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Acid / Base Equilibria

Acid / Base Equilibria. A Practical Application of the Principles of Equilibrium. Water is always in equilibrium with its ions:. 2H 2 O(l)   H 3 O + ( aq ) + OH - ( aq ) K W = [ H 3 O + ] [ OH - ] = 1.0 x 10 -14 (numeric value applies at 25 o C )

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Acid / Base Equilibria

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  1. Acid / BaseEquilibria A Practical Application of the Principles of Equilibrium

  2. Water is always in equilibrium with its ions: • 2H2O(l)   H3O+(aq) + OH-(aq) • KW = [H3O+] [OH-] = 1.0 x 10-14 (numeric value applies at 25 oC) • What are the ion concentrations in pure water at equilibrium at 25 oC?

  3. Solving the Equilibrium Equation for Water

  4. The Concept of pH and pOH • pH = - log [H3O+] • pOH = - log [OH-] • In pure water at 25 oC, we have the following: • pH = - log (1.0 x 10-7) = 7.00 • pOH = - log (1.0 x 10-7) = 7.00 • Pure water is neutral in an acid / base sense, because the concentrations of H3O+ and OH- are equal. • At 25 oC, a value of 7.00 is neutral on both the pH and pOH scales.

  5. The Conditions in Acidic, Basic, and Neutral Solutions • Acidic: [H3O+] > [OH-] • Basic: [OH-] > [H3O+] • Neutral: [H3O+] = [OH-] • ANY aqueous solution will contain BOTH H3O+ ions and OH- ions. Whether the solution is acidic, basic, or neutral depends on which ion (if either) predominates.

  6. Reaction of a Strong Acid with Water

  7. Dissolving a Water-soluble Hydroxide Compound in Water

  8. Reaction of a Weak Acid with Water

  9. Reaction of a Weak Base with Water

  10. The Hydrolysis of an Acidic Salt

  11. Finding the Missing Ka Value

  12. The Hydrolysis of a Basic Salt

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