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Understanding the pH Scale and Self-Ionization of Water

This article explores the essential concepts of the pH scale, focusing on the self-ionization of water (H2O). At 25°C, water dissociates minimally into H3O+ and OH- ions, with concentrations of 1 x 10^-7 mol/L. The ionization constant (Kw) for pure water at this temperature is 1 x 10^-14, representing the balance between hydronium and hydroxide ions. We will also delve into how to calculate pH and pOH, their interrelation, and how to derive concentrations of ions based on the pH scale.

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Understanding the pH Scale and Self-Ionization of Water

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  1. pH Calculations Soren Sorensen

  2. pH Scale

  3. Self-Ionization of Water H2O + H2O  H3O+ + OH- Though pure water is considered a non-conductor, there is a slight, but measurable conductivity due to “self-ionization”

  4. Kw – Ionization Constant for Water In pure water at 25 C: [H3O+] = 1 x 10-7 mol/L [OH-] = 1 x 10-7 mol/L Kw is a constant at 25 C: Kw = [H3O+][OH-] Kw= (1 x 10-7)(1 x 10-7) = 1 x 10-14

  5. Calculating pH, pOH pH = -log10(H3O+) pOH = -log10(OH-) Relationship between pH and pOH pH + pOH = 14 Finding [H3O+], [OH-] from pH, pOH [H3O+] = 10-pH [OH-] = 10-pOH

  6. pH + pOH = 14

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