Applications of Aqueous Equilibria Chapter 15. Titration Curves & Indicators Sections 4-5

Size: px
Start display at page:

Download "Applications of Aqueous Equilibria Chapter 15. Titration Curves & Indicators Sections 4-5"

Transcription

1 Applications of Aqueous Equilibria Chapter 15 Titration Curves & Indicators Sections 45

2 Strong Acid vs. Strong Base Titration Titrate 50.0 ml of M HNO 3 with M NaOH What is the ph when no NaOH has been added? 0.200M = [H + ] ph = log =.699 What is the ph when 10.0 ml of 0.10 M NaOH has been added? Species in solution: H +, NO 3, Na +, OH, H 2 O H + + OH H 2 O 50.0mL 10.0mL 0.200M 0.100M LIMITING HAVE 10.0mmol 1.00mmol NEED 1.00mmol 1.00mmol XS 9.00mmol 0mmol 9.00mmol H mL mL SPECTATORS = 0.15 M H + ph = log 0.15 = 0.82 What would it look like at the equivalence point? STOICHIOMETRY!.. BEFORE THE EQUIVALENCE POINT..

3 Strong Acid vs. Strong Base Titration Titrate 50.0 ml of M HNO 3 with M NaOH What is the ph when ml of 0.10 M NaOH has been added? H + + OH H 2 O 50.0mL 150.0mL 0.200M 0.100M LIMITING HAVE 10.0mmol 15.0mmol NEED 10.0mmol 10.0mmol XS 0 mmol 5.0mmol 5.0mmol OH = M OH 50.0mL mL [H + ] = 1.0 x /0.025 = 4.0 x ph = log 4.0 x = AFTER THE EQUIVALENCE POINT..

4 Strong Acid vs Strong Base Titration Curves Small volumes make large ph changes Figure 15.1 & 15.2 page 699

5 Weak Acid vs. Strong Base Titration Similar to buffer calculations Even though the acid is weak it reacts completely with the OH added Titrate 50.0 ml of M HC 2 H 3 O 2 (K a = 1.8 x 10 5 ) with 0.10 M NaOH What is the ph when no NaOH has been added? HC 2 H 3 O 2 H + + C 2 H 3 O x 10 5 = 0.10M 0 0 x +x +x 0.10x x x x ph = log 1.8 x 10 6 = 2.87 x = 1.8 x 10 6 = [H + ] EQUILIBRIUM!.. BEFORE THE EQUIVALENCE POINT..

6 Weak Acid vs. Strong Base Titration Titrate 50.0 ml of M HC 2 H 3 O 2 (K a = 1.8 x 10 5 ) with 0.10 M NaOH What is the ph when 10.0 ml of 0.10 M NaOH has been added? Species in solution before reaction: HC 2 H 3 O 2, Na +, OH, H 2 O HAVE NEED XS HC 2 H 3 O 2 + OH C 2 H 3 O 2 + H 2 O 50.0mL 10.0mL 0.100M 0.100M 1.00mmol 4.00mmol 4.00mmol HC 2 H 3 O mL mL 1.00mmol C 2 H 3 O mL mL 1.00mmol 1.00mmol 0mmol LIMITING = M HC 2 H 3 O 2 = M C 2 H 3 O 2 ACID 1.00mmol BASE STOICHIOMETRY! Use these for an equilibrium problem to find [H + ].. BEFORE THE EQUIVALENCE POINT..

7 Weak Acid vs. Strong Base Titration Titrate 50.0 ml of M HC 2 H 3 O 2 (K a = 1.8 x 10 5 ) with 0.10 M NaOH What is the ph when 10.0 ml of 0.10 M NaOH has been added? Use M HC 2 H 3 O 2 and M C 2 H 3 O 2 HC 2 H 3 O 2 H + + C 2 H 3 O M M x +x +x 0.067x x x 1.8 x 10 5 = 0.017x ph = log 7.1 x 10 5 = 4.15 x = 7.1 x 10 5 = [H + ] Halfway to the equivalence point [HC 2 H 3 O 2 ] 0 = [C 2 H 3 O 2 ] 0 so K a = [H + ] and pk a = ph EQUILIBRIUM!.. BEFORE THE EQUIVALENCE POINT..

8 Weak Acid vs. Strong Base Titration Titrate 50.0 ml of M HC 2 H 3 O 2 (K a = 1.8 x 10 5 ) with 0.10 M NaOH What is the ph when 50.0 ml of 0.10 M NaOH has been added? Species in solution before reaction: HC 2 H 3 O 2, Na +, OH, H 2 O HAVE NEED XS HC 2 H 3 O 2 + OH C 2 H 3 O 2 + H 2 O 50.0mL 50.0mL 0.100M 0.100M 0mmol C 2 H 3 O mL mL 0mmol ACID BASE STOICHIOMETRY! = M C 2 H 3 O 2 This is a base that will force water to be an acid!!.. AT THE EQUIVALENCE POINT..

9 Weak Acid vs. Strong Base Titration Titrate 50.0 ml of M HC 2 H 3 O 2 (K a = 1.8 x 10 5 ) with 0.10 M NaOH What is the ph when 50.0 ml of 0.10 M NaOH has been added? Use M C 2 H 3 O 2 that reacts with water C 2 H 3 O 2 + H 2 O HC 2 H 3 O 2 + OH 0.050M 0 0 x +x +x 0.050x x x Find K b from K w =K a x K b K b = 5.6 x = x [H + ] = 1.0 x / 5.3 x 10 6 = 1.9 x 10 9 ph = log 1.9 x 10 9 = 8.72 x = 5.3 x 10 6 = [OH ] weak acid & strong base equivalence point >7 because the anion left in solution is a (conjugate) base EQUILIBRIUM!.. AT THE EQUIVALENCE POINT..

10 Weak Acid vs. Strong Base Titration Titrate 50.0 ml of M HC 2 H 3 O 2 (K a = 1.8 x 10 5 ) with 0.10 M NaOH What is the ph when 60.0 ml of 0.10 M NaOH has been added? HAVE NEED XS HC 2 H 3 O 2 + OH C 2 H 3 O 2 + H 2 O 60.0mL 50.0mL 0.100M 0.100M LIMITING 0mmol 1.00mmol OH 60.0mL mL 6.00mmol 1.00mmol = 9.10 x 10 3 M OH weak base strong base USE ONLY THE STRONG. [H + ] = 1.0 x / 9.10 x 10 3 = 1.1 x M ph= STOICHIOMETRY!.. AFTER THE EQUIVALENCE POINT.. Try Sample Exercise 15.9 on page 705 or #55, 57, 58

11 Weak Acid vs Strong Base Titration Curves Weak acid increases in ph more rapidly before the equivalence point Levels off near the halfway point caused by buffering effects because [HA] = [A ]!!! Equivalence point is determined by stoichiometry not ph. SA & SB =7 WA & SB >7 SA & WB <7 Figure 15.3 page 704

12 Comparing Weak Acids The strength of a weak acid has no bearing on the amount of acid needed at the equivalence point. Equivalence point is determined by stoichiometry not ph! The strength of a weak acid does affect the ph of the equivalence point. The weaker the acid the higher the ph at the equivalence point. It also affects the shape of the curve. Figure 15.4 page 707

13 Calculating Ka Sample Exercise page 707 Given 100.0mL H 2 O, 2.0 mmol of HA with 20.0mL of M NaOH and a ph of HA + OH A + H 2 O 100.0mL 20.0mL 0.050M LIMITING HAVE 2.00mmol 1.00mmol 1.00mmol /120.0mL = M = [A ] 0 NEED 1.00mmol XS 1.00mmol /120.0mL = M = [HA] 0 ph = 6.00 [H + ] eq = 1.0 x 10 6 M HA H + + A x +x +x x 1.0x x approximate K a = [1.0x10 6 ] [ ] K a = 1.0x This was halfway to the equivalence point. Try #63

14 The reaction of NH 3 and HCl Weak Base vs Strong Acid Species in reaction NH 3, H +, Cl, H 2 O NH 3 + H + NH 4 + base acid from HCl conjugate acid goes to completion use stoichiometry NH H 2 0 NH 3 + H 3 O + acid water (base) conjugate base hydronium does not go to completion use equilibrium calculations The ph is less than 7 because the weak base produces a conjugate acid.

15 Endpoint when the indicator in a titration changes color not necessarily the same as equivalence point Indicators complex molecules that are weak acids, H(In) and their conjugate base, In, in equilibrium the conjugate base, In, is a different color than the H(In) HIn H + + In K a = 1.0 x 10 8 K a = [H+ ] [In ] [HIn] OR AcidBase Indicators K a = [H + ] [In ] [HIn] If an acid is added [H + ] = 1.0 x 10 1 M then 1.0 x [In ] = = There is more [HIn] 1.0 x x 10 7 [HIn] so you will see its color [In ] How much In must be present to see a change? [HIn] = 1 10

16 AcidBase Indicators Given K a, which ph will cause a change? Use [In ] / [HIn] = 1/10 K a = [H+ ] [In ] [HIn] 1.0x 10 7 = [H+ ] 1 10 [In Or use the HendersonHasselbalch ph = pka ] + log [HIn] [1] log = 1 ph = pk a 1 [10] Flipping [In ]/[HIn] to [HIn]/[In ] gives ph = pk a + 1 So now you have a range. The range for indicators is pk a ± 1. If K a = 1 x 10 7 then [HIn] [In ] yellow blue

17 When choosing an indicator make the endpoint and equivalence point as close as possible. AcidBase Indicators Figure 15.9 page 716

18 Figure 15.8 AcidBase Indicators

Chapter 17 Additional Aspects of Aqueous Equilibria (Part A)

Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) What is a dominant equilibrium? How do we define major species? Reactions between acids and bases 1. Strong Acids + Strong Base The reaction

More information

Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations

Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations Sec 1 The Common-Ion Effect: The dissociation of a weak electrolyte decreases when a strong electrolyte that has an ion in common with

More information

Chapter 17 Additional Aspects of Aqueous Equilibria (Part A)

Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) Often, there are many equilibria going on in an aqueous solution. So, we must determine the dominant equilibrium (i.e. the equilibrium reaction

More information

Chapter 16: Applications of Aqueous Equilibrium Part 2. Acid-Base Titrations

Chapter 16: Applications of Aqueous Equilibrium Part 2. Acid-Base Titrations Chapter 16: Applications of Aqueous Equilibrium Part 2 Acid-Base Titrations When you add an acid and a base together, a neutralization rxn occurs. In the lab, we do neutralization rxns all the time as

More information

Understanding the shapes of acid-base titration curves AP Chemistry

Understanding the shapes of acid-base titration curves AP Chemistry Understanding the shapes of acidbase titration curves AP Chemistry Neutralization Reactions go to Completion Every acidbase reaction produces another acid and another base. A neutralization reaction is

More information

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and

More information

Chapter 15. Acid-Base Equilibria

Chapter 15. Acid-Base Equilibria Chapter 15 Acid-Base Equilibria Section 15.1 Solutions of Acids or Bases Containing a Common Ion Common Ion Effect Shift in equilibrium position that occurs because of the addition of an ion already involved

More information

HALFWAY to EQUIVALENCE POINT: ph = pk a of the acid being titrated.

HALFWAY to EQUIVALENCE POINT: ph = pk a of the acid being titrated. CHEMISTRY 109 Help Sheet #33 Titrations Chapter 15 (Part II); Section 15.2 ** Cover topics appropriate for your lecture** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets:

More information

Titration Curves equivalence point

Titration Curves equivalence point 1 Here is an example of a titration curve, produced when a strong base is added to a strong acid. This curve shows how ph varies as 0.100 M NaOH is added to 50.0 ml of 0.100 M HCl. The equivalence point

More information

Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute)

Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) CHAPTER 16: ACID-BASE EQUILIBRIA Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) A. Weak Monoprotic Acids. (Section 16.1) 1. Solution of Acetic Acid: 2. See Table

More information

Chemistry 132 NT. Acid-Base Equilibria

Chemistry 132 NT. Acid-Base Equilibria Chemistry 132 NT Instead of having answers on a math test, they should just call them impressions, and if you got a different impression, so what, can t we all be brothers? Jack Handey 1 2 Chem 132 NT

More information

Acid Base Titrations

Acid Base Titrations ChemActivity CA47b Acid Base Titrations Model 1 Titration of a strong acid with a strong base. 20.00 ml of HNO 3 is titrated with 0.10 M NaOH. The acid-base reaction is The net ionic reaction is HNO 3

More information

Questions #4-5 The following two questions refer to the following system: A 1.0L solution contains 0.25M HF and 0.60M NaF (Ka for HF = 7.2 x 10-4 ).

Questions #4-5 The following two questions refer to the following system: A 1.0L solution contains 0.25M HF and 0.60M NaF (Ka for HF = 7.2 x 10-4 ). Multiple Choice 1) A solution contains 0.250 M HA (K a = 1.0 x 10-6 ) and 0.45 M NaA. What is the ph after 0.10 mole of HCl is added to 1.00L of this solution? a. 3.17 b. 3.23 c. 6.00 d. 10.77 e. 10.83

More information

Titration of a Weak Acid with a Strong Base

Titration of a Weak Acid with a Strong Base Titration of a Weak Acid with a Strong Base Weak Acid w/ Strong Base Overall: INITIAL ph: Weak acids do not fully dissociate we need to do an ICE table to determine initial ph. We expect it to be weakly

More information

Name: Date: Period: #: TITRATION NOTES

Name: Date: Period: #: TITRATION NOTES TITRATION NOTES I. Titration and Curves - Titration: lab technique in which one solution is used to analyze another (analyte/titrant) - point: point in a titration where just enough standard solution has

More information

Chapter 15 Acid-Base Equilibria

Chapter 15 Acid-Base Equilibria Chapter 15 Acid-Base Equilibria Acid-Base Equilibria 15.1 Solutions of Acids or Bases Containing a Common Ion A. Common Ion 1. Ion provided in solution by an aqueous acid (or base) as well as a salt a.

More information

I. Acids & Bases. A. General ideas:

I. Acids & Bases. A. General ideas: Acid-Base Equilibria 1. Application of equilibrium concepts. 2. Not much else new in the way of theory is presented. 3. Specific focus on aqueous (H O is 2 solvent) systems. 4. Assume we are at equilibrium

More information

Acid Base Equilibria

Acid Base Equilibria Acid Base Equilibria Acid Ionization, also known as acid dissociation, is the process in where an acid reacts with water to produce a hydrogen ion and the conjugate base ion. HC 2 H 3 O 2(aq) H + (aq)

More information

Analyte: The substance whose concentration is not known in a titration. Usually the analyte is in the flask or beaker beneath the burette.

Analyte: The substance whose concentration is not known in a titration. Usually the analyte is in the flask or beaker beneath the burette. Key Worksheet 15 Acids & Base Equilibria: Acid Base Titrations Objectives To be able to calculate the ph, poh, and concentrations of all species present at any point of an acid base titration. Vocabulary

More information

Titration a solution of known concentration, called a standard solution

Titration a solution of known concentration, called a standard solution Acid-Base Titrations Titration is a form of analysis in which we measure the volume of material of known concentration sufficient to react with the substance being analyzed. Titration a solution of known

More information

Lecture 8. Making a Buffer. Buffers. Professor Hicks Inorganic Chemistry (CHE152)

Lecture 8. Making a Buffer. Buffers. Professor Hicks Inorganic Chemistry (CHE152) Lecture 8 Professor Hicks Inorganic Chemistry (CHE152) Making a Buffer Buffers buffers = solutions that resist ph changes act by neutralizing added acid or base made by preparing a solution of a weak acid/base

More information

Chapter 17 Answers. Practice Examples [H3O ] 0.018M, 1a. HF = M. 1b. 30 drops. 2a.

Chapter 17 Answers. Practice Examples [H3O ] 0.018M, 1a. HF = M. 1b. 30 drops. 2a. Chapter 17 Answers Practice Examples 1a. + [HO ] 0.018M, 1b. 0 drops [HF] = 0.8 M. [H O + ] = 0.10 M, HF = 0.97 M. a. + HO 1.10 M, CHO = 0.150 M. b. 15g NaCHO a. The hydronium ion and the acetate ion react

More information

16.3 Weak Acids Weak Bases Titration

16.3 Weak Acids Weak Bases Titration 16.3 Weak Acids Weak Bases Titration Titration of Weak Acid with Strong Base Titration of Base Acid with Strong Acid Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Weak Acids Weak Bases Titration

More information

Consider a normal weak acid equilibrium: Which direction will the reaction shift if more A is added? What happens to the % ionization of HA?

Consider a normal weak acid equilibrium: Which direction will the reaction shift if more A is added? What happens to the % ionization of HA? ch16blank Page 1 Chapter 16: Aqueous ionic equilibrium Topics in this chapter: 1. Buffers 2. Titrations and ph curves 3. Solubility equilibria Buffersresist changes to the ph of a solution. Consider a

More information

CHAPTER 7 Acid Base Equilibria

CHAPTER 7 Acid Base Equilibria 1 CHAPTER 7 Acid Base Equilibria Learning Objectives Acid base theories Acid base equilibria in water Weak acids and bases Salts of weak acids and bases Buffers Logarithmic concentration diagrams 2 ACID

More information

Lecture #11-Buffers and Titrations The Common Ion Effect

Lecture #11-Buffers and Titrations The Common Ion Effect Lecture #11-Buffers and Titrations The Common Ion Effect The Common Ion Effect Shift in position of an equilibrium caused by the addition of an ion taking part in the reaction HA(aq) + H2O(l) A - (aq)

More information

Buffer solutions Strong acids and bases dissociate completely and change the ph of a solution drastically. Buffers are solutions that resist changes i

Buffer solutions Strong acids and bases dissociate completely and change the ph of a solution drastically. Buffers are solutions that resist changes i 18.3 ph Curves Buffer solutions Strong acids and bases dissociate completely and change the ph of a solution drastically. Buffers are solutions that resist changes in ph even when acids and bases are added

More information

ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA

ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while

More information

Review: Acid-Base Chemistry. Title

Review: Acid-Base Chemistry. Title Review: Acid-Base Chemistry Title Basics General properties of acids & bases Balance neutralization equations SA + SB water + salt Arrhenius vs. Bronsted-Lowry BL plays doubles tennis match with H+) Identify

More information

2] What is the difference between the end point and equivalence point for a monobasicmonoacid

2] What is the difference between the end point and equivalence point for a monobasicmonoacid 4 Titrations modified October 9, 2013 1] A solution of 0.100 M AgNO 3 is used to titrate a 100.00 ml solution of 0.100 M KCl. The K sp of AgCl is 1.8e-11 a) What is pag if 50.00 ml of the titrant is added

More information

ACID-BASE REACTIONS. Titrations Acid-Base Titrations

ACID-BASE REACTIONS. Titrations Acid-Base Titrations Page III-b-1 / Chapter Fourteen Part II Lecture Notes ACID-BASE REACTIONS Chapter (Part II A Weak Acid + Strong Base Titration Titrations In this technique a known concentration of base (or acid is slowly

More information

Chemistry 12. Bronsted Acids and Equilibria

Chemistry 12. Bronsted Acids and Equilibria Worksheet 42 Bronsted Acids and Equilibria Name Date Due Hand In With Corrections by Chemistry 12 Worksheet 42 Bronsted Acids and Equilibria 82 1. Write the formula for a proton 2. Write the formula for

More information

Acid and Base Titrations - Equation Guide

Acid and Base Titrations - Equation Guide Acid and Base Titrations - Equation Guide Strong Acid + Strong Base: Initial Region: ph = - log (n sa / V sa ) or ph = - log (C sa ) Pre-Equivalence Region: ph = - log sa # or ph = - log Equivalence: ph

More information

Acid-Base Titration Solution Key

Acid-Base Titration Solution Key Key CH3NH2(aq) H2O(l) CH3NH3 (aq) OH - (aq) Kb = 4.38 x 10-4 In aqueous solution of methylamine at 25 C, the hydroxide ion concentration is 1.50 x 10-3 M. In answering the following, assume that temperature

More information

School of Chemistry, University of KwaZulu-Natal, Howard College Campus, Durban. CHEM191 Tutorial 1: Buffers

School of Chemistry, University of KwaZulu-Natal, Howard College Campus, Durban. CHEM191 Tutorial 1: Buffers School of Chemistry, University of KwaZulu-Natal, Howard College Campus, Durban CHEM191 Tutorial 1: Buffers Preparing a Buffer 1. How many moles of NH 4 Cl must be added to 1.0 L of 0.05 M NH 3 to form

More information

Buffers. How can a solution neutralize both acids and bases? Beaker B: 100 ml of 1.00 M HCl. HCl (aq) + H 2 O H 3 O 1+ (aq) + Cl 1 (aq)

Buffers. How can a solution neutralize both acids and bases? Beaker B: 100 ml of 1.00 M HCl. HCl (aq) + H 2 O H 3 O 1+ (aq) + Cl 1 (aq) Buffers How can a solution neutralize both acids and bases? Why? Buffer solutions are a mixture of substances that have a fairly constant ph regardless of addition of acid or base. They are used in medicine,

More information

CHM 112 Dr. Kevin Moore

CHM 112 Dr. Kevin Moore CHM 112 Dr. Kevin Moore Reaction of an acid with a known concentration of base to determine the exact amount of the acid Requires that the equilibrium of the reaction be significantly to the right Determination

More information

Mixtures of Acids and Bases

Mixtures of Acids and Bases Mixtures of Acids and Bases CH202, lab 6 Goals : To calculate and measure the ph of pure acid and base solutions. To calculate and measure the ph of mixtures of acid and base solutions. Safety : Hydrochloric

More information

Lecture 12. Acid/base reactions. Equilibria in aqueous solutions.

Lecture 12. Acid/base reactions. Equilibria in aqueous solutions. Lecture 12 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added

More information

CA 47b Acid Base Titrations

CA 47b Acid Base Titrations CA 47b Acid Base Titrations Model 1 Titration of a strong acid with a strong base. 100. ml of 0.100 M HCl is titrated with 0.100 M NaOH; the species present in the aqueous solution at various volumes of

More information

Chapter 15. Acid-Base Equilibria

Chapter 15. Acid-Base Equilibria Chapter 15 Acid-Base Equilibria The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion already involved in the equilibrium

More information

Kotz 7 th ed. Section 18.3, pp

Kotz 7 th ed. Section 18.3, pp Lecture 15 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added

More information

CHEM 121b Exam 4 Spring 1999

CHEM 121b Exam 4 Spring 1999 Name SSN CHEM 121b Exam 4 Spring 1999 This exam consists of 10 multiple choice questions (each worth 2 points), and 6 written problems (points noted below). There are a total of 100 possible points. Carefully

More information

DATA SHEETS AND CALCULATIONS FOR ACIDS & BASES

DATA SHEETS AND CALCULATIONS FOR ACIDS & BASES Chemistry 112 Laboratory: Chemistry of Acids & Bases Page 73 DATA SHEETS AND CALCULATIONS FOR ACIDS & BASES Name Partner s Name Grade and Instructor Comments Part 1: Experimental Measurement Determining

More information

Advanced Placement Chemistry Chapters Syllabus

Advanced Placement Chemistry Chapters Syllabus As you work through the chapter, you should be able to: Advanced Placement Chemistry Chapters 14 16 Syllabus Chapter 14 Acids and Bases 1. Describe acid and bases using the Bronsted-Lowry, Arrhenius, and

More information

Applications of Aqueous Equilibrium Chapter 15. Common Ion Effect & Buffers Sections 1-3

Applications of Aqueous Equilibrium Chapter 15. Common Ion Effect & Buffers Sections 1-3 Applications of Aqueous Equilibrium Chapter 15 Common Ion Effect & Buffers Sections 1-3 Solutions of Acids or Bases Containing a Common Ion NaF Na + + F - HF H + + F - What effect does the NaF have on

More information

Chapter 16 Aqueous Ionic Equilibrium Buffer Solutions

Chapter 16 Aqueous Ionic Equilibrium Buffer Solutions Chapter 16 Aqueous Ionic Equilibrium 16.1-16.2 Buffer Solutions Why? While a weak acid will partially ionize to produce its conjugate base, it will not produce enough conjugate base to be considered a

More information

ACID-BASE EQUILIBRIA. Chapter 14 Big Idea Six

ACID-BASE EQUILIBRIA. Chapter 14 Big Idea Six ACID-BASE EQUILIBRIA Chapter 14 Big Idea Six Acid-Base Equilibria Common Ion Effect in Acids and Bases Buffer SoluDons for Controlling ph Buffer Capacity ph-titradon Curves Acid-Base TitraDon Indicators

More information

Problem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x

Problem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x Problem 1 What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10 5 )? Write out acid dissociation reaction: C 6 H 5 COOH C 6 H 5 COO H Make an ICE chart since this is a weak

More information

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

1. Know and be capable of applying the Bronsted-Lowery model of acids and bases (inculdig the concepts related to conjugate acid-base pairs.

1. Know and be capable of applying the Bronsted-Lowery model of acids and bases (inculdig the concepts related to conjugate acid-base pairs. Acid-Base Equilibria You have just completed a chapter on equilibrium. That chapter focused primarily on gas phase reactions (with a few exceptions). This section on Acid-Base equilibria (along with the

More information

Chapter 8 Acid-Base Equilibria

Chapter 8 Acid-Base Equilibria Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6

More information

Point: In an unbuffered, unprotected solution, a small addition of strong acid or base can cause a massive and dangerous shift in ph.

Point: In an unbuffered, unprotected solution, a small addition of strong acid or base can cause a massive and dangerous shift in ph. hem 210 Jasperse h 17 Handouts 1 h. 17 Additional Aqueous quilibria hapter 16 situations basically only involved one solute: strong or weak acid; strong or weak base; or ionic salt Real solutions often

More information

Mixtures of Acids and Bases

Mixtures of Acids and Bases Mixtures of Acids and Bases PURPOSE To investigate the resulting ph s of different mixtures of acid and base solutions. GOALS To calculate the ph of pure acid and base solutions. To calculate the ph of

More information

2. Calculate the ph of a buffer solution composed of 0.12 M benzoic acid and 0.20 M sodium benzoate.!

2. Calculate the ph of a buffer solution composed of 0.12 M benzoic acid and 0.20 M sodium benzoate.! AP Chem worksheet:buffers, The common ion effect Page 1 1. Calculate the ph of a buffer solution that is 0.060 M formic acid and 0.030 M potassium formate. (3.44) 2. Calculate the ph of a buffer solution

More information

AP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS

AP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS AP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS THE COMMON ION EFFECT The common ion effect occurs when the addition of an ion already present in the system causes the equilibrium to shift away

More information

ACID BASE EQUILIBRIUM

ACID BASE EQUILIBRIUM ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric

More information

A 95 g/mol B 102 /mol C 117 g/mol D 126 g/mol E 152 g/mol

A 95 g/mol B 102 /mol C 117 g/mol D 126 g/mol E 152 g/mol Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical reaction between the two solutions is complete.

More information

CHEM 142 Exam 3 Study Guide Chapter 15: Acid-Base Equilibria

CHEM 142 Exam 3 Study Guide Chapter 15: Acid-Base Equilibria CHEM 142 Exam 3 Study Guide Chapter 15: AcidBase Equilibria A. Terminologies and Concepts 1. BronstedLowry definitions acids vs. bases; give examples 2. Amphoteric substances define and give examples 3.

More information

CHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA. For Review

CHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA. For Review CHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA For Review 1. A common ion is an ion that appears in an equilibrium reaction but came from a source other than that reaction. Addition of a common ion

More information

1.12 Acid Base Equilibria

1.12 Acid Base Equilibria .2 Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can

More information

Acid-Base Titrations. Terms. Terms. Terms

Acid-Base Titrations. Terms. Terms. Terms Isoionic Point: The ph of pure, neutral polyprotic acid (the natural zwitterion) HAwater: H A +, A -, H +, and OH - Most HA and [H A + ][A - ] Isoelectric Point: ph at which the average charge of the polyprotic

More information

The ph of aqueous salt solutions

The ph of aqueous salt solutions The ph of aqueous salt solutions Sometimes (most times), the salt of an acid-base neutralization reaction can influence the acid/base properties of water. NaCl dissolved in water: ph = 7 NaC 2 H 3 O 2

More information

Chapter 15 Acid Base Equilibria

Chapter 15 Acid Base Equilibria Buffer Solutions The ph changes by a large amount even when a small amount of acid or base is added to pure water: Chapter 15 Acid Base Equilibria A buffer solution is a solution which resists a change

More information

Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria

Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly

More information

Operational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA

Operational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution

More information

1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O.

1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O. 1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H O. HCN + H O º H O + + CN ) Write the Brønsted-Lowry reaction for weak base NH reacting with H O NH + H O º OH + NH + ) Using the

More information

Chapter 14. Principles of Neutralization Titrations

Chapter 14. Principles of Neutralization Titrations Chapter 14 Principles of Neutralization Titrations Neutralization titrations are widely used to determine the amounts of acids and bases and to monitor the progress of reactions that produce or consume

More information

Chapter 14 Acid- Base Equilibria Study Guide

Chapter 14 Acid- Base Equilibria Study Guide Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and

More information

Acid-Base Solutions - Applications

Acid-Base Solutions - Applications Acid-Base Solutions - Applications 1 The Common Ion Effect Consider the equilibrium established when acetic acid, HC 2 H 3 O 2, is added to water. CH 3 COOH(aq) + H 2 O(l) CH 3 COO - (aq) + H 3 O + (aq)

More information

Chapter 8 Acid-Base Equilibria

Chapter 8 Acid-Base Equilibria Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6

More information

1.8K: Define a buffer as relatively large amounts of a weak acid or base and its conjugate in equilibrium that maintain a relatively constant ph when

1.8K: Define a buffer as relatively large amounts of a weak acid or base and its conjugate in equilibrium that maintain a relatively constant ph when 1.8K: Define a buffer as relatively large amounts of a weak acid or base and its conjugate in equilibrium that maintain a relatively constant ph when small amounts of acid or base are added. 1 Chem 20

More information

Homework #7 Chapter 8 Applications of Aqueous Equilibrium

Homework #7 Chapter 8 Applications of Aqueous Equilibrium Homework #7 Chapter 8 Applications of Aqueous Equilibrium 15. solution: A solution that resists change in ph when a small amount of acid or base is added. solutions contain a weak acid and its conjugate

More information

1. What do a chemical indicator and a buffer solution typically both contain?

1. What do a chemical indicator and a buffer solution typically both contain? Acids, Bases & Redox 2 - Practice Problems for Assignment 9 1. What do a chemical indicator and a buffer solution typically both contain? (a) A strong acid and its conjugate acid (b) A strong acid and

More information

Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107

Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Chapter 15 Applications of Aqueous Equilibria (mainly acid/base & solubility)

More information

PERIODIC TABLE OF THE ELEMENTS

PERIODIC TABLE OF THE ELEMENTS Chem 114 Exam 3 April 4, 2016 Name: PLEASE print your name on the exam and sign the academic integrity pledge. Print your name and fill in the circles with your I.D. # on side 1 (blue) of the scantron.

More information

Unit The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60

Unit The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60 Unit 2 1- The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60 2- How many grams of Na 2 CO 3 (mw = 106 ) A) 318 B) 0.028 C) 134 D) 201 E) 67 in 3 moles, 3- Calculate the normal

More information

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions?

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions? JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 3 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a

More information

Chapter 15, Applications of Aqueous Equilibria

Chapter 15, Applications of Aqueous Equilibria Chapter 15, Applications of Aqueous Equilibria We will focus on 3 areas: 1) titrations 2) buffers (incl. the Henderson- Hasselbalch Transformation), 3) solubility equilibria. 1 I. Neutralization Reactions

More information

5/10/2017. Chapter 10. Acids, Bases, and Salts

5/10/2017. Chapter 10. Acids, Bases, and Salts Chapter 10. Acids, Bases, and Salts Introduction to Inorganic Chemistry Instructor Dr. Upali Siriwardane (Ph.D. Ohio State) E-mail: upali@latech.edu Office: 311 Carson Taylor Hall ; Phone: 318-257-4941;

More information

4. Acid Base Equilibria

4. Acid Base Equilibria 4. Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can

More information

CHEMISTRY Matter and Change

CHEMISTRY Matter and Change CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen

More information

= ) = )

= ) = ) Basics of calculating ph 1. Find the ph of 0.07 M HCl. 2. Find the ph of 0.2 M propanoic acid (K a = 10-4.87 ) 3. Find the ph of 0.4 M (CH 3 ) 3 N (K b = 10-4.20 ) 4. Find the ph of 0.3 M CH 3 COO - Na

More information

Name AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria

Name AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria Name AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria Solutions of Acids or Bases Containing a Common Ion A common ion often refers to an ion that is added by two or more species. For

More information

Acid-Base Equilibria. And the beat goes on Buffer solutions Titrations

Acid-Base Equilibria. And the beat goes on Buffer solutions Titrations Acid-Base Equilibria And the beat goes on Buffer solutions Titrations 1 Common Ion Effect The shift in equilibrium due to addition of a compound having an ion in common with the dissolved substance. 2

More information

Chapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1

Chapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1 Chapter 16 Acids and Bases Copyright Cengage Learning. All rights reserved 1 Section 16.1 Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH ions.

More information

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin)

ph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 2 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a

More information

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion. Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when

More information

Chem 321 Lecture 10 - Acid-Base Equilibria (Review) 10/1/13

Chem 321 Lecture 10 - Acid-Base Equilibria (Review) 10/1/13 Chem 321 Lecture 10 AcidBase Equilibria (Review) 10/1/13 Student Learning Objectives In any aqueous solution at equilibrium, the water selfionization reaction is also at equilibrium. That is, and K w H2

More information

APPLICATIONS OF AQUEOUS EQUILIBRIA REACTIONS AND EQUILIBRIA INVOLVING ACIDS, BASES, AND SALTS

APPLICATIONS OF AQUEOUS EQUILIBRIA REACTIONS AND EQUILIBRIA INVOLVING ACIDS, BASES, AND SALTS APPLICATIONS OF AQUEOUS EQUILIBRIA REACTIONS AND EQUILIBRIA INVOLVING ACIDS, BASES, AND SALTS COMMON IONS Common ion effect- The addition of an ion already present(common) in a system causes equilibrium

More information

Strong Acids and Bases C020

Strong Acids and Bases C020 Strong Acids and Bases C020 Strong Acids and Bases 1 Before discussing acids and bases examine the concept of chemical equilibrium At reaction is at equilibrium when it is proceeding forward and backwards

More information

Ch 15, Applications of Aq Equilibria

Ch 15, Applications of Aq Equilibria Ch 15, Applications of Aq Equilibria We will focus on 3 areas: 1) buffers (incl. Henderson-Hasselbalch Transformation) 2) titrations 3) solubility equilibria 1 I. Neutralization Reactions A. Strong acid-strong

More information

Unit Nine Notes N C U9

Unit Nine Notes N C U9 Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release

More information

-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form

-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form NOTES Acids, Bases & Salts Arrhenius Theory of Acids & Bases: an acid contains hydrogen and ionizes in solutions to produce H+ ions: a base contains an OH group and ionizes in solutions to produce OH ions:

More information

12. Acid Base Equilibria

12. Acid Base Equilibria 2. Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can

More information

Duncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES

Duncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) 1. hydro- - HF 2. root of

More information

Quiz name: Equilibria + Acids/Bases

Quiz name: Equilibria + Acids/Bases Name: Quiz name: Equilibria + Acids/Bases Date: 1. 2. At 450 C, 2.0 moles each of H 2(g), I 2(g), and HI are combined in a 1.0 L rigid container. The value of K c at 450 C is 50. Which of the following

More information

Chem Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation

Chem Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation Chem 106 3--011 Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation 3//011 1 The net ionic equation for the reaction of KOH(aq) and

More information

Acids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017

Acids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017 Acids, Bases and ph Preliminary Course Steffi Thomas ssthomas@tcd.ie 14/09/2017 Outline What are acids and bases? Can we provide a general definition of acid and base? How can we quantify acidity and basicity?

More information

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any

More information