CHEMISTRY - BROWN 13E CH.16 - ACID-BASE EQUILIBRIA - PART 2.
|
|
- Cecil Cross
- 5 years ago
- Views:
Transcription
1 !!
2 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 of to. By taking the log of [H + ] and [OH - ] we can find ph and poh. ph log[h + ] poh log[oh ] p log By recognizing the relationship between [H + ] and [OH - ] with ph and poh we can create new formula relationships. ph log[h + ] poh log[oh ] A species with a ph greater than 7 is classified as and the [H + ] is than the [OH - ]. The the base then the the ph. A species with a ph less than 7 is classified as and the [H + ] is than the [OH - ]. The the acid then the the ph. A species with a ph equal to 7 is classified as and the [H + ] is than the [OH - ]. By using log with the equilibrium expression for water a relationship between ph and poh can be created. ph + poh 14 Page 2
3 PRACTICE: ph and poh (CALCULATIONS 1) EXAMPLE: What is the hydroxide ion and hydronium ion concentration of an aqueous solution that has a ph equal to 6.12? PRACTICE 1: Which of the following solutions will have the lowest concentration of hydronium ions? a) moles C6H5NH2 b) moles Be(OH)2 c) moles SrH2 d) moles (CH3)2NH PRACTICE 2: Which of the following statements about aqueous solutions is/are true? a) For an basic solution the concentration of H3O + is greater than the concentration of OH. b) The ph of a neutral aqueous solution is 7.00 at all temperatures. c) An acidic solution under normal conditions has a ph value less than d) If the concentration of H3O + decreases then the concentration of OH will also decrease. e) The ph of aqueous solutions is less than 7. Page 3
4 PRACTICE: ph and poh (CALCULATIONS 2) EXAMPLE: A solution is prepared by dissolving mol Sr(OH)2 in water to produce a solution with a volume of 750 ml. a) What is the [OH - ]? b) What is the [H + ]? PRACTICE: What is the Kw of pure water at 20.0 C, if the ph is 7.083? a) b) c) d) Page 4
5 CONCEPT: AUTO IONIZATION OF WATER Water can react with itself in a reaction called self ionization where and are produced. H 2 O (l) + H 2 O (l) This reaction is usually written more simply as: H 2 O (l) The equilibrium equation for water is called the (KW) for water and is given by the following: K W [H + ][OH ] At 25 o C, KW, but remember KW, like all other constants K, is temperature dependent. Increasing the temperature will KW. Constant 0 o C 10 o C 50 o C 100 o C K W 1.14 x x x x EXAMPLE: Determine the concentration of hydronium ions for a neutral solution at 25 o C and at 50 o C. Page 5
6 CONCEPT: CALCULATING ph and poh OF STRONG SPECIES STRONG ACIDS & BASES are considered Electrolytes so they ionize completely in water. HCl (aq) NaOH (aq) H 2 O H 2 O H + (aq) + Cl (aq) Na + (aq) + OH (aq) EXAMPLE 1: Calculate the ph of a M solution of CaH2. EXAMPLE 2: Calculate the ph of a M HBr solution to the correct number of significant figures. a) 3.3 b) 3.26 c) d) e) All are correct PRACTICE: Calculate the ph of ml of 4.3 x 10-7 M H2SO4. Page 6
7 CONCEPT: CALCULATING ph and poh OF WEAK SPECIES WEAK ACIDS & BASES are considered Electrolytes so they don t completely ionize in water. HF + H2O NH3 + H2O F (aq) + H3O + (aq) NH4 + (aq) + OH (aq) EXAMPLE 1: Pryridine, an organic molecule, is a very common weak base. C5H5N (aq) + H2O (l) C5H5NH + (aq) + OH - (g) Assume you have a M aqueous solution of pyridine, C5H5N, determine its ph. The Kb value for the compound is 1.5 x Page 7
8 PRACTICE: CALCULATING ph and poh OF WEAK SPECIES (CALCULATIONS 1) EXAMPLE: An unknown weak base has an initial concentration of M with a ph of Calculate its equilibrium base constant. PRACTICE: Determine the ph of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a g ml of solution. (MW of NaCN mol ). The Ka value of HCN is 4.9 x Page 8
9 CONCEPT: ACID & BASE CONSTANTS As you might already realize, there are relatively few strong acids. The great majority of acids are weak acids. Consider a weak monoprotic acid, HA, and its ionization in water: HA (aq) + H2O (l) A (aq) + H3O + (aq) The equilibrium expression for this ionization would be: K a Reactan ts Where Ka represents the and it measures the strength of weak acids. When looking at weak bases we don t use Ka, but instead, which represents the. The relationship between Ka and Kb can be expressed with the following equation: K W K a K b In general, the the Ka the stronger the acid and the the concentration of H +. In general, the the pka the stronger the acid and the the concentration of H +. PRACTICE: If the Kb of NH3 is 1.76 x 10-5, determine the acid dissociation constant of its conjugate acid. Page 9
10 PRACTICE: ACID & BASE CONSTANTS (CALCULATIONS 1) EXAMPLE 1: Knowing that HF has a higher Ka value than CH3COOH, determine, if possible, in which direction the following equilibrium lies. HF (aq) + CH3COO (aq) F (aq) + CH3COOH (aq) a) Equilibrium lies to the left. b) Equilibrium lies to the right. c) Equilibrium is equal and balanced. d) Not enough information given. EXAMPLE 2: What is the equilibrium constant for the following reaction and determine if reactants or products are favored. HCN (aq) + ClO2 (aq) CN (aq) + HClO2 (aq) The acid dissociation constant of HCN is 4.9 x and the acid dissociation of HClO2 is 1.1 x HCN (aq) + H2O (aq) CN (aq) + H3O + (aq) HClO2 (aq) + H2O (aq) ClO2 (aq) + H3O + (aq) Page 10
11 PRACTICE: ACID & BASE CONSTANTS (CALCULATIONS 2) EXAMPLE: Which of the following solutions will have the lowest ph? a) 0.25 M HC2F3O2 b) 0.25 M HIO4 c) 0.25 M HC3H5O3 d) 0.25 M H2CO3 e) 0.25 M HSeO4 PRACTICE 1: Which Bronsted-Lowry base has the greatest concentration of hydroxide ions? a) C2H8N2 (Kb 8.3 x 10-5 ) b) C5H5N (Kb 1.7 x 10-9 ) c) (CH3)3N (Kb 1.0 x 10-6 ) d) C3H7NH2 (Kb 3.5 x 10-4 ) e) C6H5NH2 (Kb 3.9 x ) PRACTICE 2: Which Bronsted-Lowry acid has the weakest conjugate base? a) HCNO (Ka 2.0 x 10-4 ) b) HF (Ka 3.5 x 10-4 ) c) HN3 (Ka 2.5 x 10-5 ) d) H2CO3 (Ka 4.3 x 10-7 ) Page 11
12 CONCEPT: DIPROTIC ACIDS Diprotic acids and bases are compounds that can donate or accept H + ion. For diprotic acids their equations can be illustrated by: H2A (aq) + H2O (l) HA (aq) + H3O + (aq) K a1 Reactan ts HA (aq) + H2O (l) A 2 (aq) + H3O + (aq) K a2 Reactan ts For diprotic bases their equations can be illustrated by: A 2 (aq) + H2O (aq) HA (aq) + OH (aq) K b1 Reactan ts HA (aq) + H2O (aq) H2A (aq) + OH (aq) K b2 Reactan ts Based on these equations the relationship between the different forms of diprotic species are: As a result of these equations for diprotic acids and bases the relationship between Ka and Kb will be: K a1 K b2 K w K a2 K b1 K w When dealing with diprotic acids: 1) H2A can be treated as a monoprotic acid and we use can be used to find ph. 2) HA represents the intermediate form and we use can be used to find ph. 3) A 2 represents the basic form and we use can be used to find ph. Page 12
13 PRACTICE: DIPROTIC ACIDS CALCULATIONS 1 EXAMPLE 1: Sulfurous acid, H2SO3, represents a diprotic acid with a Ka1 1.6 x 10-2 and Ka2 4.6 x Calculate the ph and concentrations of H2SO3, HSO3 and SO3 2 when given M H2SO3. EXAMPLE 2: Determine the ph of M Na2S. Hydrosulfuric acid, H2S, contains Ka1 1.0 x 10-7 and Ka2 9.1 x Page 13
14 CONCEPT: POLYPROTIC ACIDS Our understanding of diprotic acids and bases can be used to understand polyprotic acids and bases. For polyprotic acids their equations can be illustrated by: H 3A (aq) + H 2O (l) H 2A (aq) + H 3O + (aq) K a1 Reactan ts H 2A (aq) + H 2O (l) HA 2 (aq) + H 3O + (aq) K a2 Reactan ts HA 2 (aq) + H 2O (l) A 3 (aq) + H 3O + (aq) K a3 Reactan ts For polyprotic bases their equations can be illustrated by: A 3 (aq) + H 2O (l) HA 2 (aq) + OH (aq) K b1 HA 2 (aq) + H 2O (l) H2A (aq) + OH (aq) K b2 H2A (aq) + H 2O (l) H 3A (aq) + OH (aq) K b3 Reactan ts Reactan ts Reactan ts As a result of these equations for polyprotic acids and bases the relationship between Ka and Kb will be: K a1 K b3 K w K a2 K b2 K w K a3 K b1 K w When dealing with polyprotic acids: H3A can be treated as a monoprotic acid and we use can be used to find ph. A 3 represents the basic form and we use can be used to find ph. H 2 A [H + ] K a1 K a2 [ ] 0 + K a1 K w K a1 + [ ] 0 HA 2 [H + ] K a2k a3 [ ] 0 + K a2 K w K a2 + [ ] 0 Page 14
15 PRACTICE: POLYPROTIC ACIDS CALCULATIONS EXAMPLE 1: Determine the ph of M sodium hydrogen phosphate, Na2HPO4. Phosphoric acid, H3PO4, contains Ka1 7.5 x 10-3, Ka2 6.2 x 10-8 and Ka3 4.2 x EXAMPLE 2: Determine the ph of M citric acid, H3C6H5O7 it possesses Ka1 7.4 x 10-4, Ka2 1.7 x 10-5 and Ka3 4.0 x Page 15
CHEMISTRY - BROWN 14E CH.16 - ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
More informationCHEMISTRY - CLUTCH CH.15 - ACID AND BASE EQUILIBRIUM.
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
More informationCHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM
CHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM 1. The ph of a 0.10 M solution of NH3 containing 0.10 M NH 4 Cl is 9.20. What is the [H3O + ]? a) 1.6 x 10-5 b) 1.0 x 10-1 c) 6.3 x 10-10 d) 1.7 x 10-10 e) 2.0 x
More informationANALYTICAL CHEMISTRY - CLUTCH 1E CH.8 - MONOPROTIC ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ARRHENIUS ACIDS AND BASES The most general definition for acids and bases was developed by Svante Arrhenius near the end of the 19 th century. According to him, the cation
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 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 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 informationHonors Chemistry Study Guide for Acids and Bases. NH4 + (aq) + H2O(l) H3O + (aq) + NH3(aq) water. a)hno3. b) NH3
Honors Chemistry Study Guide for Acids and Bases 1. Calculate the ph, poh, and [H3O + ] for a solution that has a [OH - ] = 4.5 x 10-5? 2. An aqueous solution has a ph of 8.85. What are the [H + ], [OH
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 informationWeek 6 AB Strength, ph, Kw, Acids
Week 6 AB Strength, ph, Kw, Acids Q UEST IO N 1 A 0.1 M solution of an electrolyte has a ph of 4.0. What is the electrolyte? A. a strong acid B. a strong base C. a weak acid D. a weak base E. a salt of
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 informationChemistry 40S Acid-Base Equilibrium (This unit has been adapted from
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.
More informationACID-BASE EQUILIBRIA. Chapter 16
P a g e 1 Chapter 16 ACID-BASE EQUILIBRIA Nature of Acids and Bases Before we formally define acids and bases, let s examine their properties. Properties of Acids Sour taste Ability to dissolve many metals
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 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 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 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 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 informationFormulas and Possibly Necessary Data
Chemistry Quarter IV Review - Answers Formulas and Possibly Necessary Data Δtf = Kf m Δtb = Kb m m = mol solute / mass solvent(kg) C = n V m = nm - log[h3o + ] = ph - log[oh - ] = poh [H3O + ] = 10 =ph
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
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 informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More informationCalorimetry, Heat and ΔH Problems
Calorimetry, Heat and ΔH Problems 1. Calculate the quantity of heat involved when a 70.0g sample of calcium is heated from 22.98 C to 86.72 C. c Ca= 0.653 J/g C q = 2.91 kj 2. Determine the temperature
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 16.1-27 The ph of a 0.10 M solution of a weak base is 9.82. What is the K b for this base? A. 8.8 10-8 B. 2.1
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 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 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 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 informationACIDS, BASES, AND SALTS
ACIDS, BASES, AND SALTS Chapter Quiz Choose the best answer and write its letter on the line. 1. A solution in which the hydroxide-ion concentration is 1 10 2 is a. acidic. c. neutral. b. basic. d. none
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 16. Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of
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 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 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 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 informationEXAM 2 PRACTICE KEY. Leaders: Deborah Course: CHEM 178
Leaders: Deborah Course: CHEM 178 EXAM 2 PRACTICE KEY Instructor: Bonaccorsi/Vela Date: 3/6/18 Make sure you (also) know: Acid-base definitions Arrhenius Bronsted-Lowry Lewis Autoionization process of
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 informationAP Chemistry: Acids & Bases Notes
AP Chemistry: Acids & Bases Notes Objectives Definition of Acids-Bases Acid Strength Base Strength ph-poh Scale Calculating ph of Strong Acids-Bases Calculating ph of Weak Acids-Bases Calculating Ka from
More informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria
Acid-Ionization Equilibria Acid-Base Equilibria Acid ionization (or acid dissociation) is the reaction of an acid with water to produce hydronium ion (hydrogen ion) and the conjugate base anion. (See Animation:
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 information1) What is the Arrhenius definition of an acid? Of a base? 2) What is the Bronsted-Lowry definition of an acid? Of a base?
Problems, Chapter 16 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) What is the Arrhenius definition of an acid? Of a base? An Arrhenius acid is a substance that produces
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 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 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 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 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 informationFormation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic
Formation of a salt (ionic compound): Neutralization reaction molecular Full ionic Eliminate spect ions to yield net ionic Hydrolysis/ reaction with water Anions of Weak Acids Consider the weak acid HF
More informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
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 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 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 informationFirst 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 informationStrong and Weak. Acids and Bases
Strong and Weak Acids and Bases Strength of Acids H2SO4 HSO4 - + H + HNO3 NO3 - + H + Strong Acids HCl Cl - + H + H3PO4 H2PO4 - + H + Phosphoric acid Moderate Acid CH3COOH CH3COO - + H + Acetic acid HF
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 informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Solutions of a Weak Acid or Base
Acid-Base Equilibria 1 Will the following salts be acidic, basic or neutral in aqueous solution? 1.NH 4 Cl.NaCl.KC H O 4.NaNO A = acidic B = basic C = neutral Solutions of a Weak Acid or Base The simplest
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 & 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 informationArrhenius, Bronstead-Lowry, Intro to ph scale
Unit 9 Acid/Base Equilibrium In Class Problems and Notes Arrhenius, Bronstead-Lowry, Intro to ph scale Arrhenius acid and Arrhenius base. An acid is a substance which, when dissolved in water, increases
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 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 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 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 informationDynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state
CHEMISTRY 111 LECTURE EXAM III Material PART 1 CHEMICAL EQUILIBRIUM Chapter 14 I Dynamic Equilibrium I. In a closed system a liquid obtains a dynamic equilibrium with its vapor state Dynamic equilibrium:
More informationFile: AcidBase. Acids and Bases, and Salts. ph and poh. (pp.153,154,164,166,292,294,296, 298)
File: AcidBase. Acids and Bases, and Salts. ph and poh. (pp.153,154,164,166,292,294,296, 298) Show the conjugate acid-base pairs for the following reactions: Pa~e 153 1) C03-2 + H20 ~ HC03-1 + ORI Ans.
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 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 informationStudent Worksheet for Acids and Bases
Student Worksheet for Attempt to work the following practice problems after working through the sample problems in the videos. Answers are given on the last page(s). Relevant Equations Kw = 1.0*10-14 =
More informationProblem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x
Problem 1 What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10 5 )? Write out acid dissociation reaction: C 6 H 5 COOH C 6 H 5 COO H Make an ICE chart since this is a weak
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 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 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 informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following is the weakest acid? 1) A) HF (Ka = 6.8 10-4) B) HNO2 (Ka
More informationChapter 15: Acids and Bases Arrhenius Definitions:
Chapter 15: Acids and Bases Arrhenius Definitions: Acids and Bases s - compounds that produce an increase in [H + ] when dissolved in water bases - compounds that produce an increase in [OH ] when dissolved
More informationChem1120pretest2Summeri2015
Name: Class: Date: Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward
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 informationChemistry 192 Problem Set 3 Spring, 2018 Solutions
Chemistry 19 Problem Set 3 Spring, 018 Solutions 1. Problem 3, page 78, textbook Answer (a) (b) (c) (d) HOBr (acid 1) + HSO 4 (acid 1) + HS (base 1) + C 6 H 5 NH + 3 (acid 1) + H O (base ) H 3O + (acid
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 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 informationGuide to Chapter 15. Aqueous Equilibria: Acids and Bases. Review Chapter 4, Section 2 on how ionic substances dissociate in water.
Guide to Chapter 15. Aqueous Equilibria: Acids and Bases We will spend five lecture days on this chapter. During the first two class meetings we will introduce acids and bases and some of the theories
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 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 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 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 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 informationREVIEW QUESTIONS Chapter Identify the Lewis acid and base in each of the following reactions:
Chemistry 102 REVIEW QUESTIONS Chapter 16 1. For each reaction below, identify the Brønsted-Lowry acid and base and their conjugates: A) NH 4 + (aq) + CN (aq) HCN (aq) + NH 3 (aq) B) (CH 3 ) 3 N (aq) +
More information8.1 Explaining the Properties of Acids & Bases. SCH4U - Chemistry, Gr. 12, University Prep
8.1 Explaining the Properties of Acids & Bases SCH4U - Chemistry, Gr. 12, University Prep Equilibrium & Acids & Bases 2 So far, we have looked at equilibrium of general chemical systems: We learned about
More informationHomework #6 Chapter 7 Homework Acids and Bases
Homework #6 Chapter 7 Homework Acids and Bases 20. a) 2H 2O(l) H 3O (aq) OH (aq) K [H 3 O ][OH ] Or H 2O(l) H (aq) OH (aq) K [H ][OH ] b) HCN(aq) H 2O(l) H 3O (aq) CN (aq) K [H 3O ][CN ] [HCN] Or HCN(aq)
More informationUnit 6: ACIDS AND BASES
Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric
More informationAcid-Base Equilibria. Contents and Concepts. Learning Objectives
Acid-Base Equilibria Contents and Concepts Solutions of a Weak Acid or Base 1. Acid-Ionization Equilibria. Polyprotic Acids 3. Base-Ionization Equilibria 4. Acid Base Properties of Salt Solutions Solutions
More informationAcids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals.
Acids and Bases Properties of Acids and Bases Acids taste. Lemon juice and, for example, are both aqueous solutions of acids. Acids conduct electricity; they are. Some are strong electrolytes, while others
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 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 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 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 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 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 informationAqueous solutions of acids have a sour Aqueous solutions of bases taste bitter
Acid and Bases Exam Review Honors Chemistry 3 April 2012 Chapter 14- Acids and Bases Section 14.1- Acid and Base Properties List five general properties of aqueous acids and bases Properties of Acids Properties
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 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 informationChemistry 12 UNIT 4 ACIDS AND BASES
Chemistry 12 UNIT 4 ACIDS AND BASES CHAPTER 9 and 10 Recall the definitions from Unit 3: Strong electrolyte Strong electrolytic solution Weak electrolyte Weak electrolytic solution Non - electrolyte Acids
More information