TITRATIONS AND PH CURVES AP CHEM CH 15. Review H-H What is the pH of a buffer that is made by dissolving 50.0g of sodium acetate in 500.mL of 0.300M acetic.

Slides:

Advertisements

Similar presentations

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

Advertisements

Applications of aqueous equilibria Neutralization Common-Ion effect Buffers Titration curves Solubility and K sp.

Acid/Base Chemistry Part 4 (5.6) Science 10 CT05D06 Resource: Brown, Ford, Ryan, IB Chem.

AQUEOUS EQUILIBRIA AP Chapter 17.

Buffer This. There are two common kinds of buffer solutions: 1Solutions made from a weak acid plus a soluble ionic salt of the weak acid. 2Solutions made.

Buffers and Titrations

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

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?

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.

Lecture 183/4/05 Spring Break QUIZ. Quiz 6 1. What is the pH of a buffer solution containing 0.3 M HNO 2 and 0.25 M NaNO 2 ? K a (HNO 2 ) = 4.5 x

Acid/Base Titrations. Titrations Titration Curve – always calculate equivalent point first Strong Acid/Strong Base Regions that require “different” calculations.

ANALYTICAL CHEMISTRY CHEM 3811 CHAPTER 10 DR. AUGUSTINE OFORI AGYEMAN Assistant professor of chemistry Department of natural sciences Clayton state university.

Strong Acid-Base Titrations Chapter 17. Neutralization Reactions Review Generally, when solutions of an acid and a base are combined, the products are.

Titration Curves. pH mL of Base added 7 O Strong acid with strong Base O Equivalence at pH 7.

© University of South Carolina Board of Trustees Chapt. 16 More Acids and Bases Sec. 2 Titration: Strong Acid + Strong Base.

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

Chapter 16 Notes1 Chapter 16 Aqueous Equilibria: Applications 1. neutralization reactions 2. common ion effect; buffers 3. titrations strong acid - strong.

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

1 TitrationsTitrations pHpH Titrant volume, mL At what point in a reaction does neutralization occur?

Titration Calculations Weak Acid and Strong Base.

Neutralization of Acids and Bases. Titrations Standard Solution Sample Solutio n Burett e Primary Standard with a precisely known [ ] Unknown [ ] Sample.

Acid/Base Chemistry Part II CHEM 2124 – General Chemistry II Alfred State College Professor Bensley.

Additional Aspects of Aqueous Equilibria. Buffer Solutions solution that resists changes in pH upon addition of small amounts of strong acid or base consists.

Titration What is It? Acid and base combined together Graph of pH as a function of volume of titrant is called a titration curve.

Chapter 19 Buffers and Titrations. The Common Ion Effect & Buffer Solutions 2 ______________- solutions in which the same ion is produced by two different.

Titration. Weak Acid/Strong Base Titration Curve pH starts higher Rapid rise and then levels into a zone where pH doesn’t change much (buffering zone)

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

Neutralization Of strong acids and bases. Example1 1- How many ml of M H 2 SO 4 are required to neutralize exactly 525 ml of 0.06 M KOH? 2- What.

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

1081. y = 1.0 x M [OH - ] = 1.0 x M 1082.

Write chemical reactions that describe:

Addition of Strong Acids or Bases to Buffers -- Reactions between strong acids/bases and weak bases/acids proceed to completion. -- We assume that the.

Acid - Base Titration. What is a Titration? A titration is a procedure used in chemistry to determine the concentration of an unknown acid or base. A.

Why do Titration Curves Look Like THAT ???? 1/4/20161.

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

Chapter 15 Applications 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 ______.

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

BUFFERS SUROVIEC SPRING 2014 Chapter I. Buffer Solutions A. Buffer is a solution that resists a change in pH with the addition of small amounts.

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

See summary: top of p.778 in textbook

PART A M C V C = M D _______ V D = (1.0 M)(5.0 mL) ___________________ (50.0 mL) = 0.10 M HC 2 H 3 O 2.

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

ACID-BASE EQUILIBRIA AP CHEM CH 15. The Common Ion Effect The shift in equilibrium that occurs because of the addition of an ion already involved in the.

Chapter 17 Section 3. © 2009, Prentice-Hall, Inc. Titration In this technique a known concentration of base (or acid) is slowly added to a solution of.

Titration Curves. Problem   50.0 mL of 0.10 M acetic acid (K a = 1.8 x ) are titrated with 0.10 M NaOH. Calculate the pH after the additions of.

Buffers. Introduction Buffers are important in biochemical processes. Whether they occur naturally in plasma or in the cytosol of cells, buffers assure.

Acid-Base Titrations End point and equivalence point

Titration and pH Curves.

Ionic Equilibria: Part II Buffers and Titration Curves

Weak Acid/ Strong Base Titrations Weak Base/ Strong Acid Titrations

Acids & Bases III. Titration.

Chem. 1B – 10/4 Lecture.

CHEM 121 Chapter 9 Winter 2014.

Unit 5: Acid-Base Calculations Lesson 4: Mixing Strong Acids + Bases

-5 M Review: 50 mL of 0.1 M carbonic acid, H2CO3, with an initial pH of 3.5, is titrated with 0.2 M lithium hydroxide, LiOH. What volume of.

Titrations & Buffer solutions

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

Ionic Equilibria: Part II Buffers and Titration Curves

Acid-base Titration Calculations:

AP Chem Take out HW to be checked Today: Acid-Base Titrations.

Review: A buffer solution is prepared by adding moles of ammonium chloride to 500. mL of M ammonia solution. (Ka of NH4+ is 5.6x10-10) a.

Weak acid – strong base titrations:

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

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

The Common Ion Effect The solubility of a partially soluble salt is decreased when a common ion is added. Consider the equilibrium established when acetic.

Buffers and titrations

Presentation transcript:

TITRATIONS AND PH CURVES AP CHEM CH 15

Review H-H What is the pH of a buffer that is made by dissolving 50.0g of sodium acetate in 500.mL of 0.300M acetic acid? Assume the volume remains constant.

STRONG ACID – STRONG BASE TITRATIONS The net ionic equation is: Reaction continues to completion The mole is an inconveniently large unit Stoichiometry, not equilibrium

Consider the titration of 50.0mL of 0.200M nitric acid with 0.100M NaOH Amount of NaOH added (mL 0.100M NaOH) pH of resulting solution 0 mL 10 mL 20 mL 50 mL 100 mL 150 mL 200 mL Calculate the pH after: a) No NaOH has been added b)10.0mL of NaOH are added c)20.0mL of NaOH are added d)50.0mL of NaOH are added e)100.0mL of NaOH are added f)150.0mL of NaOH are added g)200.0 mL of NaOH are added

pH Curve of Previous Problem

WEAK ACID – STRONG BASE TITRATIONS The net ionic equation is: STEP ONE: STOICHIOMETRY STEP TWO: EQUILIBRIUM PROBLEM

Consider the titration of 50.0mL of 0.100M acetic acid with 0.100M NaOH Amount of NaOH added (mL 0.100M NaOH) pH of resulting solution 0 mL 10 mL 25 mL 40 mL 50 mL 60 mL 75 mL Calculate the pH after: a) No NaOH has been added b)10.0mL of NaOH are added c)25.0mL of NaOH are added d)40.0mL of NaOH are added e)50.0mL of NaOH are added f)60.0mL of NaOH are added g)75.0 mL of NaOH are added

pH Curve of Previous Problem

WEAK BASE – STRONG ACD TITRATIONS The net ionic equation is: STEP ONE: STOICHIOMETRY STEP TWO: EQUILIBRIUM PROBLEM

Consider the titration of 100.0mL of 0.050M ammonia with 0.100M HCl Amount of HCl added (mL 0.100M HCl) pH of resulting solution 0 mL 10 mL 25 mL 50 mL 60 mL Calculate the pH after: a) No HCl has been added b)10.0mL of HCl are added c)25.0mL of NaOH are added d)50.0mL of NaOH are added e)60.0mL of NaOH are added

pH Curve of Previous Problem