'Common ion effect' presentation slideshows

Topic 8: Kinetics and Equilibrium

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Chapter 15

Chapter 15. Applying equilibrium. The Common Ion Effect. When the salt with the anion of a weak acid is added to that acid, Lowers the percent dissociation of the acid. Ex: NaF and HF mixed together F- is the common ion HF ? H + + F -

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Acid-Base Equilibria and Solubility Equilibria

Acid-Base Equilibria and Solubility Equilibria. Chapter 16 16.1-16.9. Acid-Base Equilibria and Solubility Equilibria. We will continue to study acid-base reactions Buffers Titrations We will also look at properties of slightly soluble compunds and their ions in solution.

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Chapter 15

Chapter 15. Applying equilibrium. The Common Ion Effect. When the salt with the anion of a weak acid is added to that acid, It reverses the dissociation of the acid. Lowers the percent dissociation of the acid. The same principle applies to salts with the cation of a weak base.

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Seminar on Physicochemical factors Under Preformulation Study

Seminar on Physicochemical factors Under Preformulation Study. 1. PREFORMULATION. What it is?

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Intro to Titrations

Intro to Titrations. Volumetric Analysis. Volumetric analysis is when the volume of a reactant required to complete a chemical reaction is measured.

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Applications of Aqueous Equilibria

Applications of Aqueous Equilibria. Strong Acid/Strong Base Titration. Endpoint is at pH 7. A solution that is 0.10 M HCl is titrated with 0.10 M NaOH. Strong Acid/Strong Base Titration. A solution that is 0.10 M NaOH is titrated with 0.10 M HCl. Endpoint is at pH 7.

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Acids and Bases-Review

Acids and Bases-Review. The properties of acids include the following: Taste sour (but don't taste them!!) Their water solutions conduct electrical current (electrolytes) They react with bases to form salts and water Turns Blue Litmus Paper to Red

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Environmental chemistry

Environmental chemistry. E 12. water and soil. Water and soil. Solve problems relating to the removal of heavy-metal ions, phosphates and nitrates from water by chemical precipitation. State what is meant by the term cation -exchange capacity (CEC) and outline its importance.

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Acid Base Hydrolysis

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Acids and Bases

Acids and Bases. Chapter 15. Overview. Acid /Base Theories Arrhenius, Bronsted-Lowry and Lewis Acid Strength pH Equilibria / Hydrolysis Common Ion effect Buffers omit carboxylic acids, sec 15.9, 15.10. Arrhenius Definitions review. Acid: H 3 0 +1 producer in water

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The Solubility Product Constant, K sp

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Equilibrium Concept Review

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Chapter 3: Nucleophilic catalysis

Chapter 3: Nucleophilic catalysis. Principle: reaction rate is enhanced by a nucleophilic compound that forms a low-energy intermediate. Of course, the nucleophile does not end up in the reaction product. Criteria for a nucleophilic catalyst:

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CHEMISTRY 59-320 ANALYTICAL CHEMISTRY Fall - 2010

CHEMISTRY 59-320 ANALYTICAL CHEMISTRY Fall - 2010. Chapter 8: Activity and the systematic treatment of equilibrium. Chemical Equilibrium Electrolyte Effects.

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Common ion lab

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ANALYTICAL CHEMISTRY CHEM201/212/213

ANALYTICAL CHEMISTRY CHEM201/212/213. ANALYTICAL CHEMISTRY (16 Lectures + 6 Tutorials).

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Chapter 17: Additional Aspects of Aqueous Equilibria

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