ACIDS AND BASES. Nonelectrolytes - substances which do not conduct electricity in water solutions.
|
|
- Natalie Barber
- 7 years ago
- Views:
Transcription
1 ACIDS AND BASES Electrolytes substances which will conduct electricity when dissolved in water. Typical electrolytes are strong acids and salt solutions; e.g., NaCl(aq), HCl(aq), etc. Nonelectrolytes substances which do not conduct electricity in water solutions. Strong electrolytes substances which are good conductors of electricity in water solutions. Weak electrolytes substances which are poor conductors of electricity in water solutions.
2 Dissociation The separation of the ions in an ionic compound by the solvent. The ions are already present in the ionic compound. They are simply being separated into individual particles. For example, NaCl(s) H 2 O 6 Na (aq) Cl (aq) Ionization The breaking up of a polar covalent compounds into ions by the solvent. Polar covalent compounds do not contain ions as a pure substance. The ions are formed when the substance dissolves in water. For example, HCl(g) H 2 O 6 H (aq) Cl (aq)
3 Potassium chloride, KCl, a metalnonmetal compound, is classified as an ionic compound and therefore, the ions are simply separated when KCl dissolves in water according to the equation: KCl(aq) H 2 O(R) 6 K (aq) Cl (aq) Acetic acid, CH 3 COOH(R), does not conduct electricity as a pure liquid since all the bonds are covalent (nonmetalnonmetal) bonds. Therefore, acetic acid ionizes is water according to the reaction: CH 3 COOH(R) H 2 O(R) 6 H (aq) CH 3 COO (aq)
4 Arrhenius AcidBase Theory Arrhenius acids substances which dissolve in water to form the hydrogen ion, H, as the positive ion. Some Arrhenius acids are HCl(aq), HNO 3 (aq), H 2 SO 4 (aq), etc. Some Properties of Arrhenius Acids â They have a sour taste ã They change the color of indicators Litmus is red in an acid solution Phenolphthalein is colorless in an acid solution. ä Acids react with metals to form hydrogen gas. å Acids react (neutralize) bases to form a salt and water. Acid(H ) Base (OH ) 6 Salt H 2 O
5 Arrhenius Bases substances which dissolve in water to form the hydroxide ion, OH, as the negative ion. Some Arrhenius bases are soluble metal oxides and hydroxides such as NaOH(aq), KOH(aq), Ca(OH) 2 (aq), etc. Ammonia, NH 3, is also an Arrhenius base. Some Properties of Arrhenius Bases â They have a bitter taste. ã They change the color of some common indicators. Litmus is blue in a basic solution. Phenolphthalein is pink in a basic solution. ä Bases react (neutralize) acids.
6 BrönstedLowry Theory of Acids and Bases Brönsted Acids are proton donors. 1H contains 1 proton, 0 neutrons, 1 electron 1H contains 1 proton, 0 neutrons, 0 electrons Therefore, H equals a proton Protons form a coordinate covalent bond in water to form the hydronium ion, H 3 O. H H 2 O 6 H 3 O or H (aq) = H 3 O Any substance which can donate (lose) a hydrogen can be a Brönsted acid such as HCl, H 2 SO 4, H 2 O, OH, NH 3, etc.
7 Brönsted Bases are proton acceptors. Any neutral molecule and negative ion can be a Brönsted base such as OH, NH 3, H 2 O, HCO 3, CO 3 2, HCl, etc. Positive ions can never be Brönsted bases. Amphiprotic or Amphoteric substances can behave as either an acid or a base.
8 Chart L Substances on the left side of Chart L are acids. Substances on the right side of Chart L are bases. Acids lose a proton (hydrogen) to form a base and bases gain a proton (hydrogen) to form an acid. acid base conjugatebase acid HI I _ H _ HI I HI and I are conjugate pairs
9 Every BrönstedLowry acidbase reaction has a acid and a base on both sides of the equation. base acid B HA conjugate acid conjugate base An acid and its conjugate base and a base and its conjugate acid. HB A
10 Given the reaction: HCl(aq) H 2 O 6 Which substance will be the Brönsted acid? The strongest acid (HCl) will be the acid. acid HCl _ H base H 2 O H conjugate base Cl conjugate acid _ H 3 O Water will be the base. Add HCl 6 H Cl together H 2 O H 6 H 3 O acid HCl base H O 2 conjugate acid H 3 O conjugate base Cl
11 acid HCl base H conjugate base Which are the acids? HCl and H 3 O Which are the bases? H 2 O and Cl O 2 conjugate acid Which are the acid/base conjugate pairs? H 3 O Cl HCl/Cl and H 2 O/H 3 O
12 Given the following BrönstedLowry acidbase reaction: H 2 BO 3 H 3 PO 4 W H 3 BO 3 H 2 PO 4 Which are acids? Which are bases? Which are conjugate pairs? base acid H BO3 H 3 PO 4 2 conjugate acid H conjugate base Given the following BrönstedLowry acidbase reaction: 3 H 2 SO 3 HCO 3 W H 2 CO 3 HSO 3 BO 3 H 2 PO 4 Which are acids? Which are bases? Which are conjugate pairs? acid base conjugate acid conjugate base H2SO3 HCO3 H 2 CO 3 HSO 3
13 Given the following BrönstedLowry acidbase reaction: HSO 4 HS 6 Using Chart L, predict the products. HSO 4 HS W H 2S SO 4 2 Which are acids? Which are bases? Which are conjugate pairs? acid base conjugate acid conjugate base HSO HS 4 H 2 S SO 2 4
14 Given the following BrönstedLowry acidbase reaction: CO 3 2 HPO Using Chart L, predict the products. CO 3 2 HPO 4 2 W HCO 3 PO 4 3 Which are acids? Which are bases? Which are conjugate pairs? base acid conjugate acid conjugate base CO HPO HCO 3 PO 3 4
15 Given the following reaction for the ionization of an acid, HB: HB W H B The equilibrium expression becomes [H ][B ] Ka = [HB] If HB is highly ionized, then the solution would contain a large number of ions and few unionized molecules. small HB large _ H B The equilibrium constant would be large. large [H ][B ] Ka = = a large number [HB] small
16 If HB is a weak acid, then few ions would be produced and the equilibrium constant would be small. many HB few _ H B few [H ][B ] Ka = = a small number [HB] many Therefore, the larger the ionization constant, K a, the stronger the acid, the more ions present in the solution and the better the conductor of electricity. A small constant tells us that the substance is poorly ionized, there are few ions in the solution, a poor conductor of electricity, and is a weak acid.
17 Which of the following compounds is the strongest acid? Which is the weakest? H 3 PO 4 H 2 S HSO 4 NH 3 Which of the following 1.0 M acid solutions is the best conductor of electricity? The poorest? HF HBr HNO 3 CH 3 COOH Which of the above is the strongest electrolyte? The poorest?
18 Given the following BrönstedLowry acidbase reaction: NH 3 HSO 4 6 Using Chart L, predict the products. NH 3 HSO 4 W NH 4 SO 4 2 Which are acids? Which are bases? Which are conjugate pairs? base acid conjugate acid conjugate base NH HSO 4 3 NH 4 SO 2 4
19 Given the following acids and their ionization constants, K a : Acids K a Adipic acid 3.7 x 10 5 Benzoic acid 6.3 x 10 5 Formic acid 1.8 x 10 4 Hypochlorous acid 3.5 x 10 8 Which of the compounds listed above would be the strongest acid? The weakest? Which 1.0 M solution of the compounds listed above would be the best conductor of electricity?
20 Which 1.0 M solution of the compounds listed below would react with 1.00 gram of magnesium metal, Mg, at the greatest rate? Acids K a Acetic acid 1.8 x 10 5 Benzoic acid 6.3 x 10 5 Hydrofluoric acid 3.5 x 10 4 Sulfurous acid 1.5 x 10 2
21 STRONG ACIDS â Strong acids are found at the top left of Chart L. ã Strong acids are nearly completely ionized. very few molecules 100% mostly ions HCl(aq) H (aq) Cl (aq) ä Strong acids have large ionization constants. K a >> 1. å Since strong acids are nearly completely ionized, water solutions of strong acids are strong electrolytes; e.g., they are good conductors of electricity. æ The ion concentration in water solutions of strong acids is the same as the molarity of the solution. 1.0 M 100% 1.0 M 1.0 M HCl(aq) H (aq) Cl (aq) WEAK ACIDS
22 â Weak acids are found at the lower left side of Chart L. ã Weak acids are only slightly ionized. mostly molecules low % very few ions HF(aq) H (aq) F (aq) ä Weak acids have a small ionization constant. K a < 1. å Since weak acids are only slightly ionized, their water solutions are weak electrolytes; e.g., they are poor conductors of electricity. æ The ion concentration in water solutions of weak acids is very low. 1.0 M 2% 0.02 M 0.02 M HF(aq) H (aq) F (aq)
23 STRONG BASES â All soluble (IA and IIA) hydroxides are strong bases (NaOH and KOH are strong bases). ã Strong bases are nearly completely dissociated into ions. 100% mostly ions NaOH(aq) Na (aq) OH (aq) ä Since strong bases are nearly completely ionized, water solutions of strong bases are strong electrolytes; e.g., they are good conductors of electricity. å The ion concentration in water solutions of strong bases is the same as the molarity of the solution. 1.0 M 100% 1.0 M 1.0 M NaOH(aq) Na (aq) OH (aq)
24 WEAK BASES â Weak bases are found in the middle of Chart M and the upper right of Chart L. ã Weak bases are only slightly ionized. mostly molecules NH OH(aq) low % 4 very few ions NH4 (aq) OH (aq) ä Weak bases have a small ionization constant. K b < 1. å Since weak bases are only slightly ionized, their water solutions are weak electrolytes; e.g., they are poor conductors of electricity. æ The ion concentration in water solutions is very low. 1.0 M 0.4% M M NH4 OH(aq) H (aq) OH (aq)
Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
More informationName period Unit 9: acid/base equilibrium
Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton
More informationChapter 14: Acids and Bases
Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid
More informationTOPIC 11: Acids and Bases
TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and
More informationCHAPTER 16: ACIDS AND BASES
CHAPTER 16: ACIDS AND BASES Active Learning: 4, 6, 14; End-of-Chapter Problems: 2-25, 27-58, 66-68, 70, 75-77, 83, 90-91, 93-104 Chapter 15 End-of-Chapter Problems: 69-74, 125, 129, 133 16.1 ACIDS AND
More informationChemistry 52. Reacts with active metals to produce hydrogen gas. Have a slippery, soapy feeling. React with carbonates to produce CO 2
ACID AND BASE STRENGTH Experiment #2 PURPOSE: 1. To distinguish between acids, bases and neutral substances, by observing their effect on some common indicators. 2. To distinguish between strong and weak
More informationUNIT (6) ACIDS AND BASES
UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that
More informationAcids and Bases: A Brief Review
Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.
More information6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must
More informationChapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50
Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs
More informationChem101: General Chemistry Lecture 9 Acids and Bases
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
More informationAcids and Bases HW PSI Chemistry
Acids and Bases HW PSI Chemistry Name 1) According to the Arrhenius concept, an acid is a substance that. A) is capable of donating one or more H + B) causes an increase in the concentration of H + in
More informationChapter 14 - Acids and Bases
Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry
More informationUnit Two: Acids and Bases
Section One: Theoretical Stuff Unit Two: Acids and Bases The concept of acids and bases has existed for centuries. We can discuss them two ways, operational definitions and theoretical definitions. 1.
More informationTopic 8 Acids and bases 6 hours
Topic 8 Acids and bases 6 hours Hydronium ion (H3O + ) = more stable form of hydrogen ion (H + ) H + + H2O H3O + 8.1 Theories of acids and bases 2 hours 1. Arrhenius H-X / M-OH ACID a substance that dissociates
More informationAn acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
More informationQUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -
QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions
More informationCHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?
You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4
More informationCHM1 Review for Exam 12
Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and
More informationAcids and Bases. An Introduction. David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA
Acids and Bases An Introduction David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA Properties of Acids 1. Sour taste (examples: vinegar, citric acid, lemon juice) 2. Turns litmus
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationNote: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2-
AcidBase Chemistry Arrhenius acid: Substance that dissolves in water and provides H + ions Arrhenius base: Substance that dissolves in water and provides OH ions Examples: HCl H + and Cl Acid NaOH Na +
More informationAqueous Ions and Reactions
Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for
More informationAcid-Base (Proton-Transfer) Reactions
Acid-Base (Proton-Transfer) Reactions Chapter 17 An example of equilibrium: Acid base chemistry What are acids and bases? Every day descriptions Chemical description of acidic and basic solutions by Arrhenius
More informationChemistry 3202. Unit 2 Acids and Bases
Chemistry 3202 Unit 2 Acids and Bases Definitions of Acids and Bases An operational definition is one that is based on the observable properties, behaviours or uses of an entity. The earliest definitions
More informationChapter 13 & 14 Practice Exam
Name: Class: Date: Chapter 13 & 14 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Acids generally release H 2 gas when they react with a.
More informationAcid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases
Acids Identifying Acids and Bases Acid (anhydrides) contains H+ ions as the cation, with and other element as the anion Non-metal oxide H2SO4 HI P2O5 Bases Base (anhydrides) Contains OH- as the anion Combined
More informationChapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water
Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,
More informationSuggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99
Chemistry I Accelerated Study Guideline - Chapter 19 Acids, Bases and Salts ------------------------------------------------------------------------------ By the end of this unit, the skills you should
More informationSince we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.
Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHE 1400 - Spring 2015 - Chapter 7 Homework 7 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1)According to Arrhenius, an acid and a base will react
More informationChapter 15 Acids and Bases. Fu-Yin Hsu
Chapter 15 Acids and Bases Fu-Yin Hsu Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria To help break down food To activate enzymes that break
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationAcid-Base Chemistry. Brønsted-Lowry Acids & Bases
Acid-Base Chemistry ν There are a couple of ways to define acids and bases ν Brønsted-Lowry acids and bases ν Acid: H + ion donor ν Base: H + ion acceptor ν Lewis acids and bases ν Acid: electron pair
More informationCh 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent
1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled
More informationp3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic
General Chemistry II Jasperse Acid-Base Chemistry. Extra Practice Problems 1 General Types/Groups of problems: Conceptual Questions. Acids, Bases, and p1 K b and pk b, Base Strength, and using K b or p7-10
More informationCHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
More informationph: Measurement and Uses
ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic
More information4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes
Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the
More informationstoichiometry = the numerical relationships between chemical amounts in a reaction.
1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse
More informationChapter 9 Lecture Notes: Acids, Bases and Equilibrium
Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether
More informationAcid-Base Equilibrium
AcidBaseEquil 1 Acid-Base Equilibrium See AqueousIons in Chemistry 1110 online notes for review of acid-base fundamentals! Acid- Base Reaction in Aqueous Salt Solutions Recall that use [ ] to mean concentration
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationI N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS
Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification
More informationAcids and Bases. Chapter 16
Acids and Bases Chapter 16 The Arrhenius Model An acid is any substance that produces hydrogen ions, H +, in an aqueous solution. Example: when hydrogen chloride gas is dissolved in water, the following
More informationProperties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases
CAPTER Acids, Bases and Salts Properties of Aqueous Solutions of Acids and Bases Strong and Weak Acids Acids are substances that generate in aqueous solutions. Strong acids ionize 0% in water. That is,
More information3/6/2014. Chapter 15. Acids and Bases. Stomach Acid and Heartburn GERD. Curing Heartburn. Common Acids. Properties of Acids. Lecture Presentation
Lecture Presentation Chapter 15 Acids and Bases Sherril Soman Grand Valley State University Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria
More informationTitrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration
Acid-Base Indicators and Titration Curves Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More informationProperties of Acids and Bases
Lab 22 Properties of Acids and Bases TN Standard 4.2: The student will investigate the characteristics of acids and bases. Have you ever brushed your teeth and then drank a glass of orange juice? What
More informationWrite the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.
Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called
More informationACID-BASE REACTIONS/ THE PH CONCEPT.
Dr Mike Lyons School of Chemistry Trinity College Dublin. melyons@tcd.ie ACID-BASE REACTIONS/ THE PH CONCEPT. Chemistry Preliminary Course 2011 1 Lecture topics. 2 lectures dealing with some core chemistry
More information1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
More informationEXPERIMENT 10 Chemistry 110. Solutions Part 2 ACIDS, BASES, AND ELECTROLYTES
EXPERIMENT 10 Chemistry 110 Solutions Part 2 ACIDS, BASES, AND ELECTROLYTES PURPOSE: The purpose of this experiment is to determine the properties of solutions of acids, bases and electrolytes. Students
More informationTopic 5. Acid and Bases
Topic 5 5-1 Acid and Bases Acid and Bases 5-2 There are a number definitions for aicd and bases, depending on what is convenient to use in a particular situation: Arrhenius and Ostwald: Theory of electrolyte
More informationCHAPTER 18 ACID-BASE EQUILIBRIA
CHAPTER 18 ACID-BASE EQUILIBRIA 18.1 The Arrhenius definition classified substances as being acids or bases by their behavior in the solvent water. 18. All Arrhenius acids contain hydrogen and produce
More informationChapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
More informationCh 15: Acids and Bases
Ch 15: Acids and Bases A c i d s a n d B a s e s C h 1 5 P a g e 1 Homework: Read Chapter 15 Work out sample/practice exercises in the sections, Bonus problems: 39, 41, 49, 63, 67, 83, 91, 95, 99, 107,
More informationAuto-ionization of Water
2H 2 O H 3 O + + OH Hydronium ion hydroxide ion Q: But how often does this happen? This is the fundamental concept of all acid-base chemistry In pure water, how much of it is water and how much is ions?
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base A4 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA 1. LEWIS acid electron pair acceptor H, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N BF 3 see
More informationChapter 4 Chemical Reactions
Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser
More information10. Acids, Bases, and Salts. Acids and bases. 10.1 Arrhenius Acid-Base Theory. 10.2 Bronsted-Lowry Acid-Base Theory
10. Acids, Bases, and Salts Acids and bases For centuries people have known acids are in vinegar, lemon juice and many other foods taste sour. Only few hundred years ago that it was discovered that acids
More informationNH 3 + H 2 O + OH - NH 4. Acid-Base Concepts -- Chapter 15 + H + Conjugate Acid-Base Pairs: - H + base. acid
Acid-Base Concepts -- Chapter 15 1. Arrhenius Acid-Base Concept (last semester) Acid: H+ supplier Base: OH- supplier 2. Brønsted-Lowry Acid-Base Concept (more general) (a) Definition (H+ transfer) Acid:
More informationExperiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
More informationCHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHEM 1212 Test II MULTIPLE CHOICE. Choose the one alternative that est completes the statement or answers the question. 1) At 1000 K, the equilirium constant for the reaction is K p = 0.013. 2NO (g) +
More informationSolution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent
Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:
More informationExperiment 16-Acids, Bases and ph
Definitions acid-an ionic compound that releases or reacts with water to form hydrogen ion (H + ) in aqueous solution. They taste sour and turn litmus red. Acids react with certain metals such as zinc,
More informationDefinition The property of exhibiting the qualities of a base
Acids and Bases Word Acidity Alkalinity Amphiprotic Amphoteric Arrhenius Acid Arrhenius Base Basicity Bronsted/Lowry Acid Bronsted/Lowry Base Buret Caustic Conjugate pair Corrosive Electrolyte Hydrolysis
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF
More informationAcids, Bases, and ph
CHAPTER 9 1 SECTION Acids, Bases, and Salts Acids, Bases, and ph KEY IDEAS As you read this section, keep these questions in mind: What properties do acids have? What properties do bases have? How can
More informationEquilibrium Constants The following equilibrium constants will be useful for some of the problems.
1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationChemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
More information4. Acid Base Chemistry
4. Acid Base Chemistry 4.1. Terminology: 4.1.1. Bronsted / Lowry Acid: "An acid is a substance which can donate a hydrogen ion (H+) or a proton, while a base is a substance that accepts a proton. B + HA
More information16.2 THE BRØNSTED LOWRY ACID BASE CONCEPT
16.2 THE RØNSTED LOWRY ACID ASE CONCEPT Practice (Page 724) 1. (a) According to Arrhenius original theory, acids are substances that ionize in an aqueous solution, to produce aqueous hydrogen ions. (b)
More informationAcid-Base Titrations. Setup for a Typical Titration. Titration 1
Titration 1 Acid-Base Titrations Molarities of acidic and basic solutions can be used to convert back and forth between moles of solutes and volumes of their solutions, but how are the molarities of these
More informationChapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
More informationQ1: What is the ph Scale? Q6: As acids become more acidic, their ph values
Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values increase or decrease? Q2: The range of values of the ph scale is: Q7: As bases become more alkaline, their ph values increase
More information- electrolytes: substances that dissolve in water to form charge-carrying solutions
111 Electrolytes and Ionic Theory - electrolytes: substances that dissolve in water to form charge-carrying solutions * Electrolytes form ions in solution - (ions that are mobile are able to carry charge!).
More informationAP*Chemistry The Chemistry of Acids and Bases
AP*Chemistry The Chemistry of Acids and Bases "ACID"--Latin word acidus, meaning sour. (lemon) "ALKALI"--Arabic word for the ashes that come from burning certain plants; water solutions feel slippery and
More informationAcids, Bases, and Indicators Colorful Chemistry
Cool Chemistry Show Activity 7 Acids, Bases, and Indicators Colorful Chemistry GOALS In this activity you will: Identify common household acids and bases. Identify characteristic properties of acids and
More information6.4 EXPLAINING ACIDS AND BASES
Extension 5. Consumer contexts for measuring ph include fish tanks and hot tubs. ndicator solutions and ph test strips are the most appropriate technology because they are inexpensive and give results
More informationChapter 16 Acid-Base Equilibria. Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon
Chapter 16 Acid-Base Equilibria Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon dioxide dissolves in water, it forms carbonic acid, H 2 CO 3. Basic solutions
More informationAcid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!!
Acid/Base Reactions some covalent compounds have weakly bound H atoms and can lose them to water (acids) some compounds produce OH in water solutions when they dissolve (bases) acid/base reaction are very
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationAP Chemistry Summary Acids, Bases and Buffers Definitions:
AP Chemistry Summary Acids, Bases and Buffers Definitions: Arrhenius: Acid - Produces H + ions in solution HCl H + (aq) + Cl - (aq) Base - Produces OH - ions in solution NaOH Na + (aq) + OH - (aq) Dissociation
More informationChapter 6. Solution, Acids and Bases
Chapter 6 Solution, Acids and Bases Mixtures Two or more substances Heterogeneous- different from place to place Types of heterogeneous mixtures Suspensions- Large particles that eventually settle out
More informationChemistry Unit Test Review
SNC 2DI Chemistry Unit Test Review Note: this review sheet only covers the second half of our chemistry unit. You should use our mid-unit test review sheet to recall concepts from the first half of the
More informationRequired Reading Material.
JF Chemistry 1101 2014-2015 Introduction to Physical Chemistry: Acid Base and Solution Equilibria. Professor Mike Lyons School of Chemistry melyons@tcd.ie Required Reading Material. Kotz, Treichel and
More informationAcids and Bases CHAPTER 12. Opening Essay
CHAPTER 12 Acids and Bases Opening Essay Formerly there were rather campy science-fiction television shows in which the hero was always being threatened with death by being plunged into a vat of boiling
More informationEXPERIMENT 20: Determination of ph of Common Substances
Materials: ph paper and color chart (ph range 3 to 12) or ph meter distilled water white vinegar household ammonia (or baking soda) spot plate test or 3 small test tubes stirring rod solutions / fruits
More informationCopyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.
Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of
More informationClassification of Reagents in Chemistry I: Acids and Bases
University of Califnia, Davis F use with UC Davis Chem 8 and 118 Series Classification of Reagents in Chemistry I: Acids and Bases There are 3 definitions of acids and bases. All three are used in both
More information3 The Preparation of Buffers at Desired ph
3 The Preparation of Buffers at Desired ph Objectives: To become familiar with operating a ph meter, and to learn how to use the Henderson-Hasselbalch equation to make buffer solutions at a desired ph
More informationExperiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
More informationMolarity of Ions in Solution
APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.
More informationNAME PER DATE DUE ACTIVE LEARNING IN CHEMISTRY EDUCATION "ALICE" CHAPTER 21 ACIDS AND BASES. Behavior In Water. 21-1 1997, A.J.
NAME PER DATE DUE ACTIVE LEARNING IN CEMISTRY EDUCATIN "ALICE" CAPTER 21 ACIDS AND BASES Behavior In Water 21-1 1997, A.J. Girondi NTICE F RIGTS All rights reserved. No part of this document may be reproduced
More informationChapter 11: Acids and Bases
188 Chapter 11: Acids and Bases For our purposes, an acid is a substance that produces hydrogen ion (H + ) when dissolved in water. A base is a substance that produces hydroxide ion (OH - ) when dissolved
More information