Lesson 6: The Solubility Product

Slides:

Advertisements

Similar presentations

Solubility Equilibria

Advertisements

Solubility Equilibria

Equilibrium 1994A Teddy Ku A MgF 2(s) Mg 2+ (aq) + 2F - (aq) In a saturated solution of MgF 2 at 18 degrees Celsius, the concentration of Mg 2+

Solubility Products Consider the equilibrium that exists in a saturated solution of BaSO 4 in water: BaSO 4 (s) Ba 2+ (aq) + SO 4 2− (aq)

1 Solubility Equilibria Solubility Product Constant K sp for saturated solutions at equilibrium.

Notes handout, equilibrium video part 2. 2 Le Chatelier’s Principle: if you disturb an equilibrium, it will shift to undo the disturbance. Remember, in.

Solubility Product Constant A special case of equilibrium involving dissolving. Solid  Positive Ion + Negative Ion Mg(NO 3 ) 2  Mg NO 3 - Keq.

Aqueous Equilibria Entry Task: Feb 28 th Thursday Question: Provide the K sp expression for calcium phosphate, K sp = 2.0 x From this expression,

Lecture 62/2/05. Solubility vs. Solubility constant (K sp ) BaSO 4 (s) ↔ Ba 2+ (aq) + SO 4 2- (aq) K sp = [Ba 2+ ][SO 4 2- ] Ba 2+ (aq) + SO 4 2- (aq)

Lecture 71/31/07. Solubility vs. Solubility constant (K sp ) What is the difference? BaSO 4 (s) ⇄ Ba 2+ (aq) + SO 4 2- (aq) Ba 2+ (aq) + SO 4 2- (aq)

Solubility Product Constant 6-5 Ksp. is a variation on the equilibrium constant for a solute-solution equilibrium. remember that the solubility equilibrium.

The Solubility Product Principle. 2 Silver chloride, AgCl,is rather insoluble in water. Careful experiments show that if solid AgCl is placed in pure.

Solubility Product Constant

Solubility Product Constant Ksp Ksp: review 1)What is the molar mass of H 2 O? 2) How many moles are in 18 g of NaCl? 3) How many g of CaCl 2 are found.

Solubility Product Constant

Solubility Equilibria. Write solubility product (K sp ) expressions from balanced chemical equations for salts with low solubility. Solve problems involving.

Section 4: Solubility Equilibrium. Objectives Explain what is meant by solubility product constants, and calculate their values. Calculate solubilities.

Solubility Product Constant Factors Affecting Solubility Selective Precipitation.

Friday, March 21 st : “A” Day Monday, March 24 th : “B” Day Agenda  Homework questions/collect  Finish section 14.2: “Systems At Equilibrium”  Homework:

Chapter 16 Lesson 1 Solubility and Complex Ion Equilibria.

Solubility of Salts & Complex Ions. Solubility of Salts Precipitation reactions occur when one of the products in a double replacement is a water-_________.

Solubility Chapter 17. No only do acids and bases dissolve in aqueous solutions but so do ionic compounds –Many ionic compounds tend to be strong electrolytes.

Terms Solute Substance that has been dissolved in a liquid Solvent the solution (liquid or gas) part of the solute concentration Dissolves the solute Solubility.

Hannah Nirav Joe ↔. Big Ideas You will be able to Understand what K sp is Find K sp from a reaction.

Unit 17. Dissolution: the process in which an ionic solid dissolves in a polar liquid. AgCl (s) ↔ Ag + (aq) + Cl - (aq) Precipitation: the process in.

Introduction and Example 1—Molar Solubility of an AB type Compound. Molar Solubility from K sp.

Le Chatelier’s Principle

Saturated solution – no more solute will dissolve solubility product constant – equilibrium constant for ionic compounds that are only slightly soluble.

Drill: Determine the KQ/HQ ratio to make a buffer solution with a pH of 4.70 K a for HQ = 3.0 x

Unit 10 Test Review. 1. Dinitrogen trioxide gas decomposes to nitrogen monoxide gas and nitrogen dioxide gas in an endothermic process. Predict the effect.

Solubility Equilibrium Solubility Product Constant Ionic compounds (salts) differ in their solubilities Most “insoluble” salts will actually dissolve.

Solubility Equilibria

1 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) For a dissolution process,

Solubility Lesson 6 Changing solubility/Common Ion Effect.

DO NOW: What is dissolution. What is precipitation

SOLUBILITY I. Saturated Solution BaSO 4(s)  Ba 2+ (aq) + SO 4 2- (aq) Equilibrium expresses the degree of solubility of solid in water. Ksp = solubility.

Ksp – Solubility Product Constant

11 ANALYTICAL CHEMISTRY Chem. 243 Chapter 7 Precipitation Titration.

Drill: Determine the KQ/HQ ratio to make a buffer solution with a pH of 4.70 K a for HQ = 3.0 x

Solubility and Complexation Equilibria Chapter 18.

E 12 Water and Soil Solve problems relating to removal of heavy –metal ions and phosphates by chemical precipitation

Chapter 16 Solubility Equilibria. Saturated solutions of “insoluble” salts are another type of chemical equilibria. Ionic compounds that are termed “insoluble”

 Usually consider solids (salts)  Dissolving in water – “like dissolves like” ◦ Forming aqueous solutions.  Remember pure liquids and solids are not.

Chapter 17 Solubility and Simultaneous Equilibria

Ksp Values that indicate how soluble a solution is.

Chapter 7.6 Solubility Equilibria and the Solubility Product Constant

Solubility and Complexation Equilibria

Solubility Constants: Ksp

Unit 5 Cont Ksp.

KSP = Solubility product constant

Solubility Equilibria

Solubility Product Constant

Lesson 7: Predicting Precipitate Formation

The Solubility Product Constant (Ksp)

Lesson # 5 The Solubility Product

Solubility and Complex-Ion Equilibria

Solubility Remember, solubility means that the solute dissolves in water, and also that there are solubility rules that according to the AP Board, you.

Solubility Lesson 8 Review Notes.

Lesson 2: Solubility Calculations

Ksp Values that indicate how soluble a solute is.

Solubility Lesson 7 Changing solubility.

Solubility product constant for slightly soluble salt

Solubility Constant.

Solubility Product Constant

Chem 30: Solubility The Common Ion Effect.

Solubility Product Constant

AP Chem Get Equilibrium Practice Stamped

Name: Nissana Khan Class: L6 Module 2- Kinetics and Equilibria

Solubility Equilibria

Ksp Values that indicate how soluble a solute is.

Presentation transcript:

Lesson 6: The Solubility Product Unit 3: Solubility Lesson 6: The Solubility Product

The Solubility Product For a solubility equilibrium, Keq is given a special name – the solubility product constant (Ksp). The equilibrium expression is called the solubility product expression. E.g. For CaF2(s) Ca2+(aq) + 2 F-(aq), Ksp = [Ca2+][F-]2

Important! In a saturated solution, the solubility product is the ion concentrations multiplied together, while the solubility of a substance is the concentration of that substance.

The Meaning of Ksp Since the value of Ksp depends on the concentrations of the ions, a larger value of Ksp indicates a more soluble salt, and vice versa. Try This: Which of the following salts is the most soluble? The least? AgCl ; Ksp = 1.8x10-10 AgI ; Ksp = 8.5x10-17 AgBr ; Ksp = 5.4x10-13 5 min

Brain Break – Spot 6 Differences!

Preparing a Saturated Solution Two possible methods: Put a solid compound into water and let it dissolve. The ratio of the ions follows the stoichiometric ratio. Separately add the ions of the compound into water. We do not know the ratio of the ions unless we are given the experimental values! Use CaF2 as an example. – 5 min

Ksp Calculations Example 1: A solution in equilibrium with a precipitate of BaF2 contains 4.59x10-2 M Ba2+ and 2.00x10-3 M F-. What is Ksp for BaF2? Example 2: A saturated solution of BaF2 contains 3.58x10-3 mol of BaF2 in 1.00 L of solution. What is Ksp for BaF2? Example 3: What is the [Mg2+] in a saturated solution of Mg(OH)2? For #3, let x=[Mg(OH)2]dissolved then solve using Ksp. – 15 min

Practice Pg. 91 #40 Pg. 95 #42-43, 46-47, and 54 5 min