Chapter 9 Acids, Bases, & Salts

Slides:



Advertisements
Similar presentations
Go over Ch Test Summary of this week Questions over the reading Discussion / explanation Homework.
Advertisements

Buffer Capacity Lab.
Applications of aqueous equilibria Neutralization Common-Ion effect Buffers Titration curves Solubility and K sp.
AQUEOUS EQUILIBRIA AP Chapter 17.
PART 4: Salt Hydrolysis and Buffer Solutions
Chapter 16: Aqueous Ionic Equilibria Common Ion Effect Buffer Solutions Titrations Solubility Precipitation Complex Ion Equilibria.
Ch. 16: Aqueous Ionic Equilibrium Dr. Namphol Sinkaset Chem 201: General Chemistry II.
Outline:2/28/07 è Hand in Seminar Reports – to me è Pick up Quiz #6 – from me è Pick up CAPA 14 - outside è 5 more lectures until Exam 2… Today: è End.
Reactions of Acids & Bases
Chapter 8 Acids and Bases
Acid-Base Equilibria and Solubility Equilibria Chapter
1 Announcements & Agenda (02/26/07) You should be reading Ch 10! Quiz on Friday! Bring resource CD to lab! Today Acid & base reactions (8.6) Acid & base.
Buffers: -A buffer solution is that solution that allows solutions to resist large changes in pH upon the addition of limited amounts of acid Or base.
Outline:3/7/07 è Pick up CAPA 15 & 16 - outside è 4 more lectures until Exam 2… Today: è Chapter 18 Buffers Buffer calculations Titrations.
Chapter 16 Acids and Bases. Chapter 16 Table of Contents Acids and Bases 16.2Acid Strength 16.3Water as an Acid and a Base 16.4The pH Scale 16.5.
Aqueous Equilibria © 2009, Prentice-Hall, Inc. The Common-Ion Effect Consider a solution of acetic acid: If acetate ion is added to the solution, Le Châtelier.
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.
Polyprotic Acids & Bases A polyprotic acid can donate more than one H + Carbonic acid: H 2 CO 3 (aq); dissolved CO 2 in water Sulfuric acid: H 2 SO 4 (aq)
Buffer solution دکتر امید رجبی دانشیار گروه شیمی دارویی شیمی عمومی.
1 Chapter 10 Acids and Bases 10.9 Buffers. 2 When an acid or base is added to water, the pH changes drastically. A buffer solution resists a change in.
EQUILIBRIUM Part 1 Common Ion Effect. COMMON ION EFFECT Whenever a weak electrolyte and a strong electrolyte share the same solution, the strong electrolyte.
Chemistry 1011 TOPIC TEXT REFERENCE Acids and Bases
CHM 112 Summer 2007 M. Prushan Acid-Base Equilibria and Solubility Equilibria Chapter 16.
Section 2: Buffered Solutions.  Solutions prepared with common ions have a tendency to resist drastic pH changes even when subjected to the addition.
Unless otherwise stated, all images in this file have been reproduced from: Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 2007 (John Wiley)
  Weak acid/conjugate base mixtures OR weak base/conjugate acid mixtures  “buffers” or reduces the affect of a change in the pH of a solution  Absorbs.
Acid/Base Chemical Equilibria. The Brønsted Definitions  Brønsted Acid  proton donor  Brønsted Base  proton acceptor  Conjugate acid - base pair.
1 Chapter Learning Objectives a.The chemical properties of acids and bases. b.Acids and bases react with each other in a reaction known as neutralization.
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
12 AP Chemistry Buffers. What is a Buffer? A buffer solution is one, which can absorb additions of acids or bases with only slight changes in pH values.
1 Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
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 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
1 TitrationsTitrations pHpH Titrant volume, mL At what point in a reaction does neutralization occur?
Acid-Base Equilibria (Buffers ) Green & Damji Chapter 8, Section 18.2 Chang Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required.
Chapter 17 Additional Aspects of Aqueous Equilibria
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
C. Y. Yeung (CHW, 2009) p.01 Acid-Base Eqm (4): Buffer Solutions Q.:What is the new pH after addition of mol HCl at 298K? (assume no volume change)
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois Chapter 15 Applications.
Strong base neutralizes weak acid Strong acid neutralizes weak base.
19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1. Lactic acid, HC 3 H 5 O 3, has one acidic hydrogen.
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
C H E M I S T R Y Chapter 15 Applications of Aqueous Equilibria.
8.3 Bases Similar to weak acids, weak bases react with water to a solution of ions at equilibrium. The general equation is: B(aq) + H2O(l)  HB+(aq) +
Chemical calculations II
CMH 121 Luca Preziati Chapter 8: Acids and Bases Acid = produces H + An acid is a compound that: 1. Has H somewhere 2. Has the tendency (is capable) of.
Advanced Acid/Base Theory
General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 10.6 Buffers Chapter 10 Acids and Bases © 2013 Pearson Education, Inc. Lectures.
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Chapter 8 Acids.
Equilibrium – Acids and Bases. Review of Acids and Bases Arrhenius Theory of Acids and Bases ▫An acid is a substance that dissociates in water to produce.
Ch 8: Introducing Acids and Bases. pH of precipitation in the United States 2001, and in Europe as reported in 2002.
Chapter 15 Applications of Aqueous Equilibria
Chapter 8 Acids and Bases 8.5 Reactions of Acids and Bases 1 Copyright © 2009 by Pearson Education, Inc.
Chapter 15 Acid–Base Equilibria. Section 15.2 Atomic MassesBuffered Solutions Return to TOC Copyright © Cengage Learning. All rights reserved 2 Key Points.
Applications of Aqueous Equilibria
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
1 Function of the Conjugate Base The function of the acetate ion C 2 H 3 O 2  is to neutralize added H 3 O +. The acetic acid produced by the neutralization.
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Semester 2/2014 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction.
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.
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.
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.
Buffers. Introduction Buffers are important in biochemical processes. Whether they occur naturally in plasma or in the cytosol of cells, buffers assure.
Describe the composition of a buffer solution and explain its action.  What is a buffer solution?  It is an aqueous solution that resists a change.
1 Chapter 14 Acids and Bases 14.9 Acid-Base Properties of Salt Solutions Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings.
11.9 Buffers A buffer solution maintains the pH by neutralizing small amounts of added acid or base. An acid must be present to react with any OH− added,
Chapter 14 Acids and Bases
Chapter 8 Acids and Bases
Chapter 10 Acids and Bases
Chapter 8 Acids and Bases
Presentation transcript:

Chapter 9 Acids, Bases, & Salts 9.13 Buffers

Buffers When an acid or base is added to water, the pH changes drastically. to a buffer solution, the pH is maintained; pH does not change.

Buffers Buffers resist changes in pH from the addition of acid or base. in the body, absorb H3O+ or OH- from foods and cellular processes to maintain pH. are important in the proper functioning of cells and blood. in blood maintain a pH close to 7.4. A change in the pH of the blood affects the uptake of oxygen and cellular processes.

Components of a Buffer A buffer solution contains a combination of acid-base conjugate pairs. may contain a weak acid and a salt of its conjugate base. typically has equal concentrations of a weak acid and its salt. may also contain a weak base and a salt of the conjugate acid.

Buffer Action In the acetic acid/acetate buffer with acetic acid (CH3COOH) and sodium acetate (CH3COONa) The salt produces acetate ions and sodium ions. CH3COONa(aq) CH3COO-(aq) + Na+ (aq) The salt is added to provide a higher concentration of the conjugate base CH3COO- than the weak acid alone. CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq) Large amount Large amount

Function of the Weak Acid in a Buffer The function of the weak acid in a buffer is to neutralize a base. The acetate ion produced adds to the available acetate. CH3COOH + OH− CH3COO− + H2O acetic acid base acetate ion water Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

Function of the Conjugate Base The function of the acetate ion CH3COO− is to neutralize H3O+ from acids. The acetic acid produced contributes to the available weak acid. CH3COO− + H3O+ CH3COOH + H2O acetate ion acid acetic acid water Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

Summary of Buffer Action Buffer action occurs as the weak acid in a buffer neutralizes base. the conjugate base in the buffer neutralizes acid. the pH of the solution is maintained.

Learning Check Which combination(s) make a buffer solution? A. HCl and KCl B. H2CO3 and NaHCO3 C. H3PO4 and NaCl D. CH3COOH and CH3COOK

Solution B. H2CO3 + NaHCO3 A weak acid and its salt D. CH3COOH + CH3COOK A weak acid and its salt.

The pH of buffers The pH of buffers can be calculated using Ka = or Kb = Where the equation are rearranged to solve for [H3O+]=[H+] or [OH-] [H+] = Ka or [OH-] = Kb Using properties of logarithm (log) concept pH = pKa + log or pOH = pKb + log [H3O+][A-] [OH-][HB+] [HA] [B] [B] [HA] [HB+] [A-] [HA] [B] [A-] [HB+] Henderson-Hasselbach equation

Learning Check Calculate the pH of a buffer solution that contains 0.10 mol of acetic acid (CH3COOH) and 0.10 mol of sodium acetate (CH3COONa) per liter. (pKa for acetic acid is 4.74 given in Table 9.9, pg 294 of your book) CH3COOH + H2O  CH3COONa + H3O+

Solution pH = pKa + log pH = 4.74 + log pH = 4.74 + log(1) = 4.74 Note that pH = pKa when the concentration of the acid and conjugate base are equal [CH3COOH] acid [CH3COONa] conjugate base [0.10 mol/L] [0.10 mol/L]

Learning Check If the Ka of an acid is 1.0x10-6, pH = 3.00, and the concentration of the unionized acid is 1.0x10-2 M, what is the concentration of the salt?

Solution Given: pH = 3.00, Ka = 1.0x10-6 M, and [HA] = 1.0x10-2 M solve for [H3O+] = 10-pH = 10-3 = 1.0x10-3 M Ka = rearrange equation to solve for the salt [A-] [A-] = = 1.0x10-6 M [A-] = 1.0x10-5 M [H3O+][A-] [HA] [HA]_ [1.0x10-2 M]_ Ka [H3O+] [1.0x10-3 M]