  10-14 Kw=ionization constant for H2O

  3. Acidic or Basic [H3O+][OH-] = 1.0  10 -14 • ACIDIC • [H+] is greater than [OH-] • [H+] is greater than 1.0  10 -7 • BASIC • [OH-] is greater than [H+] • [H+] is less than 1.0  10 -7

  4. Ionization of Water • Find the hydroxide ion concentration of 3.0  10-2 M HCl. [H3O+][OH-] = 1.0  10-14 [3.0  10-2][OH-] = 1.0  10-14 [OH-] = 3.3  10-13 M Acidic or basic? Acidic ([H+] > 1 EE -7)

  5. Problem • Colas are slightly acidic. If the [H+] in a solution is 1.0 x 10 -5 M, is the solution acidic basic or neutral? What is the [OH-] of this solution? Answer 1: Because 1.0 x 10-5 M is greater than 1.0 x 10-7 M, the solution is acidic Known: [H+] = 1.0 x 10-5 M Kw = [H+] x [OH-] = 1 x 10-14 Answer 2: [OH-] = 1 x 10 -14 1.0 x 10 -5 = 1.0 x 10 -9 M

  6. pH Scale 14 0 7 INCREASING BASICITY INCREASING ACIDITY NEUTRAL pH = -log [H+]

  7. pH Scale pH of Common Substances

  8. pH Scale pH = -log [H+] pOH = -log [OH-] pH + pOH = 14 [ ] = concentration

  9. pH Scale • What is the pH of 0.050 M HNO3? pH = -log[H+] pH = -log[0.050] pH = 1.3 Acidic or basic? Acidic

  10. pH Scale • What is the molarity (conc) of HBr in a solution that has a pOH of 9.6? pH = -log[H+] 4.4 = -log[H+] - 4.4 = log[H+] - 4.4 (10x key)= [H+] [H+] = 4.0  10-5 M HBr pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 Acidic

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