acid : a substance which base : a substance which H +
|
|
- Benjamin Walton
- 6 years ago
- Views:
Transcription
1 4.4. BronstedLowry Theory of A&B acid : a substance which base : a substance which H Typical BronstedLowry AB rxn eqn: eg1) NH 3 H 2 O NH 4 base acid OH eg2) CH 3 COOH H 2 O CH 3 COO H 3 O H 2 O an acid and a base????? H 2 O is said to be amphiprotic Amphiprotic substance: a substance which can If a substance acts as an acid around a stronger base, or a base around a stronger acid, it is an AMPHIPROTIC substance. (eg. H 2 O Note: every BronstedLowry rxn there is an acid and a base on both sides of the rxn eqn N 2 H 5 S 2 N 2 H 4 HS A B B* A* B* & A* are acids and bases for the reverse reaction Acids classified as: Monoprotic releases one proton. Diprotic releases two protons. Triprotic releases three protons. Polyprotic releases many protons Bases classified as: Monobasic accepts one proton. Dibasic accepts two protons. Tribasic accepts three protons. Polybasic accepts many protons Polyprotic acids release H ions : step 1 step 2 step 3 H 3 PO 4 H 2 PO 4 2 HPO 4 3 PO 4 If a substance has a charge and still has an easily removable then the substance is Also, acids which have lost one proton are amphiprotic H 2 S HS S 2 Hebden #1114 1
2 4.5 Conjugate Acids and Bases Conjugate acidbase pair: the pair of molecules in a rxn eqn that. Conjugate acid: the extra proton Conjugate base: the extra proton BronstedLowry eqns have two conjugate AB pairs: eg1) base 2 acid 2 HF H 2 O F H 3 O acid 1 base 1 Conjugate Pair Conjugate A Conjugate B eg1) HF and F H 3 O and H 2 O What is the conjugate B for the following compounds? NH 4 HCO 3 H 2 PO 4 What is the conjugate A for the following compounds? CH 3 COO OH HC 2 O 4 Connect and label the conjugate pairs: a) HCl H 2 O(l) H 3 O Cl b) H 2 SO 4 H 2 O(l) H 3 O HSO 4 Hebden #16, 19 Summary for a BronstedLowry AB rxn: Conjugate Acid Conjugate Base Conjugate Base Form of A form of B form of A Conjugate Acid form of B 2
3 4.6. Strong and Weak Acids and Bases Recall: Concentrated = molarity (M) (mol/l) and Dilute = molarity BUT in chemistry And Strong acid acid Weak acid acid Strong Acid (SA) or Strong Base (SB): 100%: Eg: NaOH (s) Na OH HCl (g) H Cl Weak Acid (WA) or Weak Base (WB): than 100% dissociated: Eg: NH 3 H 2 O (l) NH 4 OH HF H 2 O (l) H 3 O F not complete dissociation eqb arrows Characteristics of Acids and Bases: are STRONG if they: are WEAK if they: dissociate in water do dissociate completely in water have an undefined, or very Ka value have a Ka value have dissociation rxn ( ) have an dissociation rxn ( ) Examples of STRONG Acids (p334): Examples of STRONG Bases (p. 122): PRACTICE: Describe the acid below as: a)monoprotic, b) diprotic, c) triprotic d) strong, e) weak H 2 SO 4 H HSO 4 HSO 4 H SO 4 2 metal hydroxides Which is a stronger acid? HNO 2 _ HPO 4 2 Which is a stronger base? HC 2 O 4 _ CN 3
4 6. The Levelling Effect Strong acids are 100% dissociated in sol n. are all equiv. to H 3 O sol ns of same conc. eg) 1M HI produces 1M H 3 O and 1M I 1M HClO 4 produces 1M H 3 O and 1M ClO 4 Strengths are leveled Similarly, the strong bases are 100% dissociated in sol n. Therefore, are all equiv. to OH sol ns of that conc eg) 1M KOH produces 1M OH and 1M K 1M NaOH produces 1M OH and 1M Na Strengths are leveled Weaker A&B dissociate to different extents, so have unique strengths. Hebden #
5 4.4. BronstedLowry Theory of A&B acid : a substance which donates a proton base : a substance which accepts a proton H Typical BronstedLowry AB rxn eqn: eg1) NH 3 H 2 O NH 4 base acid OH eg2) CH 3 COOH H 2 O CH 3 COO H 3 O acid base H 2 O an acid and a base????? H 2 O is said to be amphiprotic Amphiprotic substance: a substance which can act as either an acid or a base If a substance acts as an acid around a stronger base, or a base around a stronger acid, it is an AMPHIPROTIC substance. (eg. H 2 O Note: every BronstedLowry rxn there is an acid and a base on both sides of the rxn eqn N 2 H 5 S 2 N 2 H 4 HS A B B* A* B* & A* are acids and bases for the reverse reaction Acids classified as: Monoprotic releases one proton. Diprotic releases two protons. Triprotic releases three protons. Polyprotic releases many protons Bases classified as: Monobasic accepts one proton. Dibasic accepts two protons. Tribasic accepts three protons. Polybasic accepts many protons Polyprotic acids release H ions one at a time: step 1 step 2 step 3 H 3 PO 4 H 2 PO 4 2 HPO 4 3 PO 4 If a substance has a negative charge and still has an easily removable hydrogen then the substance is amphiprotic Also, polyprotic acids which have lost one proton are amphiprotic H 2 S HS S 2 Hebden #1114 5
6 4.5 Conjugate Acids and Bases Conjugate acidbase pair: the pair of molecules in a rxn eqn that differ by one proton. Conjugate acid: has the extra proton Conjugate base: lacks the extra proton BronstedLowry eqns have two conjugate AB pairs: eg1) base 2 acid 2 HF H 2 O F H 3 O acid 1 base 1 Conjugate Pair Conjugate A Conjugate B eg1) HF and F HF F H 3 O and H 2 O H 3 O H 2 O What is the conjugate B for the following compounds? NH 4 NH 3 HCO 3 CO 3 2 H 2 PO 4 HPO 4 2 What is the conjugate A for the following compounds? CH 3 COO CH 3 COOH OH H 2 O HC 2 O 4 H 2 C 2 O 4 Connect and label the conjugate pairs: a) HCl H 2 O(l) H 3 O Cl c) H 2 SO 4 H 2 O(l) H 3 O HSO 4 Hebden #16, 19 Summary for a BronstedLowry AB rxn: Conjugate Acid Conjugate Base Conjugate Base Form of A form of B form of A Conjugate Acid form of B 6
7 4.6. Strong and Weak Acids and Bases Recall: concentrated = high molarity (M) (mol/l) and Dilute = low molarity BUT in chemistry And Strong acid concentrated acid Weak acid dilute acid Strong Acid (SA) or Strong Base (SB): dissociate 100%: Eg: NaOH (s) Na OH HCl (g) H Cl Weak Acid (WA) or Weak Base (WB): less than 100% dissociated: Eg: NH 3 H 2 O (l) NH 4 OH HF H 2 O (l) H 3 O F not complete dissociation eqb arrows Characteristics of Acids and Bases: are STRONG if they: dissociate completely in water have an undefined, or very large Ka value have complete dissociation rxn ( ) are WEAK if they: do NOT dissociate completely in water have a defined Ka value have an equilib dissociation rxn ( ) Examples of STRONG Acids (p334): HClO 4, HI, HBr, HCl, HNO 3, H 2 SO 4 Examples of STRONG Bases (p. 122): NaOH, KOH, Mg(OH) 2,Ca(OH) 2,Fe(OH) 3, Zn(OH) 2 PRACTICE: Describe the acid below as: a)monoprotic, b) diprotic, c) triprotic d) strong, e) weak metal hydroxides H 2 SO 4 H HSO 4 b & d HSO 4 H SO 4 2 a & e Which is a stronger acid? HNO 2 > HPO 4 2 Which is a stronger base? HC 2 O 4 < CN 7
8 6. The Levelling Effect Strong acids are 100% dissociated in sol n. are all equiv. to H 3 O sol ns of same conc. eg) 1M HI produces 1M H 3 O and 1M I 1M HClO 4 produces 1M H 3 O and 1M ClO 4 Strengths are leveled Similarly, the strong bases are 100% dissociated in sol n. Therefore, are all equiv. to OH sol ns of that conc eg) 1M KOH produces 1M OH and 1M K 1M NaOH produces 1M OH and 1M Na Strengths are leveled Weaker A&B dissociate to different extents, so have unique strengths. Hebden #
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 informationUnit 4a Acids, Bases, and Salts Theory
Unit 4a Acids, Bases, and Salts Theory Chemistry 12 Arrhenius Theory of Acids and Bases The first theory that was proposed to explain the actions of acids and bases was by Svante Arrhenius. It is still
More informationUnit 2 Acids and Bases
Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions
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 informationUnit 4: Acid/Base I. abinotes. I) Introduction to Acids and Bases What is an acid?
Unit 4: Acid/Base I I) Introduction to Acids and Bases What is an acid? http://www.kidsknowit.com/flash/animations/acidsbases.swf What are properties of acids? 1) Acids react with. 2) Acids create when
More informationAcids and Bases Review Worksheet II Date / / Period. Molarity. moles L. Normality [H 3 O +1 ] [OH -1 ] ph poh
Honors Chemistry Name Acids and Bases Review Worksheet II Date / / Period Solute Name of Solute Molar Mass grams mole Molarity moles L Normality [H 3 O +1 ] [OH ] ph poh Acidic or Basic 1. HCl Hydrochloric
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 informationIV.4 - The Bronsted-Lowry Theory of Acids and Bases
IV.4 - The Bronsted-Lowry Theory of Acids and Bases The Bronsted-Lowry theory More general than the Arrhenius theory Incorporates all of the Arrhenius theory into a more general scheme Allows for the effect
More informationCHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).
CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).
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 informationAcids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.
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 O ) when dissolved in water. Acids
More informationChemistry 12 Unit 4 Topic A Hand-in Assignment
1 Chemistry 12 Unit 4 Topic A Handin Assignment Answer the following multiplechoice and written response problems on your own paper. Submit your answers for marking. You do not need to show your work for
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic sour milk, sore muscles acetic vinegar phosphoric soft drinks citric citrus fruits malic apples PROPERTIES OF ACIDS PROPERTIES OF BASES 1. Taste sour 1. Taste bitter 2. react
More informationChapter 14 Properties of Acids and Bases
Section 14.1 Defining Acids and Bases Properties of acids and bases Chapter 14 Properties of Acids and Bases taste sour Acids taste bitter Bases conduct electricity no characteristic feel react with metals
More informationAcids 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 informationDuncan. 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 informationPart 01 - Assignment: Introduction to Acids &Bases
Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4
More informationAcids 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 informationChem 1046 Lecture Notes Chapter 17
Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that
More informationChemistry 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 informationUNIT 14 - Acids & Bases
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) Practice: 1. hydro- - HF
More informationAcid / Base Properties of Salts
Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,
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 informationWorksheet 4.1 Conjugate Acid-Base Pairs
Worksheet 4.1 Conjugate AcidBase Pairs 1. List five properties of acids that are in your textbook. Acids conduct electricity, taste sour, neutralize bases, change the color of indicators, and react with
More informationArrhenius Acid-Base Concept Svante Arrhenius, 1884
Arrhenius Acid-Base Concept Svante Arrhenius, 1884 O Acids and bases are electrolytes. O Acids are substances that produce hydrogen ion, H + (aq), in solution. O Bases are substances that produce hydroxide
More informationUnit 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 informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More information-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 informationUnderstanding 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 informationACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) 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 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 informationCh 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs.
Ch 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs. Ch 18 - Acids and Bases I CAN: 1) Compare properties of acids
More informationChap 16 Chemical Equilibrium HSU FUYIN
Chap 16 Chemical Equilibrium HSU FUYIN 1 Definitions: Arrhenius & Brønsted Lowry acid and base Arrhenius theory: An acid is a substance that, when dissolved in water, increases the concentration of hydrogen
More informationGeneral Chemistry II CHM 1046 E Exam 2
General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of
More informationChapter 16. Dr Ayman Nafady
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 Dr Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions
More informationAcid Base Review Package
Acid Base Review Package 1. In which of the following eqb systems is HCO 3 acting as a BronstedLowry base? 2 a. HCO 3 H+ + CO 3 b. HCO 3 + HS 2 H 2 S + CO 3 c. HCO 3 + H 2 S H 2 CO 3 + HS d. HCO 3 + H
More informationUnit 9: Acid and Base Multiple Choice Practice
Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.
More informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
More informationCHAPTER 14 ACIDS AND BASES
CHAPTER 14 ACIDS AND BASES Topics Definition of acids and bases Bronsted-Lowry Concept Dissociation constant of weak acids Acid strength Calculating ph for strong and weak acids and bases Polyprotic acids
More informationCH 15 Summary. Equilibrium is a balance between products and reactants
CH 15 Summary Equilibrium is a balance between products and reactants Use stoichiometry to determine reactant or product ratios, but NOT reactant to product ratios. Capital K is used to represent the equilibrium
More informationAcids and bases, ph and buffers. Dr. Mamoun Ahram Lecture 2
Acids and bases, ph and buffers Dr. Mamoun Ahram Lecture 2 ACIDS AND BASES Acids versus bases Acid: a substance that produces H+ when dissolved in water (e.g., HCl, H2SO4) Base: a substance that produces
More informationI II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is
1. An equation representing the reaction of a weak acid with water is A. HCl + H 2 O H 3 O + + Cl B. NH 3 + H 2 O NH 4 + + OH C. HCO 3 H 2 O H 2 CO 3 + OH D. HCOOH + H 2 O H 3 O + + HCOO 2. The equilibrium
More informationTalk n Acids & Bases... Lady Dog! Definitions
Talk n Acids & Bases... Lady Dog! Definitions So far in this course, we have looked at processes in chemistry that deal with, or are best explained by, ionic salts or molecules. Now we will turn our attention
More informationChapter 16 exercise. For the following reactions, use figure 16.4 to predict whether the equilibrium lies predominantly. - (aq) + OH - (aq)
1 Chapter 16 exercise Q1. Practice exercise page 671 Write the formula for the conjugate acid of the following, HSO 3, F, PO 4 3 and CO. HSO 3 H H 2 SO 4 F H HF PO 4 3 H HPO 4 2 CO H HCO Q2. Practice exercise
More information2. According to the Bronsted-Lowry theory, a base is a(n) A) proton donor. B) proton acceptor. C) electron donor. D) electron acceptor.
CHEM 120 Online Chapter 10. Date: 1. Which of the following statements concerning Arrhenius acids and Arrhenius bases is incorrect? A) In the pure state, Arrhenius acids are covalent compounds. B) In the
More informationIndicator Color in acid (ph < 7) Color at ph = 7 Color in base (ph > 7) Phenolphthalein Bromothymol Blue Red Litmus Blue Litmus
Unit 9: Acids and Bases Notes Introduction and Review 1. Define Acid: 2. Name the following acids: HCl H2SO4 H2SO3 H2S 3. Bases usually contain 4. Name the following bases: NaOH Ca(OH)2 Cu(OH)2 NH4OH Properties
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 informationAcids, Bases, and Salts Review for Sections
1. Consider the following: Review for Sections 4.1 4.9 I H 2 CO 3 + F HCO 3 + HF 2 II HCO 3 + HC 2 O 4 H 2 CO 3 + C 2 O 4 2 III HCO 3 + H 2 C 6 H 6 O 7 H 2 CO 3 + HC 6 H 5 O 7 The HCO 3 is a base in A.
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 informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationChemistry I Notes Unit 10: Acids and Bases
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
More informationContents and Concepts
Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid
More informationProgressive Science Initiative. Click to go to website:
Slide 1 / 33 New Jersey Center for Teaching and Learning Progressive Science Initiative This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and
More informationJudith Herzfeld 1996,1998. These exercises are provided here for classroom and study use only. All other uses are copyright protected.
Judith Herzfeld 1996,1998 These exercises are provided here for classroom and study use only. All other uses are copyright protected. 3.3-010 According to Bronsted-Lowry Theory, which of the following
More informationACIDS, BASES & SALTS DR. RUCHIKA YADU
ACIDS, BASES & SALTS DR. RUCHIKA YADU Properties of Acids Acid is a compound which yields hydrogen ion (H+), when dissolved in water. Acid is sour to the taste and corrosive in nature. The ph value of
More informationChem12 Acids : Exam Questions M.C.-100
Chem12 Acids : Exam Questions M.C.-100 1) Given : HPO 4 2- (aq) + NH 4 + (aq) H 2 PO 4 - (aq) + NH 3 (aq), the strongest acid in the above equation is : a) NH 4 + b) HPO 4 2- c) NH 3 d) H 2 PO 4-2)
More informationPolyprotic acid-base equilibria
Polyprotic acidbase equilibria Diprotic acids and bases Polyprotic acids and bases Diprotic buffers Fractional composition Isoelectric and isoionic ph ph of diprotic acids and bases Example: amino acid
More informationResources:
I. A/B General A. Definitions 1. Arrhenius 2. B-L 3. Lewis *H+=H3O+ B. Properties 1. Acid 2. Base II. ACIDS A. Types 1. Binary 2. Ternary 3. Acid Anhydride B. Protic 1. mono 2. di 3. tri C. Strengths 1.
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 and Salts
(Hebden Unit 4 page 109 182) 182) We will cover the following topics: 1. Definition of Acids and Bases 2. Bronsted-Lowry Acids and Bases 2 1 Arrhenius Definition of Acids and Bases An acid is a substance
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 information10.1 Acids and Bases in Aqueous Solution
10.1 Acids and Bases in Aqueous Solution Arrhenius Definition of Acids and Bases An acid is a substance that gives hydrogen ions, H +, when dissolved in water. In fact, H + reacts with water and produces
More informationNH 3 (aq) + HF (aq) F (aq) + NH 4. NaOH (aq) + H 2 O (l) NaOH (aq) + H 2 O (l) KOH (aq) + H 2 CO 3 (aq) KHCO 3 (aq) + H 2 O (l)
Quiz 2.1 Acid-Base Definitions 1. The conjugate base of H 3O + is: A. H 3O B. H 2O C. H 3O D. H 3O + E. HO 2. What is the conjugate acid of C 6H 5NH 2? A. C 6H 5NH 3 + B. C 6H 5NH C. C 6H 5NH 4 + D. C
More informationConjugate Pairs Practice #1
Name: Key Skill: Learning to Draw Tie Lines Conjugate Pairs Practice #1 Look at each example drawn below. Sets of partners (called s) are matched with tie lines. HNO3 + OH - NO3 - + H2O CH3NH2 + H2O CH3NH3
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 informationCh 7 Practice Problems
Ch 7 Practice Problems 1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a eak acid), the equilibrium constant expression is [H ] [NO 2 ] = [HNO ] 2 [H ][N][O] [HNO 2] =
More information+ H + H 2 PO 4. H + + HAsO In the reaction, HClO 3 + N 2 H 4 ClO 3 + N 2 H + 5, which two species are both bases? Acid Base conj base conj acid
Chapter 7 AcidBase 1. The conjugate acid of HPO 4 2 is a. H 2 PO 4 b. H 3 PO 4 c. PO 4 3 d. PO 4 2 * e. H 2 PO 4 HPO 4 2 is base (accept H ) HPO 4 2 H H 2 PO 4 2. The conjugate base of H 2 AsO 4 is a.
More informationAcids and Bases. Properties, Reactions, ph, and Titration
Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationChapter 13 Acids and Bases
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 13 Acids and Bases Edward J. Neth University of Connecticut Outline 1. Brønsted-Lowry acid-base model 2. The
More informationPart One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow
CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many
More informationAqueous Solutions and Chemical Equilibria:
Aqueous Solutions and Chemical Equilibria: Acidbase titration Complexometric titration Separations Electrochemistry Etc., etc. Illustration: acidbase titrations Concepts and determination of ph during
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 informationChemistry 102 Chapter 15 ACID-BASE CONCEPTS
General Properties: ACID-BASE CONCEPTS ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink Neutralization
More informationUnit 4: Acids and Bases Topic A: Definitions of Acids and Bases and the Relative Strength of Acids and Bases
1 Unit 4: Acids and Bases Topic A: Definitions of Acids and Bases and the Relative Strength of Acids and Bases In this topic we will examine: Various definitions of acids and bases BrønstedLowry definitions
More informationChpt 16: Acids and Bases
Chpt 16 Acids and Bases Defining Acids Arrhenius: Acid: Substances when dissolved in water increase the concentration of H+. Base: Substances when dissolved in water increase the concentration of OH- Brønsted-Lowry:
More informationAcid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33
Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Review acid-base theory and titrations. For all titrations, at the equivalence point, the two reactants have completely reacted with
More informationAcid 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 informationChapter 10 - Acids & Bases
Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic
More informationADVANCED 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 informationCHEMISTRY - BROWN 13E CH.16 - ACID-BASE EQUILIBRIA - PART 2.
!! www.clutchprep.com CONCEPT: ph and poh To deal with incredibly small concentration values of [H + ] and [OH - ] we can use the ph scale. Under normal conditions, the ph scale operates within the range
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 informationChemical Equilibrium. What is the standard state for solutes? a) 1.00 b) 1 M c) 100% What is the standard state for gases? a) 1 bar b) 1.
Chemical Equilibrium Equilibrium constant for the reaction: aa + bb + cc + dd + [C ] c [D ] d... equilibrium constant K = [ A] a [B ] b... [] = concentration relative to standard state molarity (M): for
More informationUNIT 9 CHEMISTRY OF SOLUTIONS
UNIT 9 CHEMISTRY OF SOLUTIONS Acids and Bases 2013 Pearson Education, Inc. Chapter 10, Section 1 1 1 Arrhenius Acids Arrhenius acids produce H + ions in water. H 2 O have a sour taste. turn blue litmus
More informationUnit 9. Acids, Bases, & Salts Acid/Base Equilibrium
Unit 9 Acids, Bases, & Salts Acid/Base Equilibrium Properties of Acids sour or tart taste strong acids burn; weak acids feel similar to H 2 O acid solutions are electrolytes acids react with most metals
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 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 informationProton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College
16.2 Acids Base Proton Transfer Dr. Fred Omega Garces Chemistry 201 Miramar College Important Notes: K a when H 3 O + is produced, K b when OH is produced 1 Acids Bases; Proton Transfer BrønstedLowry AcidsBases
More informationAcids and Bases. Slide 1 / 208. Slide 2 / 208. Slide 3 / 208. Table of Contents: Acids and Bases
Slide 1 / 208 Slide 2 / 208 Acids and Bases Table of Contents: Acids and Bases Click on the topic to go to that section Slide 3 / 208 Properties of Acids and Bases Conjugate Acid and Base Pairs Amphoteric
More informationUnit 7, Lesson 08: The ph of Salt Solutions, Answers
1. Complete the following chart: Unit 7, Lesson 08: The ph of Salt Solutions, Answers on NH 4 PO 3 3- Parent Acid or Base s the parent strong or weak? Will this ion hydrolyze? f the ion will hydrolyze
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 information(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or
Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH
More informationph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate
More informationAcids and Bases. Properties of Acids. Properties of Bases. Slide 1 / 174. Slide 2 / 174. Slide 3 / 174
Slide 1 / 174 Acids and Bases PSI Chemistry covers the material approximately up to slide 75. Properties of Acids Slide 2 / 174 Acids release hydrogen ion(s) into (aqueous) solution Acids neutralize bases
More informationAcid-Base Character of Salt Solutions. Cations. Cations are potentially acidic, but some have no effect on ph.
Acid-Base Character of Salt Solutions The ph of a salt solution will depend on the acidbase nature of both the cation and anion. Cations Cations are potentially acidic, but some have no effect on ph. M(H
More informationAREA 1: WATER. Chapter 6 ACIDS AND BASES. 6.1 Properties of acids and bases
AREA 1: WATER Chapter 6 ACIDS AND BASES 6.1 Properties of acids and bases Acids are: Sour May be corrosive Dissolve in water to produce an electrolyte, Turn blue litmus red Neutralised by bases. Bases
More informationSCH4U Chapter 8 review
Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic
More informationChapter 6 Acids and Bases
Chapter 6 Acids and Bases Introduction Brønsted acid-base reactions are proton transfer reactions. Acids donate protons to bases. In the process, the acid is converted into its conjugate base and the base
More informationUnit 4: ACIDS, BASES AND SALTS
ABS - 1 Unit 4: ACIDS, BASES AND SALTS 4.1 Arrhenius Acids and Bases Acids release H + in water Bases release OH - in water Salts are products of an acid-base neutralization reaction. The salt is an ionic
More informationUnit 10: Acids and Bases
Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus
More information