Chapter 15(b) Applications of Aqueous Equilibria (cont’d)

Slides:

Advertisements

Similar presentations

Raymond Chang 10th edition Chapter 16

Advertisements

Raymond Chang 10th edition Chapter 4

Cu 1+ Cu 2+ MnO 4 1- CrO 4 2- Cr 2 O 7 2- The presence of different ions in aqueous solution can be identified in a number of ways. One method is to.

Precipitation Equilibrium

© 2011 Brooks/Cole, Cengage Learning6 | 1. © 2011 Brooks/Cole, Cengage Learning6 | 2.

Reactions in Aqueous Solutions

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.

Solubility. Solubility “Insoluble” salts are governed by equilibrium reactions, and are really sparingly soluble. There is a dynamic equilibrium between.

11111 Chemistry 132 NT If you ever drop your keys into a river of molten lava, let ‘em go, because, man, they’re gone. Jack Handey.

Chapter 16 Solubility and Complex Ion Equilibria.

Chapter 4(a) Types of Chemical Reactions and Solution Stoichiometry.

Copyright © Houghton Mifflin Company. All rights reserved. 7 | 1 Predicting Whether a Reaction Will Occur “Forces” that drive a reaction: Formation of.

Chapter 16 Acids and Bases. EXIT Copyright © by McDougal Littell. All rights reserved.2 Figure 16.1: Representation of the behavior of acids of different.

Chapter 16 Aqueous Ionic Equilibrium. pH / pOH Calculations Strong acids Strong bases Weak acids Weak bases Salts.

Solubility Equilibrium In saturated solutions dynamic equilibrium exists between undissolved solids and ionic species in solutions Solids continue to dissolve.

Ch. 16: Ionic Equilibria Buffer Solution An acid/base equilibrium system that is capable of maintaining a relatively constant pH even if a small amount.

Ksp and Solubility Equilibria

Chemistry Chapter 17 Applications of Aqueous Equilibria.

Acids and Bases Chapter Copyright © by Houghton Mifflin Company. All rights reserved. 16 Concept of Acids and Bases According to the Arrhenius concept.

Precipitates and Solubility

LO 6.1 The student is able to, given a set of experimental observations regarding physical, chemical, biological, or environmental processes that are reversible,

LO 6.1 The student is able to, given a set of experimental observations regarding physical, chemical, biological, or environmental processes that are reversible,

Chapter 15 Applications of Aqueous Equilibria. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 15–2 QUESTION Suppose the weak.

1 Selective Precipitation  a solution containing several different cations can often be separated by addition of a reagent that will form an insoluble.

Solubility Allows us to flavor foods -- salt & sugar. Solubility of tooth enamel in acids. Allows use of toxic barium sulfate for intestinal x-rays.

1 Acid-Base Equilibria and Solubility Equilibria Chapter 17 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Chapter 15(a) Applications of Aqueous Equilibria.

Solubility and Complex-ion Equilibria. Copyright © Houghton Mifflin Company.All rights reserved. Presentation of Lecture Outlines, 18–2 Solubility Equilibria.

Chapter 18 The Solubility Product Constant. Review Quiz Nuclear Chemistry Thermochemistry –Hess’s Law –Heats (Enthalpies) of…

The Composition of Solutions Copyright © Houghton Mifflin Company. All rights reserved.4–24–2 Which of the following solutions contains the greatest.

By Steven S. Zumdahl & Donald J. DeCoste University of Illinois Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry,

Reactions in Aqueous Solution

Precipitation Reactions ● A reaction in which two solutions are mixed an insoluble solid (precipitate) is formed – Double replacement – ions switch partners.

Chapter 6: Chemical Reactions.  Predict and write equations for precipitation reactions.  Write molecular, complete ionic, and net ionic equations.

Aqueous Equilibria Chapter 17 Additional Aspects of Aqueous Equilibria You love Chemistry You might have doubts, but deep, deep, deep down you know there.

Aqueous Equilibria Chapter 17 Additional Aspects of Aqueous Equilibria.

K sp and Solubility Equilibria. Saturated solutions of salts are another type of chemical equilibrium. Slightly soluble salts establish a dynamic equilibrium.

Aqueous Equilibria Chapter 16 Solubility Equilibria.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois Chapter 15 Applications.

1 Titration Curve of a Weak Base with a Strong Acid.

Which of the following solubility product expressions is incorrect?

Chapter 15 Applications of Aqueous Equilibria. Catalyst Derive the Henderson Hasselbalch equation! DON’T LOOK AT YOUR NOTES.

Some Terminology Soluble – Will dissolve in a solvent Insoluble – Will not dissolve in a solvent Solvent – The substance that dissolves the solute Solute.

Reactions in Aqueous Solution Objectives: 1. Write and balance net ionic equations 2. Use solubility rules to predict the precipitate formed in double.

Chapter 16 Lesson 2 Solubility and Complex Ion Equilibria.

Compounds in Aqueous Solutions When dissolved in water, ionic and molecular compounds behave differently.

Prentice Hall © 2003Chapter 17 Chapter 17 Additional Aspects of Aqueous Equilibria.

Aqueous Equilibria The Common-Ion Effect Consider a solution of acetic acid: NaC 2 H 3 O 2 Le Châtelier says the equilibrium will shift to the ______.

Reactions in Aqueous Solution Chapter 9 Section 3.

Acid-Base Equilibria and Solubility Equilibria Chapter 16.

Will it all dissolve, and if not, how much?. Looking at dissolving of a salt as an equilibrium. If there is not much solid it will all dissolve. As more.

Chapter 1 Ingredients of Change: Functions and Models.

Solubility Equilibria

Copyright©2004 by houghton Mifflin Company. All rights reserved.

Solubility Equilibria

Chapter 16 Solubility and Complex Ion Equilibria.

Qualitative Analysis Reactions that produce an INSOLUBLE SALT.

Zumdahl Zumdahl DeCoste

Solubility Equilibria

Solubility and Complex Ion Equilibria

Solubility and Complex Ion Equilibria

Solubility Equilibria

LO 6.1 The student is able to, given a set of experimental observations regarding physical, chemical, biological, or environmental processes that are reversible,

Solubility Equilibria

LO 6.1 The student is able to, given a set of experimental observations regarding physical, chemical, biological, or environmental processes that are reversible,

Solubility Equilibria

Solubility Equilibria

Unit 11 – Solutions and Ions in Aqueous Solutions

Solubility Equilibria

Presentation transcript:

Chapter 15(b) Applications of Aqueous Equilibria (cont’d)

Copyright © Houghton Mifflin Company. All rights reserved.15b–2 Figure 15.8: The useful pH ranges for several common indicators. Note that most indicators have a useful range of about two pH units, as predicted by the expression pK a ≠ 1.

Copyright © Houghton Mifflin Company. All rights reserved.15b–3

Figure 15.9 The pH curve for the titration of mL of 0.10 M HCl with 0.10 M NaOH.

Figure 15.10: The pH curve for the titration of 50 mL of 0.1 M HC 2 H 3 O 2 with 0.1 M NaOH.

Copyright © Houghton Mifflin Company. All rights reserved.15b–6

Precipitation of bismuth sulfide.

Copyright © Houghton Mifflin Company. All rights reserved.15b–8

Copyright © Houghton Mifflin Company. All rights reserved.15b–9 A potassium chromate solution being added to aqueous silver nitrate, forming silver chromate.

Copyright © Houghton Mifflin Company. All rights reserved.15b–10 Figure 15.11: The separation of Cu 2+ and Hg 2+ from Ni 2+ and Mn 2+ using H 2 S.

Flame test for potassium.

Flame test for sodium.

Figure 15.12: A schematic diagram of the classic method for separating the common cations by selective precipitation.

Copyright © Houghton Mifflin Company. All rights reserved.15b–14 From left to right, cadmium sulfide, chromium(III) hydroxide, aluminum hydroxide, and nickel(II) hydroxide.

Copyright © Houghton Mifflin Company. All rights reserved.15b–15 (left) Aqueous ammonia is added to silver chloride (white). (right) Silver chloride, insoluble in water, dissolves to form Ag(NH 3 ) 2 +(aq) and Cl-(aq).

Figure 15.13: The separation of the Group I ions in the classic scheme of qualitative analysis.