'Molar solubility' diaporamas de présentation

Solubility Product K sp and Solubility Predicting Precipitation Common Ion Effect

Solubility Product K sp and Solubility Predicting Precipitation Common Ion Effect. Chapter 11. The relationship between solubility and temperature can be represented by a solubility curve. Each point in the solubility curve represents a saturated solution.

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More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions

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More Equilibria in Aqueous Solutions: Slightly Soluble Salts and Complex Ions

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Solutions and Equilibrium

Solutions and Equilibrium. Solutions (homogeneous mixtures) are a part of our everyday life. Do you use mouthwash, toothpaste, cough syrup?

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Chapter 18

Chapter 18. The Solubility Product Constant. Write the net ionic equation. Solutions of sodium chromate and barium chloride are mixed. Ba 2+ + CrO 4 2- ? BaCrO 4. Ba 2+ + CrO 4 2- ? BaCrO 4. BaCrO 4 ? Ba 2+ + CrO 4 2-. Since the reaction is reversible when can flip it.

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Chapter 16

Chapter 16. Precipitation Equilibrium Solubility Product Principle. Solubility Product Constants. Silver chloride, AgCl,is rather insoluble in water. Careful experiments show that if solid AgCl is placed in pure water and vigorously stirred, a small amount of the AgCl dissolves in the water.

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Salts and Solubility

Salts and Solubility. Clicker questions for 5 actvitites Each set of clicker questions and the activity can be downloaded from the Teaching Ideas database at PhET. by Trish Loeblein updated July 2008. Salts and Solubility Activity1. Learning Goals Students will be able to:

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Solubility Lesson 7 Changing solubility

Solubility Lesson 7 Changing solubility. When to and When not to Multiply the Molarity 1. The molar solubility of Ba(OH) 2 is 2. Equal volumes of 0.0010 M Ba(NO 3 ) 2 and 0.0010 M . Ksp = ? 0.0010 M NaOH are mixed . Will a precipitate occur?

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The Solubility Product Constant, K sp

The Solubility Product Constant, K sp. Many ionic compounds are only slightly soluble in water and equations are written to represent the equilibrium between the compound and the ions present in a saturated aqueous solution. The equilibrium system is a heterogeneous system.

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Chapter 15

Chapter 15. Solubility Equilibria AP Chemistry. The Solubility Product Constant, K sp. Many important ionic compounds are only slightly soluble in water and equations are written to represent the equilibrium between the compound and the ions present in a saturated aqueous solution.

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Chapter 17 Solubility Equilibria

Chapter 17 Solubility Equilibria. Dr. Peter Warburton peterw@mun.ca http://www.chem.mun.ca/zcourses/1011.php. Solubility Equilibria. Dissolution M m X x (s) ? m M n+ (aq) + x X y- (aq) Precipitation m M n+ (aq) + x X y- (aq) ? M m X x (s)

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Review of Solubility and Precipitation Reactions

Review of Solubility and Precipitation Reactions. Aqueous Solutions. Compounds dissolved into water. Can contain molecules or ions in a solution. How do you distinguish between ion or molecule?. DISSOCIATION !!. The ability of a compound to breakdown in a solution into individual ions

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Ksp : The Solubility Product Constant

Ksp : The Solubility Product Constant. Learning Goals: I will understand the solubility product constant, Ksp , and use it to compare to Q, the trial ion product, to determine if a precipitate will form I will understand how the common ion effect affects solubility.

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(7.6)

(7.6). Solubility Product Constant (K sp ). The Terms. Solubility : - a measure of the ability of a substance to dissolve Saturated Solution : - has the maximum amount of solute dissolved in a given volume of solvent at a given temperature Unsaturated :

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Chapter 18: Solubility and Complex-Ion Equilibria

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I f you add additional solid calcium sulfate to the saturated solution, what will happen?

Assume you have a saturated solution of calcium sulfate at a temperature of 25 ? C represented by the following equation: CaSO 4 ( s ) ? Ca 2+ ( aq ) + SO 4 2- ( aq ). I f you add additional solid calcium sulfate to the saturated solution, what will happen?.

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Chapter 18 Part 2 Solubility and Complexation Equilibria

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Chapter 18: Solubility and Complex-Ion Equilibria

Chapter 18: Solubility and Complex-Ion Equilibria. Chemistry 1062: Principles of Chemistry II Andy Aspaas, Instructor. Solubility product constant. Excess of a slightly-soluble ionic compound is mixed with water An equilibrium occurs between the solid ionic compound and the dissociated ions

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Solubility

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Solubility Lesson 7 Changing solubility

Solubility Lesson 7 Changing solubility. When to and When not to Multiply the Molarity 1. The molar solubility of Ba(OH) 2 is 2. Equal volumes of 0.0010 M Ba(NO 3 ) 2 and 0.0010 M . Ksp = ? 0.0010 M NaOH are mixed . Will a precipitate occur?. Multiply by 2 because of Ba(OH) 2(s).

287 views • 8 slides