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Applications of Aqueous Equilibria

Chapter 8. Applications of Aqueous Equilibria. Chapter 8: Applications of Aqueous Equilibria. 8.1 Solutions of Acids or Bases Containing a Common Ion 8.2 Buffered Solutions 8.3 Exact Treatment of Buffered Solutions 8.4 Buffer Capacity 8.5 Titrations and pH Curves

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Chapter 15: Aqueous Equilibria

Chapter 15: Aqueous Equilibria. Renee Y. Becker Valencia Community College. Acid-Base Concepts: The Arrhenius Acid-Base Theory. Generalized Arrhenius Acid HA (aq) ? H + (aq) + A - (aq) Acids are substances that dissociate in water to produce hydrogen ions

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Hardness

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Calculating pH from K a

Calculating pH from K a. The K a for niacin (C 5 H 4 NCOOH) is 1.6 x 10 -5 . What is the pH of a 0.010 M solution of niacin?. C 5 H 4 NCOOH C 5 H 4 NCOO - ( aq ) + H + ( aq ) initial: 0.010 M 0 M 0 M change: - x M +x M +x M

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Buffers

Buffers. 4/13/2011. Definitions. Weak Acids : all proton donors that are in equilibrium Conjugate Bases : the ions that are left over after a weak acid loses it H + ions (protons) Buffer : a solution containing a mix of weak acid and the salt of its conjugate base

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Acid-Base Equilibrium

Acid-Base Equilibrium. According to Arrhenius theory , substances were acids if they contained hydrogen ion ( H + ), and bases if they contained hydroxide ion ( OH - ). However, some substances, like the base ammonia (NH 3 ), could not be classified using this definition.

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