Quiz 1. A solution of H3PO4 and its associated forms has a pH of 7.50. What is the principal species? For H3PO4, pKa1 = 2.148, pKa2 = 7.199, pKa3 =

Slides:

Advertisements

Similar presentations

Outline:3/9/07 è Chem. Dept. Seminar 4pm è 3 more lectures until Exam 2… è Chemistry Advising – 4pm Today: è More Chapter 18 Titrations.

Advertisements

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

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

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

Acid-Base Equilibria pH and pOH Relationship of Conjugate Pair acid-base strength. When acids or bases control pH:  determine K  predict pH When pH controls.

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.

Titrations. Strong Acid with Strong Base Starting pH pH = -log[F Acid ] Just before the Equivalence Point [H + ] = (V acid ·F acid -V base ·F base )/(V.

Lecture 23 10/28/ mL of 0.02 M KOH with 0.1 M HBr Construct curve from 4 points Initial pH X = 0 mL, Y = ? Equivalence point X = V eq, Y = 7 Before.

Acids & Bases Lesson 13 Weak Base/Strong Acid calculations.

Acid-Base Titrations.

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.

Which is the stronger acid? 1.HNO 2 2.HNO 3 Which is the stronger base? 1.NO NO 3 -

Chap. 2. Problem 2a. pH = - log [H + ] pH = - log (1.75 x ) pH = - (-4.76) pH = 4.76.

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

Titration Calculations Weak Acid and Strong Base.

Chem. 31 – 4/29 Lecture. Announcements Last collected homework (3.1) due today Last quiz today Today’s Lecture –Chapter 9: Polyprotic Acids Dissolution.

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

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)

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

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.

See summary: top of p.778 in textbook

Chapter 15 Applying equilibrium. Titration Curves.

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 Titration Problems West Valley High School General Chemistry Mr. Mata.

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

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.

Indicators And Titration. Indicators Usually organic acid or base whose color is sensitive to pH Indicator is weak acid or base In basic solution, indicator.

Titrations an Example Titration of sodium carbonate with hydrochloric acid Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1.

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.

Titration & pH curves [17.3].

Acid-Base Titrations End point and equivalence point

Titration and pH Curves.

Titration and pH Curves.

Question (Clickers) Which of the following does not belong: Acids...

Acids & Bases Titration.

Acids and Bases.

Principles & Modern Applications

Titration & pH curves [17.3].

Q Neutralization Curves: Potentiometric Methods

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

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

Chapter 17 Acid-Base Titrations.

Quiz 1. What is the equilibrium pH of a M solution of the diprotic 1,5-pentanedioic acid? pKa1 = and pKa2 = Show your work. a b.

Titration Stations.

SAMPLE EXERCISE 17.6 Calculating pH for a Strong Acid–Strong Base Titration Calculate the pH when the following quantities of M NaOH solution have.

Lesson 3 LT: I can model a neutralization reaction and use titration to determine the concentration of an acid or a base.

Salts neutralization reactions acids bases strong acid+ strong base

Quiz 1. What is the pH of a 5.0 x 10-6 M solution of CsOH? A. 5.3

Titrations & Buffer solutions

Titrations pH Titrant volume, mL

Ch 16: pH of Mixtures In the last chapter, we looked at pH of mixtures of only acids or only bases. This chapter looks at other types of mixtures A or.

PREPARATION OF BUFFERS

Sit where you want. Every group will need a dry erase board, marker, & napkin. Every person in your group will need a calculator and paper. Take everything.

Equivalence Point.

Acid Base Review Station Activity

Schedule Today (3/4): Continue Chapter 8

Schedule Today (3/1): Continue Chapter 8

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

Titration and Acid-Base Neutralization

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:

17.3 Acid-Base Titrations.

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

Acid-Base Reactions: TITRATION

Special Conditions for Buffers

Presentation transcript:

Quiz 1. A solution of H3PO4 and its associated forms has a pH of 7.50. What is the principal species? For H3PO4, pKa1 = 2.148, pKa2 = 7.199, pKa3 = 12.15. Show how you came to your answer using equilibrium reactions. a. H3PO4 b. H2PO4- c. HPO42- d. PO43- 2. In problem 1 above, what is the second most abundant species?

Quiz 3. How many mL of 0.250 M HCl need to be added to 20.0 mL of 0.350 M acetate to reach the equivalence point? Show your work. a. 14.0 mL b. 20.0 mL c. 28.0 mL d. none of the above 4. Consider the titration of a weak acid whose pKa is 7.7. What is the pH of the titration half way to the equivalence point? a. 7.7 b. 6.3 c. 7.0 d. more information is necessary