Ch 14/15 Test Wed up to and including 15.5. In Part A of your lab you created a solution that had equal moles of HA and A - and If mol HA = mol A - could.

Slides:

Advertisements

Similar presentations

III. Titration (p ) Ch. 15 & 16 - Acids & Bases.

Advertisements

AQUEOUS EQUILIBRIA AP Chapter 17.

CHAPTER 15: APPLICATIONS OF AQUEOUS EQUILIBRIA Dr. Aimée Tomlinson Chem 1212.

Chapter 16: Aqueous Ionic Equilibria Common Ion Effect Buffer Solutions Titrations Solubility Precipitation Complex Ion Equilibria.

Entry Task: Feb 12th Tuesday

Buffers. Buffered Solutions. A buffered solution is one that resists a change in its pH when either hydroxide ions or protons (H 3 O + ) are added. Very.

Acids and Bases Titrations AP Chemistry. Neutralization Reactions and Titrations Neutralization Reactions Strong acid + Strong Base  Salt + Water HCl.

Acid-Base Equilibria Common Ion Effect in Acids and Bases Buffer Solutions for Controlling pH Buffer Capacity pH-Titration Curves Acid-Base Titration Indicators.

Slide 1 of 45  Worked Examples Follow:. Slide 2 of 45.

Lecture 183/1/06. What is a buffer? pH of a buffer system What is the pH of a buffer that is 0.12 M lactic acid HC 3 H 5 O 3 and 0.1 M sodium lactate?

Reactions of Acids & Bases

Prentice-Hall © 2007 General Chemistry: Chapter 17 Slide 1 of 45 Chapter 17: Additional Aspects of Acid-Base Equilibria CHEMISTRY Ninth Edition GENERAL.

Lecture 223/17/06 Research Club Meeting  Today at 1:30  TSB 155  Free pizza Research Colloquium  April 4  Deadline March 27.

Lecture 193/12/07. Sample (100 mL – 0.1 M) Titrant (0.2 M) Initial pH pH at equivalence point pH at 2X equivalence point X-axis at equivalence point Strong.

Calculate the pH of a solution that is 0.20 M in NaCH 3 COO and 0.10 M in CH 3 COOH

Chapter 15 Applications of Aqueous Equilibria. The Common-Ion Effect Common-Ion Effect: The shift in the position of an equilibrium on addition of a substance.

Buffers AP Chemistry.

Acid-Base Titrations.

Chapter 15 Buffers Titration pH Curves

Acids and Bases Chapter 8. Polyprotic acids However, the most ionization occurs in the first step.  K a1 >> K a2 > K a3.... Consequently, the [H + ]

Chapter 19 More about ACID-BASES. Self-Ionization of Water Two water molecules produce a hydronium ion & a hydroxide ion by the transfer of a proton.

Chapter 18 – Other Aspects of Aqueous Equilibria Objectives: 1.Apply the common ion effect. 2.Describe the control of pH in aqueous solutions with buffers.

Additional Aqueous Equilibria CHAPTER 16

Titrations of acids and bases. HA + H 2 O H 3 O + + A -

Acid-base equilibria & common ions Consider solution containing HF (weak acid) and salt NaF What effect does presence of NaF have on dissociation equilibrium.

Updates Assignment 06 is due Mon., March 12 (in class) Midterm 2 is Thurs., March 15 and will cover Chapters 16 & 17 –Huggins 10, 7-8pm –For conflicts:

Chapter 17 Additional Aspects of Acid-Base Equilibria

Acid-Base Equilibria and Solubility Equilibria Chapter 16 Dr. Ali Bumajdad.

(equimolar amounts of acid and base have reacted)

Section 16.3 Titrations and Buffers 1.To know how to neutralize acids and bases (titration) Learning Goal.

11111 Chemistry 132 NT Instead of having “answers” on a math test, they should just call them “ impressions”, and if you got a different “impression”,

Chapter 15 Applications of Aqueous Equilibria Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1.

Chapter 16.7 and 16.8 Acid –Base Titrations Buffered Solutions.

© University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare.

Ch. 17 – Other Aspects of Equilibrium The concept of equilibrium may be used to describe the solubility of salts and the buffering action of a solution.

Acid-base equilibria & common ions Consider solution containing HF (weak acid) and salt NaF Species in solution: HF, H 2 O, Na +, F - What effect does.

Acid/Base Titration Buffers. Buffers A mixture composed of a weak acid and its conjugate base (acidic buffer) OR weak base and its conjugate acid (basic.

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

1 How Much Does the pH of a Buffer Change When an Acid or Base Is Added?  though buffers do resist change in pH when acid or base are added to them, their.

Entry Task: Jan 22 nd Thursday Turn in Determine Ka Lab.

C H E M I S T R Y Chapter 15 Applications of Aqueous Equilibria.

AP Chapter 17 Ionic Equilibria of Weak Electrolytes.

Titration and pH Curves..   A titration curve is a plot of pH vs. volume of added titrant.

Chapter 17 Sections 1-3 Common ions, Buffers and Titration © 2012 Pearson Education, Inc.

bjects/3312/ /blb1703.html.

Titrations Definition: Volumetric determination of the amount of an acid or base by addition of a standard acid or base until neutralization.

Ch 17: Additional Aspects of Aqueous Equilibria Brown, LeMay Ch 17 AP Chemistry.

Chapter 15 Acid–Base Equilibria. Section 15.2 Atomic MassesBuffered Solutions Return to TOC Copyright © Cengage Learning. All rights reserved 2 Key Points.

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 ______.

C. Johannesson III. Titration Ch. 14 & 15 - Acids & Bases.

Applications of Aqueous Equilibria

Titrations. Standard Solution Sample Solution Burette A titration is a volumetric analysis technique used to find the [unknown] of a sample solution by.

The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with one of the products.

Common Ion Effect, Buffers, and Titration March 4/6, 2015.

Chemistry Chem Olympiad Mini Quiz Buffer Notes Pancake-Ice Cream Sandwich Treat (throughout the class period)

BUFFERS Mixture of an acid and its conjugate base. Buffer solution  resists change in pH when acids or bases are added or when dilution occurs. Mix: A.

TUTORIAL 5. LEARNING OUTCOMES By the end of this session the student should be able to: Compare between different titration curves. Select an Indicator.

Obj. finish 17.2, ) The pH range is the range of pH values over which a buffer system works effectively. 2.) It is best to choose an acid with.

Acid Reactions I Acids & Active Metals: Single replacement reactions Active metals (K, Na, Ca, Mg, Al, Zn, Fe, Sn) Produce H 2 Oxidation-reduction reactions.

PH Titration Curves & Indicators. Objectives 1)Review AS understanding of titration calculations for: Reacting volumes & Reactant concentrations 1)Predict,

C. Y. Yeung (CHW, 2009) p.01 Titration Curves Acid-Base Eqm (5): Titration Curves Titration Curves Acid-Base Eqm (6): Titration Curves Plotting the Titration.

CHAPTER 17: ADDITIONAL ASPECTS OF AQUEOUS EQUILIBRIA Dr. Aimée Tomlinson Chem 1212.

Chapter 16: Acid Base Equilibria and Solubility Equilibria Common Ion Effects Buffers Titration Solubility.

Titration A standard solution is used to determine the concentration of another solution.

Buffers In general, what is a buffer?????

Acid-Base Equilibria Common Ion Effect on pH of Acids and Bases

Lecture PowerPoint Chemistry The Molecular Nature of Matter and Change

Week 5. Buffers solutions

Acid-Base Reactions: TITRATION

Ch. 15 & 16 - Acids & Bases III. Titration (p )

Presentation transcript:

Ch 14/15 Test Wed up to and including 15.5

In Part A of your lab you created a solution that had equal moles of HA and A - and If mol HA = mol A - could we find pH? How?

Based on the results of your mini lab, part B… 1.What is a buffer? 2.What is it composed of? 3.Does it have any limitations?

Which of the following mixtures would be described as a buffer solution? mL of 0.1 M NaOH and 25.0 mL of 0.1 M HCl mL of 0.1 M CH 3 COOH and 25.0 mL of 0.1 M HCl mL of 0.05 M NaOH and 25.0 mL of 0.1 M CH 3 COOH mL of 0.1 M NaF and 25.0 mL of 0.1 M HF

PROBLEM:The molecular scenes below represent samples of four HA/A - buffers. (HA is blue and green, A - is green, and other ions and water are not shown.) (a)Which buffer has the highest pH? (b)Which buffer has the greatest capacity? Why? (c)Should we add a small amount of concentrated strong acid or strong base to convert sample 1 to sample 2 (assuming no volume changes)?

Find the pH of 1.The original buffer: 25.0 mL of 0.1 M NaF and 25.0 mL of 0.1 M HF 2. In what range would this buffer be the most effective? 3. The solution if 10 mL of 0.10 M NaOH is added Compare to scenario if 10 mL of 0.10 M NaOH was added to 50 mL of water

Preparing a Buffer A buffer of pH 10.0 is needed to study the effects of acid rain on soil. Which of the following mixtures would be the best to choose? NaC 6 H 5 COO, C 6 H 5 COOH (K a of C 6 H 5 COOH = 6.3x10 -5 ) Na 2 CO 3, NaHCO 3 (K a of HCO 3 - = 4.7x ) How many grams of Na 2 CO 3 must be added to 1.5 L of 0.20 M NaHCO 3 to make the buffer?

Titration Reaction of acid and base Neutralization is a one way reaction (DR) The neutralization reaction can produce an equilibrium system between a weak acid and its conjugate base (or weak base and conjugate acid)

Titration Curve Plot pH vs. volume of titrant added Let’s produce a titration curve for the reaction of a strong acid ( 0.10 M HCl 50 mL) with a strong base ( 0.20 M NaOH)

What if a weak acid was titrated against NaOH instead? 50 mL 0.10 M HC 2 H 3 O 2 (instead of HCl) titrated against strong base ( 0.20 M NaOH) What is the pH at the half equivalence point? What is the significance of this point? How would the titration curve change?

We need to titrate 0.25 M NH 3 with 0.15 M HCl. Which indicator would be best? IndicatorpKapH rangeColor Change Bromocresol green Yellow -> blue Bromothymol blue Yellow->blue Phenolphthalein Colorless->Pink

What is this?