BRØNSTED ACIDS & BASES

Size: px
Start display at page:

Download "BRØNSTED ACIDS & BASES"

Transcription

1 ACIDS & BASES

2 BRØNSTED ACIDS & BASES

3 BRØNSTED ACIDS & BASES Brønsted acids are proton donors. Brønsted bases are proton acceptors. Amphoteric species can act as either an acid or a base, depending on the conditions. HSO 4 + HCl H 2 SO 4 + Cl HSO 4 + OH SO H 2 O

4 CONJUGATE ACIDS/BASES: CONJUGATE PAIRS base conjugate acid HSO 4 + OH SO H 2 O acid conjugate base

5 STRENGTHS OF ACIDS

6 MOLECULAR STRUCTURE AND STRENGTH What determines the strength of an acid is how easy it is to remove the acidic proton. There are two things to consider: 1.) How easy it is to break the bond between the acidic proton and the rest of the molecule. a.) Bond length (longer = easier to break) b.) Polarity (more polar = easier to break) 2.) How stable the conjugate base of the acid is after removing the acidic proton. a.) For a monatomic anion, more E.N. = more stable b.) For a polyatomic anion, delocalization of charge = more stable

7 THE HYDROHALIC ACIDS Relative acidity: HF << HCl < HBr < HI Even though the fluoride ion is the most stable (F is most E.N.), the length of the H-X bond is more important here.

8 THE OXOACIDS An acid that has one or more oxygen atoms along with another element. Nitric acid, nitrous acid, sulfuric acid, sulfurous acid, perchloric acid, hypoiodous acid etc. Same central atom, different number of oxygen atoms: More oxygen atoms mean the anion has more resonance forms and is more stable, making the acid stronger. Different central atom, same number of oxygen atoms: the more E.N. central atom makes the bond more polar, and also stabilizes the resulting anion more making the acid stronger.

9 CARBOXYLIC ACIDS Organic acids of the form RCO 2 H where R is the general symbol for a group containing C and/or H, and maybe other elements.

10 ACID-BASE PROPERTIES OF WATER

11 THE AUTOIONIZATION OF WATER H 2 O + H 2 O H 2 O or H 3 O + + OH H + + OH K W = [H 3 O + ][OH ] or K W = [H + ][OH ] At 25 o C in pure water [H 3 O + ] = [OH ] = 1.0 x 10 7 or K W = 1.0 x 10 14

12 AQUEOUS SOLUTIONS In any aqueous solution, not just pure water: K W = [H + ][OH ] = 1.0 x If [H + ] = [OH ] then the solution is neutral If [H + ] > [OH ] then the solution is acidic If [H + ] < [OH ] then the solution is basic

13 ph

14 THE ph SCALE ph = log H 3 O + H 3 O + = 10 ph poh = log OH OH = 10 poh H 3 O + OH = ph + poh = 14

15 STRONG ACIDS & STRONG BASES

16 THE STRONG ACIDS Hydrochloric acid These acids completely dissociate in water Hydrobromic acid Hydroiodic acid Nitric acid The [H 3 O + ] = [acid] because they completely dissociate. Chloric acid Perchloric acid Sulfuric acid (only the first acidic proton completely dissociates) HClO 4 (aq) H + (aq) + ClO 4 (aq)

17 THE STRONG BASES Lithium hydroxide Sodium hydroxide Potassium hydroxide Rubidium hydroxide Cesium hydroxide Calcium hydroxide Strontium hydroxide Barium hydroxide These bases completely dissociate in water The [OH ] = [base] (or 2x[base]) because they completely dissociate. Even though calcium hydroxide and strontium hydroxide are only slightly soluble, what does dissolves does so completely. Ba(OH) 2 (aq) Ba 2+ (aq) + 2OH (aq)

18 WEAK ACIDS AND Ka

19 K a If an acid is not a strong acid, it is a weak acid. Weak acids do not completely dissociate in water, but rather exist at equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A (aq) The equilibrium expression is K a = H 3O + A HA K a is the acid ionization constant

20 𝐾𝑎

21 CALCULATING ph FROM K a Calculating ph means finding [H + ]. This is an equilibrium problem, so we set up an i.c.e. table. Example: Calculate the ph of a solution whose initial concentration of acetic acid is M. ph = 2.54

22 PERCENT IONIZATION % ionization = H+ eq HA In general if the % ionization is < 5% we can assume that [H + ] eq << [HA] 0 and can be neglected in the denominator of the equilibrium expression. Otherwise the quadratic formula must be used. % ionization increases as the [HA] 0 approaches zero.

23 PERCENT IONIZATION What is the percent ionization of acetic acid in the preceding example? = = % Therefore it was safe to neglect [H + ] eq in the equilibrium expression.

24 WEAK BASES AND Kb

25 K b If an base is not a strong base, it is a weak base. Weak bases do not completely dissociate in water, but rather exist at equilibrium: B(aq) + H 2 O(l) HB + (aq) + OH (aq) The equilibrium expression is K a = HB+ OH B K b is the base ionization constant

26 𝐾𝑏

27 CALCULATING ph FROM K b Calculating ph means finding [H + ]. This is an equilibrium problem, so we set up an i.c.e. table. Example: Calculate the ph of a solution whose initial concentration of ethylamine is M. ph = (% ionization = 9.9%, so had to use the quadratic formula)

28 K a FROM ph What is the value of K a for a weak acid if a M solution of the acid gives a solution with ph = 2.34? K a = 4.1 x 10-5

29 K b FROM ph What is the value of K b for a weak base if a M solution of the base gives a ph of 9.44? K b = 1.9 x 10-9

30 CONJUGATE ACID-BASE PAIRS

31 CONJUGATE S STRENGTHS The conjugate base of a strong acid is a weak conjugate base. The conjugate acid of a strong base is a weak conjugate acid. The conjugate base of a weak acid is a strong conjugate base * The conjugate acid of a weak base is a strong conjugate acid * * A strong conjugate base is a weak base * A strong conjugate acid is a weak acid.

32 K b, K a, and K w K b K a = K w pk b + pk a = 14 The K a for nitrous acid is 4.5 x What is K b for the nitrite ion? K b = 2.2 x 10-11

33 POLYPROTIC ACIDS

34 POLYPROTIC ACIDS Acids that have more than one acidic proton lose them successively. The K a s are labeled K a1, K a2, and K a3 (if there is a third acidic proton). K a1 > K a2 > K a3 H 3 C 6 H 5 O 7 H 2 C 6 H 5 O 7 + H + K a1 = 7.1 x 10 4 H 2 C 6 H 5 O 7 HC 6 H 5 O H + K a2 = 1.7 x 10 5 HC 6 H 5 O 7 2 C 6 H 5 O H + K a3 = 6.4 x 10 6

35 Acid Name K a pk a Carbonic, H 2 CO 3 1 st 4.5 x nd 4.7 x Hydrogen sulphide, H 2 S 1 st 9.5 x nd 1.0 x Phosphoric acid, H 3 PO 4 1 st 7.1 x nd 6.3 x rd 4.5 x Sulphuric acid, H 2 SO 4 1 st large 2 nd 1.2 x Telluric acid, H 6 TeO 6 1 st 2.0 x nd 1.0 x rd 3.0 x Sulphurous acid, H 2 SO 3 1 st 1.2 x nd 6.6 x Selenous acid, H 2 SeO 3 1 st 3.5 x nd 5.0 x Tellurous acid, H 2 TeO 3 1 st 3.0 x nd 2.0 x Ascorbic acid, H 2 C 6 H 6 O 6 1 st 7.9 x nd 1.6 x Citric acid, H 3 C 6 H 5 O 7 1 st 7.1 x nd 1.7 x rd 6.4 x

36 Calculate the concentrations of all species present at equilibrium in a 0.25 M solution of citric acid at 25 o C. [H 3 C 6 H 5 O 7 ] = 0.24 M [H 2 C 6 H 5 O 7 ] = M [HC 6 H 5 O 7 2 ] = M [C 6 H 5 O 7 3 ] = M [H + ] = M

37 SALTS AS ACIDS AND BASES

38 SALT HYDROLYSIS When a strong electrolyte is dissolved in water, if the anion is the conjugate base of a weak acid, or the cation is the conjugate acid of a weak base, hydrolysis occurs affecting the ph of the solution. For example, if a M solution of KF is prepared, the following occurs: F + H 2 O HF + OH What is the ph of the resulting solution? K a for HF = 7.1 x 10 4 ph = 8.18

39 THE METAL CATION CAN ALSO REACT WITH H 2 O Small, highly charges metal cations such as Al 3+, Cr 3+, Fe 3+, Bi 3+, and Be 2+ associate with water molecules through ion-dipole interactions. For example the aluminum ion: Al(H 2 O) 6 3+ (aq) Al(OH)(H 2 O) 5 2+ (aq) + H + (aq) K a = 1.3 x 10 5

40 SALT SOLUTIONS Metal cations that are relatively large and/or not highly charged do not undergo hydrolysis. Thus, the group 1A and 2A metals (except Be) do not do this. Anions that are conjugate bases of strong acids do no undergo hydrolysis either. If both the cation and anion hydrolyze: If K a > K b the solutions is acidic If K b > K a the solution is basic If K a K b the solution is neutral, or close to neutral.

41 OXIDES AND HYDROXIDES

42 ALKALI METAL OXIDES AND ALKALINE EARTH METAL HYDROXIDES ARE BASIC (EXCEPT BeO WHICH IS AMPHOTERIC) Na 2 O(s) + H 2 O(l) 2NaOH(aq) CaO(s) + H 2 O(l) Ca(OH) 2 (aq)

43 NONMETAL OXIDES WHOSE NONMETAL HAS A HIGH OXIDATION NUMBER ARE ACIDIC CO 2 (g) + H 2 O(l) SO 3 (g) + H 2 O(l) N 2 O 5 (g) + H 2 O(l) P 4 O 10 (g) + H 2 O(l) Cl 2 O 7 (g) + H 2 O(l) H 2 CO 3 (aq) H 2 SO 4 (aq) 2HNO 3 (aq) 4H 3 PO 4 (aq) 2HClO 4 (aq)

44 LEWIS ACIDS AND BASES

45 DEFINITIONS A Lewis acid is an electron pair donor. A Lewis base is an electron pair acceptor. In every Lewis-base reaction a coordinate covalent bond is formed.

Chapter 16: Acids, Bases, and Salts

Chapter 16: Acids, Bases, and Salts Chapter 16: Acids, Bases, and Salts Key topics: ph scale; acid-base properties of water K a = acid ionization constant; K b = base ionization constant Polyprotic acids BrØnsted Acids and Bases Acid: Base:

More information

Chapter 16 Acid-Base Equilibria. Acids and Bases. What happens when an acid dissolves in water? Acid and base strength. Conjugate acids and bases

Chapter 16 Acid-Base Equilibria. Acids and Bases. What happens when an acid dissolves in water? Acid and base strength. Conjugate acids and bases 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 information

Chapter 16 Acid-Base Equilibria

Chapter 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 information

Unit 7: Acids & Bases

Unit 7: Acids & Bases Definitions of Acids & Bases Unit 7: Acids & Bases Chapter 16 Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved

More information

Chapter 14 - Acids and Bases

Chapter 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 information

Chapter 7 Acids and Bases

Chapter 7 Acids and Bases Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions Midterm Exam 2 7.5 Calculating the ph of Weak Acid Solutions

More information

Chapter 16. Acid-Base Equilibria Acids and Bases: A Brief Review Brønsted-Lowry Acids and Bases. Conjugate Acid-Base Pairs

Chapter 16. Acid-Base Equilibria Acids and Bases: A Brief Review Brønsted-Lowry Acids and Bases. Conjugate Acid-Base Pairs 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 Brønsted-Lowry Acids and Bases In the Brønsted-Lowry system, a Brønsted-Lowry

More information

Bronsted Acids & Bases

Bronsted Acids & Bases Acids and Bases 1 Bronsted Acids & Bases Acid: substance capable of donating a proton (H + ). Base: substance capable of accepting a proton. (definition not dependent on OH - ) 2 Conjugate Pairs CH 3 COOH

More information

Chapter 16. Some Definitions. Some Definitions. What Happens When an Acid Dissolves in Water? 27/07/2014. If it can be either HCO 3 HSO 4 H 2 O

Chapter 16. Some Definitions. Some Definitions. What Happens When an Acid Dissolves in Water? 27/07/2014. If it can be either HCO 3 HSO 4 H 2 O Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Some Definitions Chapter 16 AP Chemistry 2014-15 North Nova Education Centre Mr. Gauthier Arrhenius

More information

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 16.

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 16. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten Chapter 16 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the

More information

Acids and Bases. Chapter 15. Acids. Bases. A Brønsted acid is a proton donor A Brønsted base is a proton acceptor

Acids and Bases. Chapter 15. Acids. Bases. A Brønsted acid is a proton donor A Brønsted base is a proton acceptor Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain

More information

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Acids and Bases

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Acids and Bases Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Acids and Bases Three definitions of acid Who Theory: Acid= When Arrhenius increases H + 1880

More information

Acids and Bases: A Brief Review

Acids 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 information

Aqueous Equilibria: Chemistry of the Water World. Chapter Outline

Aqueous Equilibria: Chemistry of the Water World. Chapter Outline Aqueous Equilibria: Chemistry of the Water World Chapter Outline 15.1 Acids and Bases: The BrØnsted Lowry Model 15.2 Acid Strength and Molecular Structure 15.3 ph and the Autoionization of Water 15.4 Calculations

More information

CHEM 12 Acids and Bases 3/22/2016

CHEM 12 Acids and Bases 3/22/2016 Acids and Bases Name: Expected background knowledge from acids and bases introductory reading: Definitions (Arrhenius, BL) of an acid and base Definitions of conjugate acid and base pairs Properties of

More information

Acids and Bases. Ch a pt e r Aqueous Equilibria: Chemistry 4th Edition McMurry/Fay. MOH(aq) M + (aq) + OH (aq)

Acids and Bases. Ch a pt e r Aqueous Equilibria: Chemistry 4th Edition McMurry/Fay. MOH(aq) M + (aq) + OH (aq) 15 Ch a pt e r Aqueous Equilibria: Acids and Bases Chemistry th Edition McMurry/Fay Dr. Paul Charlesworth Michigan Technological University AcidBase Concepts 01 Arrhenius Acid: A substance which dissociates

More information

Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE

Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE CHEMISTRY THE CENTRAL SCIENCE Professor Angelo R. Rossi Department of Chemistry Spring Semester Acids and Bases: Definitions Arrhenius Definition of Acids and Bases Acids are substances which increase

More information

Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water.

Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Ch 15-16 Acids and Bases 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 base.

More information

Acid-Base Properties of Salt Solutions and Acid-Base Strength

Acid-Base Properties of Salt Solutions and Acid-Base Strength AcidBase Properties of Salt Solutions and AcidBase Strength A salt is simply another name for an ionic compound. Remember, that most salts are strong electrolytes that completely dissociate in solution.

More information

IV. Acids and Bases. react with metals to produce hydrogen gas

IV. Acids and Bases. react with metals to produce hydrogen gas IV. Acids and Bases Properties of Acids and Bases Acids ph

More information

Classes of Chemical Reactions

Classes of Chemical Reactions Classes of Chemical Reactions Reactions in aqueous media Precipitation reactions Acid-Base reactions Oxidation-Reduction reactions Reversible reactions Classes of Chemical Reactions Water (H 2 O), a unique

More information

CH 3 NH 2 + H 2 O <=== CH 3 NH 3 + OH - b. CH 3 CH 2 NH 2 + H 2 O <=== CH 3 CH 2 NH OH - c. HC 2 H 3 O 2 + H 2 O <=== H 3 O + -

CH 3 NH 2 + H 2 O <=== CH 3 NH 3 + OH - b. CH 3 CH 2 NH 2 + H 2 O <=== CH 3 CH 2 NH OH - c. HC 2 H 3 O 2 + H 2 O <=== H 3 O + - Sample Test 2 CHAPTER 16 1. Acids and bases can be defined in several ways. Which of the following are definitions of bases according to these definitions? a compound the produces hydronium ions in water

More information

Chem 1721 Brief Notes: Chapters 15 and 16

Chem 1721 Brief Notes: Chapters 15 and 16 Chem 1721 Brief Notes: Chapters 15 and 16 Chapter 15: Acids and Bases; Chapter 16: Acid-Base Equilibria Bronstsed-Lowry definitions of acids and bases are based on proton transfer acids are proton donors

More information

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

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 information

ACID-BASE NEUTRALIZATION

ACID-BASE NEUTRALIZATION ACID-BASE NEUTRALIZATION ACID-BASE NEUTRALIZATION REACTIONS A second type of chemical reaction that occurs in aqueous solution is an acid-base neutralization reaction So, what are acids and bases? ACIDS

More information

Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water

Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water Quiz number 5 will be given in recitation next week, Feb 26Mar 2 on the first part of Chapter 16, to be covered in lectures this week. 16.1 Acids and Bases: A Brief Review 16.2 BronstedLowry Acids and

More information

Hydrolysis: - Reaction between a salt (ion or ions in a salt) and water to produce an acidic or basic solution.

Hydrolysis: - Reaction between a salt (ion or ions in a salt) and water to produce an acidic or basic solution. Hydrolysis: Reaction between a salt (ion or ions in a salt) and water to produce an acidic or basic solution. Net ionic equations for hydrolysis: An ion + water a molecule or ion + H 3 O + or OH SPECTATORS

More information

Arrhenius Model. Hydronium Ion. Chapter 13 Acids and Bases

Arrhenius Model. Hydronium Ion. Chapter 13 Acids and Bases Chapter 13 Acids and Bases What are Acids and Bases? Strong and Weak Acids and Bases Relative Strengths of Weak Acids Acidic, Basic, and Neutral Solutions The ph Scale Buffered Solutions 131 Copyright

More information

Models of Acids and Bases. The reaction of an acid HA with water to form H 3 O+ and a conjugate base A-. Conjugate Acid/Base Pairs

Models of Acids and Bases. The reaction of an acid HA with water to form H 3 O+ and a conjugate base A-. Conjugate Acid/Base Pairs Models of Acids and Bases ACIDS and BASES Arrhenius Concept: Acids produce H in solution, bases produce OH ion. Brønsted-Lowry: Acids are H donors, bases are proton acceptors. Review Chapter 4 Acids &

More information

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Chapter 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 information

Chapter 16 Acid-Base Equilibria

Chapter 16 Acid-Base Equilibria Chapter 16 AcidBase Equilibria Acids and bases are found in many common substances and are important in life processes. Group Work: Make a list of some common acids and bases. How do we know which is which?

More information

[H + ] =10 ph poh = -Log [OH - ] [OH - ]=10 poh

[H + ] =10 ph poh = -Log [OH - ] [OH - ]=10 poh Self Ionization of Water H 2 O H + + OH - Acids & Bases ph poh [H + ] [OH - ] Pure Water [H + ] = [OH - ], remember: [ ] means concentration 1 x 10 7 = 1 x 10 7 [H + ] > [OH - ], there is an acidic solution

More information

ACIDS AND BASES. In aqueous solution bases have the following properties: bitter taste soapy feeling turn red litmus paper blue neutralise acids

ACIDS AND BASES. In aqueous solution bases have the following properties: bitter taste soapy feeling turn red litmus paper blue neutralise acids acid H appears in the formula base contains OHˉ group acid + base salt + H 2 O HCl + NaOH NaCl + H 2 O ACIDS AND BASES In aqueous solution acids have the following properties: sour taste turn blue litmus

More information

ph of strong acid and base

ph of strong acid and base ph of strong acid and base What does strong mean in terms of acids and bases? Solubility. Basically, if you say an acid or base is strong, then it dissociates 100% in water. These types of situations are

More information

Acids. Names of Some Common Acids. Names of Acids. Learning Check. Solution 8.1. Acids and Bases

Acids. Names of Some Common Acids. Names of Acids. Learning Check. Solution 8.1. Acids and Bases Chapter 8 Acids and Bases Acids 8.1 Acids and Bases Arrhenius acids produce H + ions in water. H 2 O HCl(g) H + (aq) + Cl - (aq) are electrolytes. have a sour taste. turn litmus red. neutralize bases.

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: Acids and Bases In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the properties

More information

Acid-Base Equilibrium. Introduction to Aqueous Acids. Models of Acids and Bases. Introduction to Aqueous Bases. Lewis Acids and Bases

Acid-Base Equilibrium. Introduction to Aqueous Acids. Models of Acids and Bases. Introduction to Aqueous Bases. Lewis Acids and Bases Acid-Base Equilibrium Dr. Ron Rusay Fall 2007 Introduction to Aqueous Acids Acids: taste sour and cause certain dyes to change color. Copyright 2003-2007 R.J. Rusay Introduction to Aqueous Bases Bases:

More information

CHEM 101/105 Aqueous Solutions (continued) Lect-07

CHEM 101/105 Aqueous Solutions (continued) Lect-07 CHEM 101/105 Aqueous Solutions (continued) Lect-07 aqueous acid/base reactions a. a little bit more about water Water is a polar substance. This means water is able to "solvate" ions rather well. Another

More information

Autoionization of Water

Autoionization of Water Water itself is a weak acid and weak base: Two water molecules react to form H 3 O + and OH - (but only slightly) H 2 O H 2 O H 3 O + OH - Autoionization of Water H 2 O (l) + H 2 O (l) H 3 O + (aq) + OH

More information

Chapter Fourteen: ACIDS AND BASES

Chapter Fourteen: ACIDS AND BASES Chapter Fourteen: ACIDS AND BASES 1 Contents p622 14-1 The Nature of Acids and Bases p623 Arrheniuis postulates that acids produce hydrogen ios in aqueous solution, while bases produce hydroxide ions.

More information

Talk in. Arrhenius Acid- Base Definition and ph

Talk in. Arrhenius Acid- Base Definition and ph Talk in. Arrhenius Acid Base Definition and ph When we think of acids, we typically think of the Arrhenius definition. Svante Arrhenius (18591927) Arrhenius Acid = Any compound that increases the hydronium

More information

Answers and Solutions to Text Problems

Answers and Solutions to Text Problems Acids and Bases 10 Answers and Solutions to Text Problems 10.1 According to the Arrhenius theory: a. acids taste sour. b. acids neutralize bases. c. acids produce H 3 O + ions in water. d. potassium hydroxide

More information

UNIT (6) ACIDS AND BASES

UNIT (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 information

Acids and Bases. 1. The solvent 2. The salt

Acids and Bases. 1. The solvent 2. The salt Acids and Bases A logical place to go from our study of hydrogen compounds is Acids and Bases. In 1884 Arrhenius devised a theory to explain acid/base behavior. His theory states that Acids contain protons

More information

Define what strong and weak always mean in aqueous chemistry. species in the equilibrium solution of a weak diprotic acid.

Define what strong and weak always mean in aqueous chemistry. species in the equilibrium solution of a weak diprotic acid. 1 of 14 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly

More information

Proton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College

Proton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College 15.2 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 information

Acids and Bases Chapter 15

Acids and Bases Chapter 15 Acids Acids and Bases Chapter 15 Topics: p scale, Strengths of Acids and Bases, Ionization Constants of Weak Acids and Bases; Properties of Salts ave a sour taste. Vinegar owes its taste to acetic acid.

More information

CHAPTER 14 REVIEW. Acids and Bases. Answer the following questions in the space provided. c. H 2 S. a. nitrous acid. b.

CHAPTER 14 REVIEW. Acids and Bases. Answer the following questions in the space provided. c. H 2 S. a. nitrous acid. b. CHAPTER 14 REVIEW Acids and Bases SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Name the following compounds as acids: sulfuric acid a. H 2 SO 4 sulfurous acid b. H 2

More information

Sample Exercise 16.1 Identifying Conjugate Acids and Bases

Sample Exercise 16.1 Identifying Conjugate Acids and Bases Sample Exercise 16.1 Identifying Conjugate Acids and Bases (a) What is the conjugate base of each of the following acids: HClO 4, H 2 S, PH 4+, HCO 3? (b) What is the conjugate acid of each of the following

More information

CHAPTER 16 (MOORE) ACIDS, BASES AND ACID-BASE EQUILIBRIA

CHAPTER 16 (MOORE) ACIDS, BASES AND ACID-BASE EQUILIBRIA CHAPTER 16 (MOORE) ACIDS, BASES AND ACID-BASE EQUILIBRIA This chapter deals with acids and bases and their equilibria. We will treat acids as proton (H + ) donors in solution and bases as proton acceptors.

More information

Chapter 15 Review. 2. Which is the formula for the hydronium ion? A. OH - B. H 2 O C. H 3 O + D. H 3 O - E. H 2 O +

Chapter 15 Review. 2. Which is the formula for the hydronium ion? A. OH - B. H 2 O C. H 3 O + D. H 3 O - E. H 2 O + Chapter 15 Review Student: 1. Which is not a characteristic property of acids? A. tastes sour B. turns litmus from blue to red C. reacts with metals to yield CO 2 gas D. neutralizes bases E. reacts with

More information

Chapter 16 Acid and Bases. There is an equilibrium between these two ions in water or in any aqueous solution:

Chapter 16 Acid and Bases. There is an equilibrium between these two ions in water or in any aqueous solution: 1 I. Acidic and Basic water solutions: Chapter 16 Acid and Bases A. Dissociation of water The H + ion (or the H 3 O + ion) is characteristic of acidic water solutions. The OH - ion gives basic solutions

More information

Chem 105 Wed Acids and Bases Neutralization reactions OWL 10/2/2009 1

Chem 105 Wed Acids and Bases Neutralization reactions OWL 10/2/2009 1 Chem 105 Wed 10-2-2009 Acids and Bases Neutralization reactions OWL 10/2/2009 1 Definition Acid and Base Acid = Compound that produces H + ions when dissolved in water. Base = Compound that produces OH

More information

Acids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set

Acids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know

More information

Acid-Base Chemistry. Brønsted-Lowry Acids & Bases

Acid-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 information

Equilibrium 1. Molecular Chapter Ionic (Weak Acid / Base ) - Chapter Ionic ( Insoluble Salts) - Chapter 17

Equilibrium 1. Molecular Chapter Ionic (Weak Acid / Base ) - Chapter Ionic ( Insoluble Salts) - Chapter 17 Equilibrium 1. Molecular ------------------- Chapter 15 2. Ionic (Weak Acid / Base ) - Chapter 16 3. Ionic ( Insoluble Salts) - Chapter 17 STRONG Acids & Bases 1. COMPLETELY IONIZED (a) HCl(aq) H + (aq)

More information

Reactions in aqueous solutions Acids, Bases and Neutralization reactions

Reactions in aqueous solutions Acids, Bases and Neutralization reactions Reactions in aqueous solutions Acids, Bases and Neutralization reactions ACIDS Many acids and bases are industrial and household substances and some are important components of biological fluids. Hydrochloric

More information

LESSON ASSIGNMENT. After completing this lesson, you should be able to: 9-2. Calculate buffers problems.

LESSON ASSIGNMENT. After completing this lesson, you should be able to: 9-2. Calculate buffers problems. LESSON ASSIGNMENT LESSON 9 ph and Buffers. TEXT ASSIGNMENT Paragraphs 9-1 through 9-23. LESSON OBJECTIVES After completing this lesson, you should be able to: 9-1. Calculate the ph and poh of a molar acid

More information

ACIDS AND BASES. Chapter 4 Section 4.4 Acid Base Reactions ( ) Chapter 18 Section 18.1, 18.2, 18.3 Naming Acids 70

ACIDS AND BASES. Chapter 4 Section 4.4 Acid Base Reactions ( ) Chapter 18 Section 18.1, 18.2, 18.3 Naming Acids 70 ACIDS AND BASES Chapter 4 Section 4.4 Acid Base Reactions (150 157) Chapter 18 Section 18.1, 18.2, 18.3 Naming Acids 70 Problems: Chapter 18: 5, 7, 21, 23, 24, 43, 44 Chapter 4: 49, 53, 54 Concepts: Definitions

More information

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.

Since 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 information

CHAPTER 14. Acids and Bases

CHAPTER 14. Acids and Bases CHAPTER 14 Acids and Bases 14.1 The Nature of Acids and Bases Arrhenius model Acid supplies H + to an aqueous solution Base supplies OH - to an aqueous solution Bronsted-Lowry model Acid is a proton (H

More information

Chemistry 51 Chapter 10 ACIDS & BASES. The most common definition of acids and bases was formulated by the Swedish chemist Svante Arrhenius in 1884.

Chemistry 51 Chapter 10 ACIDS & BASES. The most common definition of acids and bases was formulated by the Swedish chemist Svante Arrhenius in 1884. ACIDS & BASES Many common substances in our daily lives are acids and bases. Oranges, lemons and vinegar are examples of acids. In addition, our stomachs contain acids that help digest foods. Antacid tablets

More information

Arrhenius Model Acid. Base. Brønsted-Lowry Model Acid. Base. + H O: + H Cl: H O H + [ :Cl: ] -

Arrhenius Model Acid. Base. Brønsted-Lowry Model Acid. Base. + H O: + H Cl: H O H + [ :Cl: ] - Chapter 14 1. Students will be able to define an acid and base in terms of both the Arrhenius and the Bronsted-Lowry definitions and provide examples of each (including examples that follow the Bronsted-Lowry

More information

1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is:

1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is: 1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is: a) K = [H+ ][NO 2 ] [HNO 2 ] b) K = [H+ ][N][O] 2 [HNO 2 ] c) K =

More information

Chapter 15 Acids- Bases. The Nature of Acids and Bases. Some Common Acid. Principles of Chemistry A Molecular Approach, 1 st Ed. Nivaldo J.

Chapter 15 Acids- Bases. The Nature of Acids and Bases. Some Common Acid. Principles of Chemistry A Molecular Approach, 1 st Ed. Nivaldo J. Chapter 15 -Acids and Bases Principles of Chemistry A Molecular Approach, 1 st Ed. Nivaldo J. Tro Dr. Azra Ghumman Memorial University of Newfoundland The Nature of Acids and Bases Properties of Acids:

More information

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g.

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g. Unit 7 Solutions, Acids & Bases Solution mixture + solvent - substance present in the amount solute - in the solvent solvent molecules solute particles ionic substances (separate) based on! Liquid Mixtures

More information

This reaction is often abbreviated as: HA(aq) H + (aq) + A (aq)

This reaction is often abbreviated as: HA(aq) H + (aq) + A (aq) CHAPTER FOURTEEN ACIDS AND BASES For Review 1. a. Arrhenius acid: produce H + in water b. Bρrnsted-Lowry acid: proton (H + ) donor c. Lewis acid: electron pair acceptor The Lewis definition is most general.

More information

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50

Chapter 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 information

Chapter 16 Acids and Bases

Chapter 16 Acids and Bases Chapter 16 Acids and Bases Properties of Acids and Bases 1. Circle the letters of all the terms that complete the sentence correctly. 2. The properties of acids include _. a. reacting with metals to produce

More information

Chapter 10. Acids, Bases, and Salts

Chapter 10. Acids, Bases, and Salts 1 Chapter 10 Acids, Bases, and Salts 2 Ch 10.1 Arrhenius Acid-Base Theory (also in Chapter Medley) Arrhenius Acids produce Arrhenius Bases produce H + in water OH - in water HCl hydrochloric acid KOH HNO

More information

Chemical reactions. Classifications Reactions in solution Ionic equations

Chemical reactions. Classifications Reactions in solution Ionic equations Chemical reactions Classifications Reactions in solution Ionic equations Learning objectives Distinguish between chemical and physical change Write and balance chemical equations Describe concepts of oxidation

More information

PX212CH1516. C MgCO Al(OH) 6. Which of the following acids has the weakest conjugate base in aqueous solution? A) CH 3 COOH B) HOCl C) HF D) HNO 2

PX212CH1516. C MgCO Al(OH) 6. Which of the following acids has the weakest conjugate base in aqueous solution? A) CH 3 COOH B) HOCl C) HF D) HNO 2 C MgCO Al Al(OH) PX212CH1516 1. Which of the following reactions is not readily explained by the Arrhenius concept of acids and bases? A) HCl(g) + NH 3 (g) NH 4 Cl(s) B) HCl(aq) + NaOH(aq) NaCl(aq) + H

More information

Chem 1B Dr. White 1. Chapter 14 Acids and Bases. 14.1 Nature of Acids and Bases. A. Acids. B. Bases

Chem 1B Dr. White 1. Chapter 14 Acids and Bases. 14.1 Nature of Acids and Bases. A. Acids. B. Bases Chem 1B Dr. White 1 Chapter 14 Acids and Bases 14.1 Nature of Acids and Bases A. Acids B. Bases Chem 1B Dr. White 2 C. Arrhenius Definition 1. acid 2. base 3. Acid-base reaction involving Arrhenius acids

More information

Announcements First Exam December 21---Christmas Break begins December 22. Silberberg Chapter 17-18, Skoog 2-7, 11-13

Announcements First Exam December 21---Christmas Break begins December 22. Silberberg Chapter 17-18, Skoog 2-7, 11-13 Announcements First Exam December 21---Christmas Break begins December 22. Silberberg Chapter 17-18, Skoog 2-7, 11-13 10-15 Conceptual Multiple choice questions that have little if any math 3-5 multiple

More information

Acids, Bases, and Salts

Acids, Bases, and Salts Acids, Bases, and Salts General Chemistry Ron Robertson I. Definitions The terms acid, base and salt are attempts to classify and organize reactions - these terms are used to model the behavior of species

More information

Conjugate Acid Base Pairs. Brønsted-Lowry Acids and Bases. Brønsted Lowry Acids & Bases HA + B: A - + BH + Chapter 2

Conjugate Acid Base Pairs. Brønsted-Lowry Acids and Bases. Brønsted Lowry Acids & Bases HA + B: A - + BH + Chapter 2 Brønsted Lowry Acids & Bases Acid-Base Chemistry & Organic Compounds Brønsted-Lowry Acid: Proton (H + ) Donor Brønsted-Lowry Base: Proton (H + ) Acceptor General reaction: HA + B: A - + BH + Chapter 2

More information

TYPES OF CHEMICAL REACTION

TYPES OF CHEMICAL REACTION TYPES OF CHEMICAL REACTION I. METATHESIS REACTIONS (or DOUBLE DISPLACEMENT RXNS) In these reactions the ions of the reactants are exchanged: A + B (aq) + C + D (aq) AD (?) + CB (?) Double Displacement

More information

Types of Reactions. What are Acids &Bases? Chapter 15. Acids & Bases. Definition? a) Arrhenius. b) Bronsted-Lowry. c) Lewis

Types of Reactions. What are Acids &Bases? Chapter 15. Acids & Bases. Definition? a) Arrhenius. b) Bronsted-Lowry. c) Lewis Chapter 15. Acids & Bases Acid/Base Definitions Types of Acids/bases Polyprotic Acids The Ion Product for Water The ph and Other p Scales Aqueous Solutions of Acids and Bases Hydrolysis The Common Ion

More information

Chapter 15 Acids and Bases reading guide.

Chapter 15 Acids and Bases reading guide. Chapter 15 Acids and Bases reading guide. Be active while reading the text. Take notes, think about what you ve read, and ask yourself questions while reading. Use this document as a guide for making your

More information

Solutions for Ch. 14 Acids and Bases Practice Questions

Solutions for Ch. 14 Acids and Bases Practice Questions s for Ch. 14 Acids and Bases Practice Questions 1. In the following reactions, label the Acid, Base, Conjugate Acid, and Conjugate Base. Also indicate the two conjugate acid-base pairs Plan Your Strategy

More information

5. The conjugate base of formic acid, HCOOH, is. A) OH B) CH 3 COO C) HCOO D) CO 2

5. The conjugate base of formic acid, HCOOH, is. A) OH B) CH 3 COO C) HCOO D) CO 2 1. A Br๘nsted acid is a(n). A) proton donor B) hydroxide ion donor C) proton acceptor D) electron donor 2. A Br๘nsted base. A) is a cation B) does not possess a lone pair of electrons C) possesses a lone

More information

Name: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Name: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. Class: Date: Chapter 13 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. In the Brønsted-Lowry model an acid is a. a proton donor. b. a proton

More information

CHAPTER 16: ACIDS AND BASES

CHAPTER 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 information

Chapter 18. Acids and Bases

Chapter 18. Acids and Bases Chapter 18 Acids and Bases Warm Up Name any acids that you have at home. What are they usually used for? Name any bases that you have at home. What are they usually used for? Today s Agenda QOTD: What

More information

A Note on phase symbols, solubility and soluble compounds. Ch 4. Aqueous Reactions and Solution Stoichiometry. Dissociation.

A Note on phase symbols, solubility and soluble compounds. Ch 4. Aqueous Reactions and Solution Stoichiometry. Dissociation. Ch 4. Aqueous Reactions and Solution Stoichiometry Understand the nature of ions in solutions Recognize and write common chemical reactions Use the activity series to predict products of reactions Write

More information

Chapter 15: Properties of Acids. Properties of Bases

Chapter 15: Properties of Acids. Properties of Bases : Properties of Acids An acid is any substance that releases hydrogen ions, H +, into water. Blue litmus paper turns red in the presence of hydrogen ions. Blue litmus is used to test for acids. Acids have

More information

Name Hour. Acids, Bases, Salts & Neutralization. Solution Stoichiometry Notepack

Name Hour. Acids, Bases, Salts & Neutralization. Solution Stoichiometry Notepack Name Hour Acids, Bases, Salts & Neutralization Solution Stoichiometry Notepack The Concentration of a Solution Molarity, Page 509: 1. Define concentration: 2. Define concentrated: 3. Define dilute: 4.

More information

Polyprotic Acids <-- Now it s a tough call as to whether polyprotic acids are important enough for their own piece of paper. But you have to know how

Polyprotic Acids <-- Now it s a tough call as to whether polyprotic acids are important enough for their own piece of paper. But you have to know how Weak Acids Weak acids do not dissociated completely in aqueous solutions. They are somewhat stable molecules and therefore there is an equilibrium constant associated with their dissociation. It s called

More information

Chapter 15: Acids and Bases I. Chem 102 Dr. Curtis

Chapter 15: Acids and Bases I. Chem 102 Dr. Curtis Chapter 15: Acids and Bases I Chem 102 Dr. Curtis Acids and Bases Acids Sour taste vinegar Dissolve many metals Ability to neutralize bases Strong or Weak Bases Bitter taste caffeine, poisons from plants

More information

Chapter 15: Acids and Bases

Chapter 15: Acids and Bases Chapter 15: Acids and Bases Essentials of General Chemistry Ebbing Gammon Ragsdale 2nd Edition Dr. Azra Ghumman Memorial University of Newfoundland 1 Acids and Bases 15.1 Arrhenius Concept of Acids and

More information

Complete the following table: Compound Dissociation reaction NaOH. Zn(NO3)2. Set 00 / Story of general chemistry, gen chem 1 to gen chem 2

Complete the following table: Compound Dissociation reaction NaOH. Zn(NO3)2. Set 00 / Story of general chemistry, gen chem 1 to gen chem 2 Chemistry the study of matter, the stuff of the universe Questions 1. What is stuff? 2. How much stuff? 3. Properties of stuff? 4. What does stuff do? 5. Why does stuff do that? Why is this course required?

More information

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases

Acid/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 information

4/30/2015. Example: Step 1: the equations NaOH Na + + OH 2.00M 2.00M 2.00M HNO 3 H + + NO

4/30/2015. Example: Step 1: the equations NaOH Na + + OH 2.00M 2.00M 2.00M HNO 3 H + + NO Example: During an experiment, a student pours 25.0 ml of 1.40 mol/l nitric acid into a beaker that contains 15.0 ml of 2.00 mol/l sodium hydroxide solution. What is the final ph of the solution? Step

More information

AP Chemistry- Acids and Bases General Properties of Acids and Bases. Bases- originally defined as any substance that neutralized an acid

AP Chemistry- Acids and Bases General Properties of Acids and Bases. Bases- originally defined as any substance that neutralized an acid AP Chemistry Acids and Bases General Properties of Acids and Bases Acids Electrolyte Taste Litmus Phenolphthalein React with metals to give off H 2 gas H 2 SO 4 (aq) + Mg (s) MgSO 4 (aq) + H 2 (g) Ionize

More information

Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution

Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution 2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution Oxides; acidic, basic, amphoteric Classification of oxides - oxide

More information

Acids and Bases. CHEM 102 T. Hughbanks

Acids and Bases. CHEM 102 T. Hughbanks Acids and Bases CHEM 102 T. Hughbanks According to the Brønsted Lowry theory, all acid base reactions can be written as equilibria involving the acid and base and their conjugates. All proton transfer

More information

Acids & Bases. Mr. Matthew Totaro Legacy High School AP Chemistry Pearson Education, Inc.

Acids & Bases. Mr. Matthew Totaro Legacy High School AP Chemistry Pearson Education, Inc. Acids & Bases Mr. Matthew Totaro Legacy High School AP Chemistry 2012 Pearson Education, Inc. Properties of Acids Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au corrosive 2

More information

Lecture 6. Classes of Chemical Reactions

Lecture 6. Classes of Chemical Reactions Lecture 6 Classes of Chemical Reactions Lecture 6 Outline 6.1 The Role of Water as a Solvent 6.2 Precipitation Reactions 6.3 Acid-Base Reactions 1 Electron distribution in molecules of H 2 and H 2 O The

More information

Summary of MQ2 Results: Mean =124 (71 %) Hi = 175. Lo = 32. Your scores will be posted on WebCT

Summary of MQ2 Results: Mean =124 (71 %) Hi = 175. Lo = 32. Your scores will be posted on WebCT Summary of MQ2 Results: Mean =124 (71 %) Hi = 175 Lo = 32 Your scores will be posted on WebCT 16.5 Strong Acids and Bases Strong Acids Strong Bases 16.6 Weak Acids Calculating K a from ph Using K a to

More information

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined). Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are

More information