Quiz 1. What is the equilibrium pH of a 0.175 M solution of the diprotic 1,5-pentanedioic acid? pKa1 = 4.345 and pKa2 = 5.422. Show your work. a. 11.4 b.

Slides:

Advertisements

Similar presentations

LAB 11 Determination of Buffer Capacity. Outline Purpose Buffers Buffer Example Equilibrium Expression and the Henderson-Hasselbalch Equation Things to.

Advertisements

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

Common Ion Effect Revisited. pH changes due to Common Ion Effect.

Acids ph buffers A2 chemistry. Using the post it notes write down the name of the species and whether each species round the room is an acid, base or.

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

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

Chapter 11 Polyprotic Acid and Bases. 2 Diprotic Acids Compounds with two acid/base groups Can be two acids groups Oxalic Acid Can be two basic groups.

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.

Slide 1 of 52  Worked Examples Follows:. Slide 2 of 52.

The Relationship between K a and K b : For the ionization of the weak acid HA ; HA + H 2 O ↔ H 3 O + + A -, K a = [H 3 O + ] [A - ] [HA] For the ionization.

Buffer calculations g of propanoic acid is dissolved in water and mixed with 25.0 mL of mol L –1 NaOH. The final solution is made up to

Henderson – hasselbalch equation

Lecture 1: Introduction and review –Quiz 1 –Website: –Review of acid/base chemistry –Universal features of.

Acids ph buffers A2 chemistry. Using the post it notes write down the name of the species and whether each species round the room is an acid, base or.

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

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

Buffers. What Are They? Solutions that resist changes in pH with addition of small amounts of acid or base Require two species: an acid to react with.

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.

Common Ion Effect Buffers.

 Take out your purple sheet, 17.2 worksheet, and problem set 1  Questions on 17.2 worksheet?  Questions on problem set 1?

QUIZ ON CH. 14 AND 15. 1) What does pH measure? What are the terms for a liquid with a pH of 3, a pH of 7, and a pH 10? pH measures [H+] concentration.

Common Ion Effect Buffers. Common Ion Effect Sometimes the equilibrium solutions have 2 ions in common For example if I mixed HF & NaF The main reaction.

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

Using the ICE method for neutralisation Mols Propanoic acid Mols NaOHMols Propanoate Initial (I) x10 -3 x.108 = Change (C)

Acid/base chemistry Buffers Henderson-Hasselbalch equation.

Buffered Solutions What is a buffer? Calculations involving Buffers.

16.2 Buffers: Solutions That Resist pH Change

Buffers and Henderson-Hasselbach Equation

Aqueous Equilibria Chapter 15

Acids and Bases Bundle 4: Water.

Aqueous Equilibria Chapter 15

Weak Acid – Strong Base Titration

Buffer Capacity BCH 312 [PRACTICAL].

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

Applications of Aqueous Equilibria

CHAPTER 2 Water, pH, and Ionic Equilibria to accompany

PH and Buffers.

Acids and Bases Bundle 4: Water.

Acids and Bases Bundle 4: Water.

Chapter 17 Acid-Base Titrations.

Chapter 9 Monoprotic Acid-Base Equilibria

Experiment 7 Preparation and Properties of Buffers

Buffered Solutions - A solution that can resist a change in pH when an acid, H+, or base, OH-, is added.

Types of Acid Base Equilibrium Problems

Calculate the pH of a solution that is 0

Chem. 31 – 12/6 Lecture.

Week 5. Buffers solutions

Salts neutralization reactions acids bases strong acid+ strong 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

Buffers and Acid/Base Titration

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

Titration Basics Titration = addition of a measurable volume of a known solution (titrant) to an unknown solution until it is just consumed Use the stoichiometry.

Chapter 15 Acid-Base Equilibria.

Titration curve Typical ph titration of a weak monoprotic acid vs strong base.

Indicators are weak acids that change color when they become bases.

Acids Lesson 9 Weak Acids pH Calculations.

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

Calculating pH (and pOH)

Buffers and Henderson-Hasselbalch

Common Ion Effect Buffers.

Titration of a weak acid with strong base

A Different Look At Buffers

Solving weak acid equilibrium problems:

Buffers in a Nutshell pp

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.

Special Conditions for Buffers

Buffers and titrations

Presentation transcript:

Quiz 1. What is the equilibrium pH of a 0.175 M solution of the diprotic 1,5-pentanedioic acid? pKa1 = 4.345 and pKa2 = 5.422. Show your work. a. 11.4 b. 2.6 c. 3.6 d. 2.81 x 10-3 2. From problem 1 above, what is the equilibrium concentration of the base form of 1,5-pentanedioic acid? a. 2.8 x 10-3 M b. 0.175 M c. 4.7 x 10-11 M d. 3.8 x 10-6

Quiz 3. Consider a buffer solution made from the weak base A2- with pKa1 = 4.5 and pKa2 = 9.0. In a buffer solution with pH = 8.7, which Henderson-Hasselbalch equation should be used for calculations? a. b. c. d. 4. Consider a buffer where the [HA] + [A-] = 0.250 M and [A-] / [HA] = 2.00. What is [HA]? Show your work. a. 0.125 M b. 8.33 x 10-2 M c. 0.167 M d. none of these