Stuff. Make-up Exam tomorrow night, Date: Tuesday Feb 17. Room: C-109 Time: 6-8 (1.5 hr) Problems for Acid-Bases posted. Hour Exam Solutions posted
|
|
- Grant Atkins
- 6 years ago
- Views:
Transcription
1 Stuff Make-up Exam tomorrow night, Date: Tuesday Feb 17. Room: C-109 Time: 6-8 (1.5 hr) Problems for Acid-Bases posted. Hour Exam Solutions posted Lecture slides up to date Can I ask the girls to what high school you attended. Thank you!
2 Kw is an equilibrium constant that describes the autoionization of water. H 2 O(l) H + (aq) + OH (aq) K w = [H + ][OH - ] H 2 O(l) + H 2 O(l) H 3 O + (aq) + OH (aq) Base Acid Acid Base K w = [H 3 O + ][OH - ] When we measure equilibrium concentrations of OH and H + we find that: K w = [H3O + ][OH - ] = 1 X Called the Ion-Product of Water
3 ph is the human defined logarithmic scale for measuring acidity. It is directly related to [H + ] concentration in an aqueous solution. ph = -log [H + ] = -log [H3O + ] logarithmic form p = -log [H + ] = 10 -ph exponential form ---Each ph unit or number represents a power of 10 (or an order of magnitude as it is called). A solution with a ph of 4 is 10X more than one with ph=3, 100X more than ph=2 and 1000X more than ph = 1.
4 Acidic, basic and neutral solutions are identified by their ph values [H3O + ] ph [OH - ] ph = -log [H3O + ] K w = [H3O + ][OH - ] = The ion-product of water is a constant!
5 ph is measured with dyed paper or with a commercial instrument. ph meter ph (indicator) paper
6 Known dye indicators change color within narrow ph limits.
7 Kw is related to ph via logarithm. K W = [H 3 O + ][OH - ]= 1.0 X take -log of both sides -log Kw = -log ([H 3 O + ][OH - ]) = -log(1.0 X ) -log K W = - log[h 3 O + ] + -log[oh - ] = -log (10-14 ) pk W = ph + poh = -(-14) pk W = ph + poh = 14 K W = [H 3 O + ][OH - ] = Connect The Dots: Kw---pH---pOH
8 [H3O + ] ph [OH - ] poh Relation ships between [H 3 O + ], ph, [OH - ] and poh
9 A Logarithm is Just An Exponent Let y be any number. Also, let b be a number and let s call it the base, b. Lastly let s call the power we raise the base to an exponent and label it as x y = b x 100 = 10 x b = base, x = exponent and y = a number b = 10 and y =100 and x = exponent The logarithm of 100 {log (100)} is the value of the exponent, x, needed to raise 10 to in order to obtain 100. log (100) = x = 2 The logarithm of 100 is value of the exponent required in the equation above!
10 Logs are easy if you see the riff. What is the log10 of the following numbers? 1000, 100, 10, 1, 0, 0.1, 0.01, log = log 1000 = x log = log 100 = x log 10 = x log 1 = x log 0 = x log 0.1 = x log 0.01 = x Determining the log 10 is the same as computing x in this equation! means 10 X = X = X = X = 1 10 X = 0 10 X = X = 0.01
11 In math we use two common logarithm functions. Log to the base 10 and the natural log. log = log 10 log to the base 10 log e = log = ln the natural log Properties of Logs log (A B) = log A + log B ( ) A log = log A log B B log A n = n log A antilog(log x) = 10 log x = x
12 Antilog of a number means use the number as an exponent. Sometimes we know the base and the exponent, but we need to compute the number. We can write it like this: log (?) = 2 In words we would say: The log10 of what number is equal to 2? Finding this number is called taking the antilogarithm Antilog [log (?)] = Antilog (2)? = 10 2 = 100 The antilog 10 is the same as the base 10 operator!
13 Log and Exponential Forms Logarithmic Form ph = -log [H 3 O + ] Exponential Form 10 -ph = [H 3 O + ] poh = -log [OH - ] 10 -poh = [OH - ] pk a = -log K a 10 -pka = pk a When H 3 O +, OH -, K a are large values----the pk s are small values. Strong acids have large H 3 O and K a therefore small ph and small pk a
14 The ph of rainwater collected in a certain region of the northeastern United States on a particular day was What is the H + ion concentration of the rainwater? The OH - ion concentration of a blood sample is 2.5 x 10-7 M. What is the ph of the blood?
15 The ph of rainwater collected in a certain region of the northeastern United States on a particular day was What is the H + ion concentration of the rainwater? ph = -log [H + ] antilog(-ph) = antilog (log [H + ]) [H + ] = 10 -ph = = 1.5 x 10-5 M The OH - ion concentration of a blood sample is 2.5 x 10-7 M. What is the ph of the blood? ph + poh = poh = -log [OH - ] = -log (2.5 x 10-7 ) = 6.60 ph = poh = = 7.40
16 Problem: Calculating [H 3 O + ], ph, [OH - ], and poh In a restoration project, a conservator prepares copperplate etching solutions by diluting concentrated nitric acid, HNO 3, to 2.0 M, 0.30 M, and M HNO 3. Calculate [H 3 O + ], ph, [OH - ], and poh of the three solutions at 25 o C. PLAN: HNO 3 is a strong acid so [H 3 O + ] = [HNO 3 ]. Use K w to find the [OH - ] and then convert to ph and poh.
17 In a restoration project, a conservator prepares copperplate etching solutions by diluting concentrated nitric acid, HNO 3, to 2.0 M, 0.30 M, and M HNO 3. Calculate [H 3 O + ], ph, [OH - ], and poh of the three solutions at 25 o C. For 2.0 M HNO 3, [H 3 O + ] = 2.0 M, and ph = -log [H 3 O + ] = = ph [OH - ] = K w / [H 3 O + ] = 1.0 x /2.0 = 5.0 x M; poh = For 0.3 M HNO 3, [H 3 O + ] = 0.30 M and -log [H 3 O + ] = 0.52 = ph [OH - ] = K w /[H 3 O + ] = 1.0 x /0.30 = 3.3 x M; poh = For M HNO 3, [H 3 O + ] = M and -log [H 3 O + ] = 2.20 = ph [OH - ] = K w / [H 3 O + ] = 1.0 x /6.3 x 10-3 = 1.6 x M; poh = 11.80
18 Equilibrium Problems Strong Acids/Bases Weak Acid/Bases 100% dissociation of [HA] % ionization varies with concentration of acid. [H 3 O + ] = [HA]. No need for ICE table. [H 3 O + ] = [HA]. ICE Table Is Needed 1. Simplification If 100 x Ka < [A]0 then [HA] - x = [HA] 2. Perfect square 3. Quadratic equation
19 Know your strong acids and bases and you will recognize the problem hydrohalic acids perchloric nitric sulfuric Group I hydroxides Group II hydroxides
20 Acid-Bases Equilibrium Problems HCl(aq) + H 2 O H 3 O + (aq) + Cl (aq) 0.004% at equilibrium % at equilibrium STRONG ACID CH 3 CO 2 H(aq) + H 2 O H 3 O + (aq) + CH 3 CO 2 (aq) 98.7% at equilibrium 1.3% at equilibrium WEAK ACID
First Exam December 19---Christmas Break begins December 21. Silberberg Chapter 17-18, Skoog 2-7, 11-13
Announcements First Exam December 19---Christmas Break begins December 21. Silberberg Chapter 17-18, Skoog 2-7, 11-13 Please keep up with the work (lots of problems in this Chapter) and see me if you have
More informationChemistry 132 NT. Acids and Bases
Chemistry 132 NT It is the mark of an instructed mind to rest satisfied with the degree of precision that the nature of a subject permits, and not to seek exactness where only an approximation of the truth
More informationIntroduction to Acids & Bases II. Packet #26
Introduction to Acids & Bases II Packet #26 1 Review I Svante Arrhenius was the first person to recognize the essential nature of acids and bases. 2 Review II Arrhenius postulated that: Acids produce hydrogen
More informationIntroduction to Acids & Bases. Packet #26
Introduction to Acids & Bases Packet #26 Review I Svante Arrhenius was the first person to recognize the essential nature of acids and bases. Review II Arrhenius postulated that: Acids produce hydrogen
More informationSTOICHIOMETRY OF ACID-BASE NEUTRALIZATION REACTIONS. Ms. Grobsky
STOICHIOMETRY OF ACID-BASE NEUTRALIZATION REACTIONS Ms. Grobsky ACID-BASE NEUTRALIZATION REACTIONS Remember, an acid-base neutralization reaction is a special type of double replacement reaction in which
More informationThe Chemistry of Acids and Bases Separately Chapter 14 Part I
Page III-14a-1 / Chapter Fourteen Part I Lecture Notes The Chemistry of Acids and Bases Separately Chapter 14 Part I Strong and Weak Acids/Bases Generally divide acids and bases into STRONG or WEAK categories.
More informationChem 105 Tuesday March 8, Chapter 17. Acids and Bases
Chem 105 Tuesday March 8, 2011 Chapter 17. Acids and Bases 1) Define Brønsted Acid and Brønsted Base 2) Proton (H + ) transfer reactions: conjugate acid-base pairs 3) Water and other amphiprotic substances
More informationChapter 16 - Acids and Bases
Chapter 16 - Acids and Bases 16.1 Acids and Bases: The Brønsted Lowry Model 16.2 ph and the Autoionization of Water 16.3 Calculations Involving ph, K a and K b 16.4 Polyprotic Acids 16.1 Acids and Bases:
More informationAcids and Bases. Reading Assignments: Acids. Bases. Chapter 15 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005
Reading Assignments: Chapter 15 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Or Related topics in other textbooks. Acids and Bases Consultation outside lecture room: Office Hours: Tuesday & Thursday
More informationCHEMFILE MINI-GUIDE TO PROBLEM SOLVING CHAPTER 17. Name Date Class. 1 of 12
CHAPTER 17 In 1909, Danish biochemist S. P. L Sørensen introduced a system in which acidity was expressed as the negative logarithm of the H concentration. In this way, the acidity of a solution having
More informationStoichiometry of Acid-Base Neutralization Reactions. Ms. Grobsky
Stoichiometry of Acid-Base Neutralization Reactions Ms. Grobsky Revisit of Acid-Base Neutralization Reactions Remember, an acid-base neutralization reaction is a special type of double replacement reaction
More informationAcid Base Equilibria
Acid Base Equilibria Critical for most aqueous chemistry (if you ve missed it biochemistry is mostly aqueous chemistry) H2O(l) H + (aq) + OH - (aq) For this reaction which has a higher entropy? H2O(l)
More informationWeak Acid / Base calculations Just to note, the Ka/Kb calculation method from the previous set of notes made a small assumption.
Weak Acid / Base calculations Just to note, the Ka/Kb calculation method from the previous set of notes made a small assumption. Ex. HC 2 H 3 O 2 (aq) H + (aq) + C 2 H 3 O 2 - (aq) [HC 2 H 3 O 2 ] = 0.10M
More informationChapter 15 - Acids and Bases Fundamental Concepts
Chapter 15 - Acids and Bases Fundamental Concepts Acids and Bases: Basic Definitions Properties of Acids Sour Taste React with active metals (Al, Zn, Fe) to yield H 2 gas: Corrosive React with carbonates
More informationEquilibrium constant
Equilibrium constant Equilibrium constant Many reactions that occur in nature are reversible and do not proceed to completion. They come to an equilibrium where the net velocity = 0 The velocity of forward
More informationLecture 20 Chapter 17, Sections 4-5 More weak acids and bases. Identifying acids and bases Conjugate acids and bases Salts of weak acids and bases
Lecture 20 Chapter 17, Sections 4-5 More weak acids and bases Identifying acids and bases Conjugate acids and bases Salts of weak acids and bases Acids and Bases Strong vs. Weak K a vs. K b ph = -log([h])
More informationGrace King High School Chemistry Test Review
CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),
More informationACID-BASE TITRATION AND PH
ACID-BASE TITRATION AND PH Section 1 Aqueous Solutions and the Concept of ph Hydronium and Hydroxide Ions Acids and bases form hydroxide and hydronium ions These ions are not the only ones in an aqueous
More informationAdvanced Chemistry Practice Problems
Finding ph 1. Question: Determine the ph for each of the given solutions. a. 0.150 M HNO3 b. 0.150 M CH3COOH, a = 1.8 10-5 c. 0.150 M CHOOH, a = 3.5 10-4 Answer: The method to determine the ph of a solution
More informationDr. Diala Abu-Hassan, DDS, PhD Lecture 3 MD summer 2014
ph, DDS, PhD Dr.abuhassand@gmail.com Lecture 3 MD summer 2014 www.chem4kids.com 1 Outline ph Henderson-Hasselbalch Equation Monoprotic and polyprotic acids Titration 2 Measuring the acidity of solutions,
More informationProblem Solving. ] Substitute this value into the equation for poh.
Skills Worksheet Problem Solving In 1909, Danish biochemist S. P. L Sørensen introduced a system in which acidity was expressed as the negative logarithm of the H concentration. In this way, the acidity
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationDefinitions. Acids give off Hydrogen ions (protons) Bases give off hydroxide ions
Acids and Bases Arrhenius- Definitions Acids give off Hydrogen ions (protons) Bases give off hydroxide ions This definition did not include enough acids but does explain many. Brønsted-Lowry Acids are
More informationCHEMISTRY 1AA3 Tutorial 2 Answers - WEEK E WEEK OF JANUARY 22, (i) What is the conjugate base of each of the following species?
CHEMISTRY 1AA3 Tutorial 2 Answers - WEEK E WEEK OF JANUARY 22, 2001 M.A. Brook B.E. McCarry A. Perrott 1. (i) What is the conjugate base of each of the following species? (a) H 3 O + (b) NH 4 + (c) HCl
More informationDepartment of Chemistry University of Texas at Austin
Polyprotic and Special Cases Calculations Supplemental Worksheet KEY For the following polyprotic acid questions: Citric acid (H3C6H5O6) Ka1 = 8.4 x 10 4 Ka2 = 1.8 x 10 5 Ka3 = 4.0 x 10 6 Oxalic acid (H2C2O4)
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 4 Acid and Bases 2 Acids Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce
More informationThe Arrhenius Definition of Acids & Bases
ACIDS & BASES The Arrhenius Definition of Acids & Bases An acid produces the hydrogen ion in water. A base produces the hydroxide ion in water. Brønsted Lowry Acids & Bases Brønsted acids are proton donors.
More informationCHEM 116 Buffers and Titration
CHEM 116 Buffers and Titration Lecture 20 Prof. Sevian Today s agenda Equilibrium in acid-base systems Finish comparing strong vs. weak acids (and strong vs. weak bases) Buffers When approximately equal
More informationAcids, Bases, and ph. ACIDS, BASES, & ph
I. Arrhenius Acids and Bases ACIDS, BASES, & ph Acid any substance which delivers hydrogen ion (H + ) _ to the solution. Base any substance which delivers hydroxide ion (OH ) to the solution. II ph ph
More informationCalculating ph. How is ph related to the concentration of hydronium ions? Acidic, Basic or Neutral? [H 3 O + ] [OH ] [H 3
Why? Calculating ph How is ph related to the concentration of hydronium ions? In biology and other science courses ph is introduced as a way to quantify the acidity or basicity of a solution. This property
More informationChapter 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 informationC4S: ACID BASE EQUILIBRIUM Lesson 3
C4S: ACID BASE EQUILIBRIUM Lesson 3 Defining ph and poh We already know that in an acidic solution, [H3O + ] is greater than [OH ]. In an alkaline or basic solution, [OH ] is greater than [H3O + ]. If
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 2 Acid and Bases 3 Acid and Bases 4 Acids 5 Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain
More informationChapter 15. Preview. Lesson Starter Objectives Hydronium Ions and Hydroxide Ions The ph Scale Calculations Involving ph
Preview Lesson Starter Objectives Hydronium Ions and Hydroxide Ions The ph Scale Calculations Involving ph Section 1 Aqueous Solutions and the Concept of ph Lesson Starter Describe what is taking place
More informationChapter 16 Acid-Base Equilibria
Page 1 of 20 Chapter 16 Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids: taste sour and cause certain dyes to change color. Bases: taste bitter and feel soapy. Arrhenius concept o acids
More informationACID 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 informationObjectives. Base Chemistry
May 09, 2014 Objectives AcidAcid Base Chemistry Base Chemistry Chapter 19 Properties of Acids Aqueous solutions of acids taste sour. Change the color of acid/base indicators Many will conduct electrical
More information11/15/11. Chapter 16. HA(aq) + H 2 O(l) H 3 O + (aq) + A (aq) acid base conjugate conjugate
Chapter 16 Table of Contents Chapter 16 16.1 16.2 16.3 16.4 16.5 16.6 Buffered Solutions Copyright Cengage Learning. All rights reserved 2 Models of Arrhenius: Acids produce H + ions in solution, bases
More informationThe Chemistry of Acids and Bases
The Chemistry of 1 Acids and Bases 2 Acid and Bases 3 Acid and Bases 4 Acid and Bases 5 Strong and Weak Acids/Bases Generally divide acids and bases into STRONG or WEAK ones. STRONG ACID: HNO 3 (aq) +
More informationChapter 16 ACIDS AND BASES. (Part I) Dr. Al Saadi. Brønsted Acids and Bases
Chapter 16 ACIDS AND BASES (Part I) Dr. Al Saadi 1 Brønsted Acids and Bases A Brønsted acid is a species that donates a proton. (a proton donor). HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq) acid hydronium
More informationPrinciples of Reactivity: The Chemistry of Acids and Bases. Acids, Bases and Arrhenius
Principles of Reactivity: The Chemistry of Acids and Bases **a lot of calculations in this chapter will be done on the chalkboard Do not rely on these notes for all the material** Acids, Bases and Arrhenius
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
More informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationUnit 4-1 Provincial Practice Questions Page 1
Page 1 Page 2 Page 3 Page 4 Page 5 1.00 Page 6 Page 7 Page 8 55. The conjugate base of HAsO 4 2 is A. H 3 O + B. 3 AsO 4 C. H 3 AsO 4 D. H 2 AsO 4 56. Consider the following acidbase equilibrium: HC 6
More informationChapter 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 informationph and poh * OpenStax
OpenStax-CNX module: m51117 1 ph and poh * OpenStax This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 4.0 By the end of this section, you will be able to:
More informationWhat is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
More informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationTitration region & buffer calculations. An acid base region is a circumstance
CH102 Summer 1 2012 Boston University An acid base region is a circumstance not a sequence of operations Region 1: Only weak acid (base) Region 2: Both weak acid (base) and its conjugate base (acid) Region
More informationA) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species
3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates
More informationAcids and Bases. Click a hyperlink or folder tab to view the corresponding slides. Exit
Acids and Bases Section 18.1 Introduction to Acids and Bases Section 18.2 Strengths of Acids and Bases Section 18.3 Hydrogen Ions and ph Section 18.4 Neutralization Click a hyperlink or folder tab to view
More informationWhat is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
More information8.2. The Equilibrium of Weak Acids and Bases. The Ion Product Constant for Water. 388 MHR Unit 4 Chemical Systems and Equilibrium
In this section, you will 8.2 Section Preview/ Specific Expectations define and perform calculations that involve the ion product constant for water, K w, and the acid dissociation constant, K a compare
More informationIn the Brønsted-Lowry system, a Brønsted-Lowry acid is a species that donates H + and a Brønsted-Lowry base is a species that accepts H +.
16.1 Acids and Bases: A Brief Review Arrhenius concept of acids and bases: an acid increases [H + ] and a base increases [OH ]. 16.2 BrønstedLowry Acids and Bases In the BrønstedLowry system, a BrønstedLowry
More informationMarch 21, 2005 (Print Clearly)
Chemistry 202 Exam 4 KEY March 21, 2005 (Print Clearly) 1. (16 pts) Fill in the blanks with the best answer. 2 points each. (a) Consider the reaction 3A(g) + B(g) 3 C(s) + 3 D(g).!H reaction = -150.0 kj/mol.
More informationChapter 16: Acids and Bases I. Chem 102 Dr. Eloranta
Chapter 16: Acids and Bases I Chem 102 Dr. Eloranta Acids and Bases Acids Sour taste (vinegar) Dissolve many metals Ability to neutralize bases Strong or Weak Bases Bitter taste (caffeine, poisons from
More informationChapter 15. Properties of Acids. Structure of Acids 7/3/08. Acid and Bases
Chapter 15 Acid and Bases Properties of Acids! Sour taste! React with active metals! React with carbonates, producing CO 2! Change color of vegetable dyes!blue litmus turns red! React with bases to form
More information2 NO, has reached a state of dynamic equilibrium, which statement below is true?
Chemistry 11-014, Vining Exam #3 NAME: Answer Key Take Home Version 1. When the reversible reaction, N + O NO, has reached a state of dynamic equilibrium, which statement below is true? (a) Both the forward
More informationAqueous Solutions and the Concept of ph
Aqueous Solutions and the Concept of ph Key Terms self-ionization of water ph poh Section 1 10I, 10J Main Ideas Self-ionization of water forms hydronium and hydroxide ions. The concentrations of hydronium
More informationCHAPTER Acid & Base
CHAPTER 19 19.1 Acid & Base Common Reactions with Acids Dilute: small amount of solute 1-M Concentrated: large amount of solute Indicator: changes color to show the presence of acids or bases : eat or
More informationAll Your Acids and Bases are Belong to us...acid-base Equilibria: Ch Acid-Base Def ns. I. Properties
Acid-Base Def ns. I. Properties Acids Taste sour Feel like water Corrosive ph
More informationSchool 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 informationCHEMISTRY. Chapter 16 Acid-Base Equilibria
CHEMISTRY The Central Science 8 th Edition Chapter 16 Acid-Base Equilibria Kozet YAPSAKLI Why study acids bases? bases are common in the everyday world as well as in the lab. Some common acidic products
More informationAcid-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 informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationWhat is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
More informationLecture 10. Professor Hicks Inorganic Chemistry II (CHE152) Scale of [H 3 O + ] (or you could say [H + ]) concentration
Lecture 10 Professor Hicks Inorganic Chemistry II (CHE152) ph Scale of [H 3 O + ] (or you could say [H + ]) concentration More convenient than scientific notation ph = log [H 3 O + ] still not sure? take
More informationTHE BIG IDEA: REACTIONS. 1. Review nomenclature rules for acids and bases and the formation of acids and bases from anhydrides. (19.
HONORS CHEMISTRY - CHAPTER 19 ACIDS, BASES, AND SALTS OBJECTIVES AND NOTES - V14 NAME: DATE: PAGE: THE BIG IDEA: REACTIONS Essential Questions 1. What are the different ways chemists define acids and bases?
More informationph scale [H 3 O + ] varies over a very wide range. The ph scale simplifies expressing acidity/basicity.
ph scale [H 3 O + ] varies over a very wide range. The ph scale simplifies expressing acidity/basicity. ph = log[h 3 O + ] = log 1 + [H3O ] (really an approximation; just as we did for K expressions we
More informationIMPORTANT NOTE : any numbers to the left of the decimal in ph calculation do not count in significant figures for logarithms.
ph the measure of the acidity or alkalinity ph scale often used as a quick reference < 7 acid 7 neutral >7 base Sören Sörenson defined ph mathematically ph = - log 10 [H + ] the Ap@ in ph comes from the
More informationAcids, 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 informationAcids & Bases Strong & weak. Thursday, October 20, 2011
Acids & Bases Strong & weak 1 Acid Base Dissociation Acid-base reactions are equilibrium processes. The relationship between the relative concentrations of the reactants and products is a constant for
More informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
More informationWhat are the properties of acids and bases?
Text CH. 14 and 15 What are the properties of acids and bases? identify acids and bases based on general observable properties explain how an indicator is used to determine whether a solution is acidic,
More informationChapter 4 Acid-Base Equilibrium DRAFT Answer Key. p. 6. BC Science Chemistry 12 Edvantage Interactive
p. 2 p. 3 p. 6 BC Science Chemistry 12 Edvantage Interactive 2012 1 p. 7 p. 8 p. 9 BC Science Chemistry 12 Edvantage Interactive 2012 2 BC Science Chemistry 12 Edvantage Interactive 2012 3 p. 12 p. 14
More informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
More informationExam Practice. Chapters
Exam Practice Chapters 16.6 17 1 Chapter 16 Chemical Equilibrium Concepts of: Weak bases Percent ionization Relationship between K a and K b Using structure to approximate strength of acids Strength of
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationChapter 16. Acid-Base Equilibria
Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An
More information4.3 ANSWERS TO EXAM QUESTIONS
4. ANSWERS TO EXAM QUESTIONS. (a) (i) A proton donor () (ii) Fully ionised or fully dissociated () (iii) 0 0 4 () mol dm 6 () 4 (b) (i) 50 0 /5 000 () = 0 06 mol dm () () (ii) Mol OH added = 50 0 50/000
More informationAcid-Base Chemistry. Key Considerations
Acid-Base Chemistry Varying Definitions, depends on context/application Arrhenius Acid Base Brönsted/Lowry Lewis 1 Key Considerations Autoprotolysis of Water Water is an amphiprotic substance: can behave
More informationTitration 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 informationMixtures 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 informationChapter 7 Acids and Bases
Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7
More informationChapter 16 Acid Base Equilibria
Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar
More informationLecture Presentation. Chapter 16. Acid Base Equilibria. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 16 Acid Base Equilibria John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius An acid is a substance that, when dissolved in water, increases
More informationProbably Worth Knowing. Recognizing conjugates
Probably Worth Knowing HW database reset and new assignment posted. Not due until Thurs (4/19) which is also Ex 2 date. Exam 2 will cover the last little bit of Kinetics, all of equilibrium and all of
More informationChapter Menu Chapter Menu
Chapter Menu Chapter Menu Section 18.1 Section 18.3 Section 18.4 Introduction to Acids and Bases Hydrogen Ions and ph Neutralization Section 18.1 Intro to Acids and Bases Objectives: Compare the Arrhenius,
More informationAcids & Bases. Chapter 17
Acids & Bases Chapter 17 Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H + ], (also thought of as hydronium ion, H 3 O + )
More informationCHEMISTRY 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 informationLecture 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 informationDo Now May 1, Obj: Observe and describe neutralization reactions. Copy: Balance the neutralization reaction. KCl(aq) + H 2 O(l)
Do Now May 1, 2017 Obj: Observe and describe neutralization reactions. Copy: Balance the neutralization reaction. HCl + KOH KCl(aq) + H 2 O(l) If I had 100 ml of a 0.01 M HCl solution, what is the ph of
More informationObjectives To prepare a dilute solution of a weak acid. To prepare a buffer of a specific ph value.
E x p e r i m e n t Chemistry Is phun! Objectives To prepare a dilute solution of a weak acid. To prepare a buffer of a specific ph value. To observe the effects of adding acid and base to a buffer solution.
More informationAP Chemistry CHAPTER 16 STUDY GUIDE Acid-Base Equilibrium
AP Chemistry CHAPTER 16 STUDY GUIDE AcidBase Equilibrium 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept
More informationAcids - Bases in Water
more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,
More informationLecture #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 informationAdvanced 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 informationSection 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You
More informationAcids and Bases Unit 11
Mr. B s Chemistry Acids and Bases Unit 11 Name Block Let s start our discussion of acids and bases by defining some terms that are essential to the topics that follow. Arrhenius acids and bases are: acid
More informationCHAPTER 19. Acids, Bases, and Salts Acid Base Theories
CHAPTER 19 Acids, Bases, and Salts 19.1 Acid Base Theories ACIDS tart or sour taste Electrolytes Strong acids are corrosive Acid Facts... indicators will change color Blue litmus paper turns pink react
More information