'Strong base titration' diaporamas de présentation

Chapter 17 Additional Aspects of Aqueous Equilibria

Chapter 17 Additional Aspects of Aqueous Equilibria . The Common Ion Effect. The common ion effect is an event that occurs when an ionic equilibrium shifts due to the addition of a solute that contains an ion that is the same as an existing ion in the equilibrium. .

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Applications of Aqueous Equilibria

Applications of Aqueous Equilibria. Buffers, Acid-Base Titrations and Precipitation Reactions. Buffers. Buffers are solutions of a weak acid and its conjugate base.

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Ch 17: Additional Aspects of Aqueous Equilibria

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Applications of Aqueous Equilibria

Applications of Aqueous Equilibria. Buffers, Acid-Base Titrations and Precipitation Reactions. Buffers. Buffers are solutions of a weak acid and its conjugate base.

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Applications of Aqueous Equilibria

Applications of Aqueous Equilibria. Acid-Base Equilibria More Acid-Base Equilibria Solubility of Salts Formation of Complex Ions. Applications of Aqueous Equilibria. Natural processes that involve these equilibria weathering of minerals uptake of nutrients by plants tooth decay

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Aqueous Ionic Solutions and Equilibrium

Aqueous Ionic Solutions and Equilibrium. Chapter 19. Common Ion Effect. Shift in equilibrium that occurs because of the addition of an ion already involved in the equilibrium reaction. What happens to the equilibrium if 0.10 M NaF is added?.

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The solubility of a partially soluble salt is decreased when a common ion is added.

The Common Ion Effect. The solubility of a partially soluble salt is decreased when a common ion is added. Consider the equilibrium established when acetic acid, HC 2 H 3 O 2 , is added to water.

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Chapter 15 Application of Aqueous Equilibria

Chapter 15 Application of Aqueous Equilibria. Common Ion Effect The shift in equilibrium that occurs because of the addition of an ion already involved in the equilibrium reaction. This effect makes a solution of NaF and HF less acidic than a solution of HF alone.

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Aqueous Equilibria

Aqueous Equilibria. Solubility Equilibrium. For substances that are not appreciably soluble, we use the solubility product, K sp , as the equilibrium expression for that process. HgCl 2(s) ? Hg 2+ ( aq ) + 2 Cl - ( aq ) K sp = [Hg 2+ ][Cl - ] 2

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Chapter 16

Chapter 16. Acids- Base Titration and pH. Section 16.1. Aqueous Solutions and the Concept of pH. Self Ionization of Water. When two molecules of water produce a hydronium and hydroxide ion by the transfer of a proton. H 2 O + H 2 O ? ? H 3 O + + OH -.

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Catalyst

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Chapter 16 Lecture 2 Titrations

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Ionic products of water

Ionic products of water . Water molecules can function as both acids and bases. One water molecule (acting as a base) can accept a hydrogen ion from a second one (acting as an acid). This will be happening anywhere there is even a trace of water. A hydroxonium ion and a hydroxide ion are formed.

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Acid-Base Titrations

Acid-Base Titrations. Acid-Base Titrations. Add solution (either the acid or the base) from buret to solution in flask The concentration of one solution is known. One concentration is unknown.

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Weak Acid + Strong Base Titration

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