Acid – Base Titrations.

Slides:

Advertisements

Similar presentations

Titrations and Indicators IB Chemistry Power Points Topic 18 Acids and Bases

Advertisements

Neutralization Reactions Reaction that occurs between an acid and a base. Example: HCl + NaOH  NaCl + H 2 O & Water Products always include: A “Salt”

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.

Slide 1 of Acid-Base Indicators  Color of some substances depends on the pH. HIn + H 2 O In - + H 3 O + In the acid form the color appears to.

8.7 Acid-Base Titration Learning Goals … … determine the pH of the solution formed in a neutralization reaction.

Lecture 203/13/06. Titration Why use? Equivalence point vs. Endpoint Math?

Lecture 193/14/05 Spring Break Quiz Seminar today.

Lecture 172/28/07 LECTURE TONIGHT. Titration Curve Why do you use one? Equivalence point vs. Endpoint pH vs. acid/base added.

Lecture 213/15/06 Environmental Club Meeting  Today at 5:30  Laska classroom 317.

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

Burette clamp ring stand burette erlenmeyer flask Titration.

Acid/Base Indicators Substance that changes color in the presence of an acid or a base – Red or Blue Litmus – Phenolphthalein (phth) – Bromothymol blue.

Basic acid/base titrations. Types of acid base titration There are four different types of acid/base titrations; 1) Strong acid with strong base. 2) Strong.

Procedure for calculating pH of a titration Volume of titrant needed is based on amount of analyte.

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

PH and Titration Notes Chemistry. pH  measure of the strength of acids and bases  pH = power of hydrogen  pH = -log [H + ]  logarithmic scale – so.

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

Choosing an Appropriate Indicator. Not every acid-base indicator is appropriate for signaling the neutralization point of a reaction. Table M Common Acid-Base.

Chapter 16 More Work with Acids and Bases pH Self-Ionization of Water: 2H 2 O H 3 O + + OH - -Occurs in 2 per 1 billion molecules in PURE (deionized.

PROBLEM: You titrate 25.0 mL of 0.10 M NH 3 with 0.10 M HCl. (a) What is the pH of NH 3 solution before the titration begins? (b) What is the pH at the.

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:

(equimolar amounts of acid and base have reacted)

Chapter 15(a) Applications of Aqueous Equilibria.

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

REACH will present significant challenges to all of us

Acids and Bases pH, Titration, and Indicators. pH VIII. pH (power of hydrogen or hydronium) - measurement of hydronium concentration A. pH = -log [H 3.

PH. Aim: How is the pH of a solution determined? Objectives: 1.Students should be able to identify if a substance is an acid, a base or neutral when provided.

Ionisation of water and pH For any Bronsted conjugate Acid-Base pair pH concept pH = -log[H + ] pX = -logX pH scale [H + ] > M, pH < 7 ACIDIC [H.

Acid-Base Titration and pH. Self-Ionization of Water H 2 O + H 2 O  H 3 O + + OH - Though pure water is considered a non-conductor, there is a slight,

Acid-Base Indicators The most common acid-base indicators are complex molecules that are themselves weak acids (represented by HIn). They exhibit one color.

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

Applications of Acid-Base Equilibria

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.

bjects/3312/ /blb1703.html.

Titration Curves I. Strong Acid + Strong Base 0.1 M HCl 0.1 M NaOH

Acid-Base Titrations.

pH CURVES & INDICATORS Richard Grime – Ripon Grammar School

Loose Ends from Bell Work An acidic solution makes the color of pH paper turn ___________________, while a basic solution makes the color of pH paper turn.

NEUTRALIZATION, INDICATORS, AND TITRATIONS. NEUTRALIZATION REACTIONS So far we have only looked at acid and base reactions with water Ka and Kb reactions.

Yesterday’s Homework Page 611 # 19 Page 612 # 20.

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

Titrations Chapter 13.

Acids and Bases Applied Chemistry. Acids  Definition: A substance that produces hydrogen ions (H + or H +1 ) in water.  General reaction in water: HA.

Acid-Base Reactions. Neutralization acid + base salt + water HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O (l) H + + Cl - + Na + + OH - Na + + Cl - + H 2 O (l)

Acid-Base Reactions. Neutralization acid + base salt + water HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O H + + Cl - + Na + + OH - Na + + Cl - + H 2 O H + +

Chapter 16 More Work with Acids and Bases pH Self-Ionization of Water: 2H 2 O H 3 O + + OH - -Occurs in 2 per 1 billion molecules in PURE (deionized.

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

Titration & pH curves [17.3].

Acid-Base Titrations End point and equivalence point

Titration and pH Curves.

strong acid strong base

Titration & pH curves [17.3].

Review of Diprotic Acid Titration

Wake-up Strong acids completely ionize in water. Explain what this means. Name the following acids/bases: a. HNO2 b. Hydrosulfuric acid c. Be(OH)2.

(Acid/Base neutralization)

Equivalence point - point at which the titrant and the analyte are present in stoichometrically equivalent amounts.

pH, Titration, and Indicators

NH4+ (aq) H+ (aq) + NH3 (aq)

ACIDS AND BASES.

PRACTICAL (2) Acid – based Equilibrium

Titrations & Buffer solutions

Warm-Up Do not turn in pH practice!

Acids Lesson 20 Titration Curves.

Chapter 4.8 Review Acid-Base Reactions.

Unit 14 – Acid, Bases, & Salts

Determining the pH and Titrations

Titration Curves I. Strong Acid + Strong Base 0.1 M HCl 0.1 M NaOH

Presentation transcript:

Acid – Base Titrations

Titration of HCl with NaOH

0.00 mL Titrant Added Titration Reaction H+ OH- H2O end = 0.1000 M = 0 M lots Equilibrium Reaction H2O H+ OH- Initial lots 0.1000 0 Change - x + x + x Equilibrium lots ~0.1000 x [H+] = 0.1000 M Concentration pH = - log(0.1000) = 1.00

25.00 mL Titrant Added (Equivalence Point) Titration Reaction H+ OH- H2O start (0.1000M)(0.02500L) (0.1000M)(0.02500L) = 0.002500 mol = 0.002500 mol = 0 mol end 0 mol 0 mol lots = 0 M = 0 M lots Equilibrium Reaction H2O H+ OH- Initial lots 0 0 Change - x + x + x Equilibrium lots x x 10-14 = x2 x = [H+] = 10-7 M Concentration pH = - log(10-7) = 7.00

50.00 mL Titrant Added Titration Reaction H+ OH- H2O start (0.1000M)(0.02500L) (0.1000M)(0.05000L) = 0.002500 mol = 0.005000 mol = 0 mol end 0 mol 0.002500 mol 0.002500 mol 0.002500mol/0.07500L = 0 M = 0.03333 M lots Equilibrium Reaction H2O H+ OH- Initial lots 0 0.03333 Change - x + x + x Equilibrium lots x ~0.03333 [OH-] = 0.03333 M Concentration pOH = - log(0.03333) = 1.50 or pH = 14 - 1.50 = 12.50

Concentration Effects 0.1 M HCl titrated with 0.1 M NaOH 0.001 M HCl titrated with 0.001 M NaOH Methyl Red Indicator Thymol Blue Indicator Phenolphthalein Indicator

Strong Acid vs. Strong Base Titration

Titration of HAc with NaOH

0.00 mL Titrant Added Titration Reaction HAc OH- Ac- H2O end = 0.1000 M = 0 M = 0M lots Equilibrium Reaction HAc H+ Ac- Initial 0.1000 0 0 Change - x + x + x Equilibrium ~0.10000 x x 1.75 x 10-5 = x2 / 0.1000 x = [H+] = 0.00132 M Concentration pH = - log(0.00132) = 2.88

12.50 mL Titrant Added Titration Reaction HAc OH- Ac- H2O start (0.1000M)(0.02500L) (0.1000M)(0.01250L) = 0.002500 mol = 0.001250 mol 0 0 end 0.001250 mol 0 mol 0.001250 0.00125 0.001250mol/0.03750L = 0.03333 M = 0 M = 0.03333 M lots Equilibrium Reaction HAc H+ Ac- Initial 0.03333 0 0.03333 pH = 4.76 + log(0.03333/0.03333) = 4.76 Concentration pH = 4.76

25.00 mL Titrant Added Titration Reaction HAc OH- Ac- H2O start (0.1000M)(0.02500L) (0.1000M)(0.02500L) = 0.002500 mol = 0.002500 mol 0 0 end 0 mol 0 mol 0.002500 0.002500 0.002500/0.05000 = 0 M = 0 M = 0.05000 lots Equilibrium Reaction Ac- H2O HAc OH- Initial 0.05000 lots 0 0 Change - x - x + x + x Equilibrium ~0.05000 lots x x Kb = 10-14 / (1.75 x 10-5) = 5.71 x 10-10 = x2 / 0.05000 x = [OH-] = 5.34 x 10-6 M Concentration pOH = - log(5.34 x 10-6) = 5.27 or pH = 14 - 5.27 = 8.73

50.00 mL Titrant Added Titration Reaction HAc OH- Ac- H2O start (0.1000M)(0.02500L) (0.1000M)(0.05000L) = 0.002500 mol = 0.005000 mol 0 0 end 0 mol 0.002500 mol 0.002500 0.002500 mol 0.002500mol/0.07500L = 0 M = 0.03333 M = 0.03333 M lots Equilibrium Reaction Ac- H2O HAc OH- Initial 0.03333 lots 0 0.03333 Change - x - x + x + x Equilibrium ~0.03333 lots x ~0.03333 [OH-] = 0.03333 M Concentration pOH = - log(0.03333) = 1.48 or pH = 14 - 1.48 = 12.52

Methyl Red Thymol Blue Phenolphthalein

Effect of Concentration and Strength

Weak Acid vs. Weak Base Titration

Acid-Base Indicators Phenolphthalein Basic Form = Pink Acidic Form = Colorless

Bromothymol Blue

0.1 M HAc titrated with 0.1 M NaOH Methyl Red Indicator Phenolphthalein Indicator