Chapter 14. Acids and Bases
|
|
- Eleanore Morrison
- 5 years ago
- Views:
Transcription
1 Chapter 1. Acids and Bases
2 Reactions in aqueous solutions Precipitation reactions Acid-Base reactions xidation-reduction reactions Precipitation reaction : a reaction which results in the formation of an insoluble products, or precipitate. Acid-Base reaction : a reaction between an acid and a base. xidation-reduction reaction : intermolecular electron transfer reaction
3 Nature of Acids and Bases Properties of acids and bases Acids ave a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with carbonates and bicarbonates to produce carbon dioxide gas Bases ave a bitter taste. Feel slippery. any soaps contain bases.
4 Nature of Acids and Bases Acid Definitions Base Arrhenius + producer - producer Brønsted-Lowry + donor + acceptor Lewis e - pair acceptor e - pair donor Defined only in aqueous solutions Development of concept acid base Cl(aq) + Na(aq) (l) + NaCl(aq) + (aq) + Cl - (aq) Na + (aq)+ - (aq) + (aq) + - (aq) (l)
5 Nature of Acids and Bases Acid Definitions Base Arrhenius + producer - producer Brønsted-Lowry + donor + acceptor Lewis e - pair acceptor e - pair donor Defined in both aqueous and non-aqueous solutions Development of concept base acid (l) Cl(aq) 3 + (aq) Cl - (aq) (hydronium ion) B + A B + + A - conjugate conjugate conjugate conjugate base 1 acid acid 1 base conjugate base: everything that remains of the acid molecule after a proton is lost. conjugate acid: formed when the proton is transferred to the base.
6 Nature of Acids and Bases Acid Definitions Base Arrhenius + producer - producer Brønsted-Lowry + donor + acceptor Lewis e - pair acceptor e - pair donor Defined in both aqueous and non-aqueous solutions Development of concept N 3 (g) + Cl(g) N Cl(s) N + Cl - B + A B + + A - conjugate conjugate conjugate conjugate base 1 acid acid 1 acid 1 conjugate base: everything that remains of the acid molecule after a proton is lost. conjugate acid: formed when the proton is transferred to the base.
7 Nature of Acids and Bases Acid dissociation (ionization) reactions Cl(aq) + (l) 3 + (aq) + Cl - (aq) A(aq) + (l) 3 + (aq) + A - (aq) [ 3 [ A [ 3 [ A [ [ A C[ A a [ 3 [ A [ A [ [ A [ A Acid dissociation constant In short, A(aq) + (aq) + A - (aq) Cl(aq) + (aq) + Cl - (aq) C 3 C(aq) + (aq) + C 3 C - (aq) N + (aq) + (aq) + N 3 (aq) C 6 5 N 3+ (aq) + (aq) + C 6 5 N (aq) [Al( ) 6 3+ (aq) + (aq) + [Al()( ) 5 + (aq)
8 Acid Strength A(aq) + (l) 3 + (aq) + A - (aq) A(aq) + (aq) + A - (aq) a [ 3 [ A [ A [ [ A [ A
9 Acid Strength A(aq) + (l) 3 + (aq) + A - (aq) oxyacids : the acidic proton is attached an oxygen atom. S N 3 Cl 3 P S diprotic acid N Cl P triprotic acid S (aq) + (aq) + S - (aq) : strong S - (aq) + (aq) + S - (aq) : weak rganic acids with carboxyl groups : the acidic proton is carboxylic proton. Generally weak. R C C 3 C C 6 5 C thers: Cl. Cl...
10 Acid Strength A(aq) + (l) 3 + (aq) + A - (aq) a s of strong acids are not listed. Cl(aq) + (aq) + Cl - (aq) a [ [ Cl [ Cl too small to be measured accurately
11 Water as an Acid and a Base Acid Strength Water is amphoteric (it can behave either as an acid or a base). (l) + (l) 3 + (aq) + - (aq) autoionization N 3 + N 3 N + + N - dissociation constant (ion-product constant) w = [ + [ - = 1. x 1-1 at 5 o C ([ + =[ - =1. x 1-7 ) Aqueous solution 1. Neutral solution: [ + = [ - = 1. x 1-7 (ex, pure water). Acidic solution: [ + > [ - 3. Basic solution: [ + < [ - In any case, w = [ + [ - = 1. x 1-1 at 5 o C
12 Water as an Acid and a Base Acid Strength Ex) At 5 o C, a. 1. x b. 1. x c [ +, [ -? neutral, acid, basic? a. [ + = 1. x 1-9 (basic) b. [ + = 1. x 1-7 (neutral) c. [ + = 1. x 1-15 (acidic) Ex) At 6 o C, w = 1 x 1-13 a. 3 + (aq) + - (aq) endothermic, exothermic? b. [ +, [ - in neutral aqueous solution? a. At 5 o C, w = 1 x 1-1 T, w => endothermic b. [ + = [ - = (1x1-13 ) 1/ = 3 x 1-7
13 p Scale In aqueous solution, [ + is typically quite small, we use p scale. p log[ decimal places Neutral solution, [ + = 1. x 1-7 p log significant figures p in water usually ranges from to 1. p log[ p p w log p p 1 w [ log w [ log[ log[ Ex) At 5 o C, p of a sample of human bood is 7.1. p, [ +, [ - p [ [ 1 p
14 Calculating the p of Strong Acid Solutions Ex).1 N 3 (aq), p? 1. Find the major species in the solution. A(aq) + (aq) + A - (aq) a >>1 (l) + (aq) + - (aq) w = 1-1. Calculate p. N 3 (aq) + (aq) + N 3- (aq) Supplying.1 + and.1 N 3 - (l) + (aq) + - (aq) equilibrium, by Le Châtelier's principle, [ - << 1-7 ajor supplier of + :.1 N 3 => [ + =.1 => p =1. Ex) 1. x 1-1 Cl (aq), p? Cl(aq) + (aq) + Cl - (aq) Supplying 1.x1-1 + and 1.x1-1 Cl - (l) + (aq) + - (aq) Produced [ + by Cl is too small to affect water autodissociation. ajor supplier of + : => [ + = 1.x1-7 => p =7.
15 Calculating the p of Weak Acid Solutions 1. List major species in solution. A(aq) + (aq) + A - (aq) a << 1 (l) + (aq) + - (aq) w = 1-1. Choose species that can produce + and write reactions. 3. Based on values, decide on dominant equilibrium.. Write equilibrium expression for dominant equilibrium. 5. List initial concentrations in dominant equilibrium. 6. Define change at equilibrium (as x ). 7. Write equilibrium concentrations in terms of x. 8. Substitute equilibrium concentrations into equilibrium expression. 9. Solve for x the easy way. ( [A -x [A ) 1. Verify assumptions using 5% rule. 11. Calculate [ + and p. Ex) p of 1. F(aq)? a = 7. x 1-1. F,. F(aq) + (aq)+f - (aq) a = 7. x 1 - (l) + (aq)+ - (aq) w = 1. x F(aq) + (aq)+f - (aq) a = 7. x 1 -. a 5.[ F [ F [ [ [ F [ F ~9. F(aq) + (aq) + F - (aq) initial 1. eq 1.-x x x a 7.1 x.71 [ [ F [ F x 1. x x [F.71.7% p log[ log(.71 ) 1.57
16 Calculating the p of Weak Acid Solutions 1. List major species in solution. A(aq) + (aq) + A - (aq) a << 1 (l) + (aq) + - (aq) w = 1-1. Choose species that can produce + and write reactions. 3. Based on values, decide on dominant equilibrium.. Write equilibrium expression for dominant equilibrium. 5. List initial concentrations in dominant equilibrium. 6. Define change at equilibrium (as x ). 7. Write equilibrium concentrations in terms of x. 8. Substitute equilibrium concentrations into equilibrium expression. 9. Solve for x the easy way. ( [A -x [A ) 1. Verify assumptions using 5% rule. 11. Calculate [ + and p. Ex) p of.1 Cl(aq)? a = 3.5 x Cl,. Cl(aq) + (aq)+cl - (aq) a = 3.5 x 1-8 (l) + (aq)+ - (aq) w = 1. x Cl(aq) + (aq)+cl - (aq) a = 3.5 x 1-8. a [ Cl [ [ [ Cl [ Cl [ Cl ~9. Cl(aq) + (aq) + Cl - (aq) initial.1 eq.1-x x x a [ [ Cl [ Cl x x.1 x.1 5 x [Cl % p log[ log( ).3
17 Calculating the p of Weak Acid Solutions p of a ixture of Weak Acids Ex) p of the aq solution containing 1. CN ( a = 6. x 1-1 ) and 5. N ( a =. x 1 - )? [CN -? p? 1. CN, N,. CN(aq) + (aq)+cn - (aq) a = 6. x 1-1 N (aq) + (aq)+n - (aq) a =. x 1 - (l) + (aq)+ - (aq) w = 1. x N (aq) + (aq)+n - (aq) a =. x 1 -. a [ [ N.1 [ N 5~9. N (aq) + (aq) + N - (aq) initial x 1-7 ( ) eq 5.-x x x a.1 [ [ N [ N x.51 x 5. x x [N 11. p log[ [CN -? a % log( [ [ CN [ CN (.51 )[ CN 1. 8 [ CN 1.1 ) 1.35 CN(aq) + (aq) + CN - (aq) initial x 1-7 ( ) eq 1.-y ( 1.) x y
18 Calculating the p of Weak Acid Solutions Percent Dissociation amount dissociated () % Dissociation 1 % initial concentration () Ex) 1. C 3 C(aq) ( a = 1.8 x 1-5 ), % dissociation? C 3 C(aq) + (aq) + C 3 C - (aq) 5 x a 1.81 initial 1. 1.x1-7 ( ) 1. x eq 1.-x x x 3 x [.1 x 1. % dissociation 3 [ C3C [ C3C.1 1%.% [ C C 1. 3 Ex).1 C 3 C(aq) ( a = 1.8 x 1-5 ), % dissociation? C 3 C(aq) + (aq) + C 3 C - (aq) 5 x a 1.81 initial.1 1.x1-7 ( ).1 x eq.1-x x x 3 x [ 1.31 x.1 % dissociation 3 [ C3C [ C3C % 1.3% [ C C.1 3
19 Calculating the p of Weak Acid Solutions Percent Dissociation amount dissociated () % Dissociation 1 % initial concentration () Ex) 1. A(aq) C 3 C(aq) ( a = 1.8 x 1-5 ), % dissociation? + + A - (aq) A:weak acid [.1 3 A(aq) + (aq) + A - (aq) initial [A % dissociation eq [A.% -x x x a [ [ A [ A x [ A x x [ A Suppose the solution is diuluted 1 times at a time, Ex).1 C 3 C(aq) ( x [ a = 1.8 x 1-5 ), % dissociation? new [ A new 1 3 [ 1.31 [ A [ A new % dissociation 1.3% 1 [ new[ A new ( x /1) x a Q [ A [ A /1 1[ A 1 new Equilibrium => more dissociation
20 Acid Bases Definitions Base Arrhenius + producer - producer Brønsted-Lowry + donor + acceptor Lewis e - pair acceptor e - pair donor Strong and weak are used in the same sense for bases as for acids strong = complete dissociation (hydroxide ion supplied to solution) Na(s) Na + (aq)+ - (aq). strong bases all the hydroxides of Group 1A elements (Li, Na,, Rb, Cs) hydroxides of Group A elements (Ca(), Ba(), Sr() ) low solubility
21 Bases Definitions Acid Base Arrhenius + producer - producer Brønsted-Lowry + donor + acceptor Lewis e - pair acceptor e - pair donor Ex) p of 5. x 1 - Na solution? Na(aq) Na + (aq) + - (aq) Supplying 5. x 1 - Na + and - (l) + (aq) + - (aq) equilibrium, by Le Châtelier's principle, [ + << 1-7 ajor supplier of - : 5. x 1 - Na => [ - = 5. x 1 - w [ [ [ (5.1 ) [.1 13 p log(.1 13 ) 1.7
22 Bases weak = very little dissociation (or reaction with water) N 3 (aq) + (l) N + (aq) + - (aq) B(aq) + (l) B + (aq) + - (aq) base acid conjugate conjugate acid base b [ B [ [ B weak bases: many amines (R-N or R N)...
23 Bases Ex) p of 15. N 3 (aq) ( b = 1.8 x 1-5 )? ajor species: N 3, N 3 (aq) + (l) N + (aq) + - (aq) b = 1.8 x 1-5 (l) + (aq) + - (aq) w = 1. x 1-1 ajor - supplier: N 3 (aq) + (l) N + (aq) + - (aq) initial x 1-7 ( ) eq 15.-x x x b [ N [ [ N x 15. x x 1.61 [ N3 [ N 5% rule : [ N p log[ 3 3 p log(1.6 1 p 1. x % ) 1.8 5
24 Polyprotic Acids Polyprotic acids: can furnish more than one proton ( + ) to the solution. C 3 : diprotic acid C 3 (aq) + (aq) + C 3- (aq) C 3- (aq) + (aq) + C 3 - (aq) a1 a [ [ C [ C [ [ C3 [ C C (g) + (l) + (aq) + C 3- (aq) 3 P : triprotic acid 3 P (aq) + (aq) + P - (aq) P - (aq) + (aq) + P - (aq) P - (aq) + (aq) + P 3- (aq) a1 a a3 [ [ P [ P [ [ P [ P 3 [ [ P [ P 3
25 Polyprotic Acids Polyprotic acids: can furnish more than one proton ( + ) to the solution. a 3 a1 a In most cases, only the first disssociation step makes a important contribution to [ +.
26 Polyprotic Acids Ex) p of 5. 3 P (aq)? eq concentrations of 3 P, P -. P -, and P 3-? ajor species: 3 P, 3 P (aq) + (aq) + P - (aq) initial 5. eq 5.-x x x a1 a a3 [ [ P [ P 3 [ [ P [ P 3 [ [ P [ P a1 [ [ P [ P.19 5% rule : 5% 5. 1 [ x 1.91 [ P x x 5. x 5. [ p P x x a [ [ P [ P 1 (1.9 1 ) [ P [ P a [ [ P [ P 1 (1.9 1 ) [ P [ P
27 Polyprotic Acids Ex) p of 1. S (aq)? S (aq) + (aq) + S - (aq) S - (aq) + (aq) + S - (aq) a1 a [ [ S [ S [ [ S [ S very large 1.1 ajor species: +, S -, S - (aq) + (aq) + S - (aq) initial eq 1.-x 1.+x x a [ (1 x) x (1.) x x % rule : 5% x Q=, equilibrium x 1.1 p.
28 Ex) p of 1. x 1 - S (aq)? Polyprotic Acids S (aq) + (aq) + S - (aq) S - (aq) + (aq) + S - (aq) a1 a [ [ S [ S [ [ S [ S very large 1.1 ajor species: +, S -, S - (aq) + (aq) + S - (aq) initial.1.1 eq.1-x.1+x x (.1 x) x (.1) x a 1.1 x x.1.1 5% rule : 5%.1 (.1 x) x 3 a 1.1 x.71 or.51.1 x [.1 x p Q=, equilibrium
29 Salt : ionic compound Acid-Base Properties of Salts A salt in water produces anions and cations. Each ion behave as acids or bases. Salts That Produce Neutral Solutions Salts that consist of the cations of strong bases and the anions of strong acids have no effect on [ + when dissolved in water. => neutral solution NaCl(aq) Na + (aq) + Cl - (aq) Cl(aq) + (aq) + Cl - (aq) Na(aq) Na + (aq) + - (aq) no => Cl - no effect on [ + (or [ - ) no =>Na + : no effect on [ - (or [ + ) Examples) Cl, NaCl, NaN 3, N 3
30 Acid-Base Properties of Salts Salts That Produce Basic Solutions For any salt whose cation has neutral properties (such as Na + or + ) and whose anion is the conjugate base of a weak acid, the aqueous solution will be basic. NaC 3 C in an aqueous solution. => ajor species: C 3 C -, Na +, C 3 C - (aq) + (l) C 3 C(aq) + - (aq) a b for acetic acid 1.81 [ C3C[ [ C C C 3 C(aq) + (aq) + C 3 C - (aq) 5 3 [ C3C [ [ C C 3 no effect on [ + a [ b [ C3C [ [ C C [ 3 w [ C3C[ [ C C 3 For any weak acid and its conjugate base, a x b = w b w a basic solution
31 Acid-Base Properties of Salts Salts That Produce Basic Solutions For any salt whose cation has neutral properties (such as Na + or + ) and whose anion is the conjugate base of a weak acid, the aqueous solution will be basic. Ex) p of.3 NaF solution? ( a for F = 7. x 1 - ) ajor species in the solution: Na +, F -, Na + : neutral F - (aq) + (l) F(aq) + - (aq) [ -? F - (aq) + (l) F(aq) + - (aq) initial.3 1. x 1-7 ( ) eq.3-x x x b [ F[ [ F x.1 [ 6 w a x (5% rule : [ F x , p 1 p p 5.69 x.3 x 5% ) x.3
32 Acid-Base Properties of Salts Base Strength in Aqeous Solution In acid strength section, we said CN(aq) + (l) 3 + (aq) + CN - (aq) a = 6. x 1-1 CN: weak acid => CN - : strong base? CN - (aq) + (l) CN(aq) + - (aq) b = w / a = 1.6 x 1-5 stronger than (CN - competing with for + ) Actually b is small => CN - : weak base weaker than - (CN - competing with - for + ) base strength : - > CN - >
33 Acid-Base Properties of Salts Salts That Produce Acidic Solutions Salts in which the anion is not a base and the cation is the conjugate acid of a weak base produce acidic solution. Ex) p of.1 N Cl solution? ( b for N 3 = 1.8 x 1-5 ) ajor species in the solution: N +, Cl -, Cl - : neutral N + (aq) N 3 (aq) + + (aq) initial.1 1. x 1-7 ( ) eq.1-x x x a [ N3[ [ N x w b x (5% rule : [ N [ x 7.51 p x.1 x 6 5% ) x.1
34 Acid-Base Properties of Salts Salts That Produce Acidic Solutions Aqueous solution containing highly charged metal ion => acidic Al( ) 6 3+ (aq) + (aq) + Al()( ) 5 + (aq) Ex) p of.1 AlCl 3 aq solution? ( a for Al( ) 6 3+ = 1. x 1-5 ) ajor species in the solution: Al 3+, Cl -, Cl - : neutral Al( ) 3+ 6 (aq) Al()( ) + 5 (aq) + + (aq) initial.1 1. x 1-7 ( ) eq.1-x x x a [ Al( )( [ Al( x 3.71 ) ) x (5% rule : [ Al( ) [ [ 1.1 x 3.71 p x.1 x x.1 5% )
35 Acid-Base Properties of Salts Salts Consting of Basic Anion and Acidic Cation Salts in which the anion is the conjugate base of a weak acid and the cation is the conjugate acid of a weak base produce either acidic or basic solution. a > b (p<7, acidic), a = b (p=7, neutral), a < b (p>7, basic) Ex) acidic, neutral, basic in solution? (a) N C 3 C, (b) N CN, (c) Al (S ) 3 (a) a for N + = 5.6 x 1-1, b for C 3 C - = 5.6 x 1-1 => neutral (b) a for N + = 5.6 x 1-1, b for CN - = w / a (CN) = 1.6 x 1-5 => basic (c) a for Al( ) 6+ = 1. x 1-5, b for S - = w / a (S - ) = 8.3 x 1-13 => acidic Ex) p of.1 N CN solution? ajor species in solution: N +, CN -, N + (aq) N 3 (aq)+ + (aq), a = 5.6 x 1-1 CN - (aq)+ (l) CN(aq)+ - (aq), b = 1.6 x 1-5 (l) + (aq)+ - (aq), w = 1. x 1-7 CN - (aq) + (l) CN(aq) + - (aq) initial.1 1. x 1-7 ( ) eq.1-x x x b 1.61 x 1.31 [ 3 5 [ CN[ [ CN x (5% rule : [ CN x , p.89 p 1 p x x.1 x % ).1
36 Acid-Base Properties of Salts Case Actually, alll depend on the relative magnitudes of a, b, and w (case 1) a << w and b << w => w dominant => neutral (case ) a << w => b dominant => basic (case 3) b << w => a dominant => acidic (case ) a > b => a dominant => acidic (case 5) a < b => b dominant => basic (case 6) a = b => neural
37 Effect of Structure on Acid-Base Properties Brønsted-Lowry (Acid) + donor (Base) + acceptor Any molecule containing a hydrogen atom is potentially an acid. C nonpolar polar What structural properties of a molecule cause it to behave as an acid or as a base? Bond strength (the lower, the more acidic) and bond polarity (the higher, the more acidic) -Cl Bond strength (kcal/mol) 1 13 Acidic? No Strong acid Bond polarity most least
38 Effect of Structure on Acid-Base Properties xyacids acidity - Bond Polarity Aqueous solution containing highly charged metal ion => acidic Al 3+ electron density
39 Effect of Structure on Acid-Base Properties xyacids Is --Y always acidic? No. We know Na, are basic. --Y Electronegativity of Y high very low -Y bond characteristics covalent and strong ionic In aqueous solution polar - bond broken polar -Y bond broken Releasing + and -Y - - and Y + Acidic, Basic? acidic basic
40 Acid-Base Properties of xides Acidic xides (Acid Anhydrides): xides with -Y bond is strong and covalent. => forming acidic solution in water. Ex) S 3, S, N, C S 3 (g) + (l) S (aq) S (g) + (l) S 3 (aq) C (g) + (l) C 3 (aq) N (g) + (l) N 3 (aq)+ N (aq) S N Basic xides (Base Anhydrides): xides with -Y bond is ionic. => forming basic solution in water. Ex), Ca Ca(s) + (l) Ca() (aq) (s) + (l) (aq) - (aq) + (l) - (aq) oxide ion has high affinity for proton.
41 Lewis Acid-Base odel Definitions Acid Base Arrhenius + producer - producer Brønsted-Lowry + donor + acceptor Lewis e - pair acceptor e - pair donor Brønsted-Lowry Lewis base acid acid base acid base A Brønsted-Lowry acid must contain at least one ionizable proton!
42 Lewis Acid-Base odel Al Al( ) 6 3+ BF 3 + N 3 BF 3 N 3 Lewis acid Lewis base Lewis acid Lewis base S 3 (g) + (l) S (aq) (S) Lewis acid () Lewis base ()Lewis base () Lewis acid Bronsted-Lowry acid S S A Brønsted-Lowry acid must contain at least one ionizable proton! A Lewis acid doesn't require it!
43 Solving Acid-Base Problems: Summary Don't memorize. ain questions are ajor species? What is their chemical behavior?
Chapter 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 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 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 informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationChapter 14. Acids and Bases
Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton
More informationAdvanced Placement Chemistry Chapters Syllabus
As you work through the chapter, you should be able to: Advanced Placement Chemistry Chapters 14 16 Syllabus Chapter 14 Acids and Bases 1. Describe acid and bases using the Bronsted-Lowry, Arrhenius, and
More informationADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA
ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while
More informationChemistry: The Central Science. Chapter 16: Acid-Base Equilibria. 16.1: Acids and Bases: A Brief Review
Chemistry: The Central Science Chapter 16: Acid-Base Equilibria 16.1: Acids and Bases: A Brief Review Acids have a sour taste and cause certain dyes to change color Base have a bitter taste and feel slippery
More informationChapter 7 Acids and Bases
Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationProperties of Acids. Base Chemistry. Properties of Bases. Three Acid and Base Theories. 1) Arrhenius Theory. May 09, Naming Acids Review
May 09, 2013 Properties of Acids AcidAcid Base Chemistry Base Chemistry Taste sour Are strong or weak electrolytes React with bases to form water and salts React with active metals to produce H2 Turn litmus
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases 14.1 The Nature of Acids and Bases Bronsted-Lowry Acid-Base Systems Bronsted acid: proton donor Bronsted base: proton acceptor Bronsted acid base reaction: proton transfer from
More informationAcids and Bases. Chapters 20 and 21
Acids and Bases Chapters 20 and 21 Acid and Bases Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with
More informationWhat we learn from Chap 17
Acids and Bases hapter 17 What we learn from hap 17 17.2 This chapter concerns the nature and uses of acids and bases. It is the second in our three-chapter h discussion i about equilibrium, and reinforces
More informationChapter 16. Acid-Base Equilibria
Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An
More informationCu 2+ (aq) + 4NH 3(aq) = Cu(NH 3) 4 2+ (aq) I (aq) + I 2(aq) = I 3 (aq) Fe 3+ (aq) + 6H 2O(l) = Fe(H 2O) 6 3+ (aq) Strong acids
There are three definitions for acids and bases we will need to understand. Arrhenius Concept: an acid supplies H + to an aqueous solution. A base supplies OH to an aqueous solution. This is the oldest
More informationAcid/Base Theories The common characteristics of acids
Acid/Base Theories The common characteristics of acids describe them as: Acids aving a sour taste Being electrolytes (some weak) Reacting with metals to produce gas (usually 2 ) Reacting with bases to
More informationAcids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
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 informationWednesday, February 25, Acid and Base Reactions
Acid and Base Reactions Dilute aqueous solution of acetic acid, C3COO Aqueous solution of sodium hydroxide, NaO The role of the ydrogen Ion Cl (aq) Æ + (aq) + Cl - (aq) What does the neutral atom consist
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many
More informationAcid Dissociation Constant
CE 131 Lecture 37 Lewis Acids and Bases Chapter 16: pp. 800-802. Acid Dissociation Constant C 2 3 2 + 2 3 + + C 2 3-2 [ 3 + ][C 2 3-2 ] K = [ 2 ][C 2 3 2 ] [ 3 + ][C 2 3-2 ] K a = K [ 2 ] = [C 2 3 2 ]
More informationLecture Presentation. Chapter 16. Acid Base Equilibria. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 16 Acid Base Equilibria John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius An acid is a substance that, when dissolved in water, increases
More 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 information[H + ] OH - Base contains more OH - than H + [OH - ] Neutral solutions contain equal amounts of OH - and H + Self-ionization of Water
19.1 Acids & Bases 1. Compare and contrast the properties of acids & bases. 2. Describe the self-ionization of water & the concept of K w. 3. Differentiate between the Arhennius & Bronsted-Lowry models
More informationCHAPTER 14 THE CHEMISTRY OF ACIDS AND BASES
CHAPTER 14 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 informationChapter 16. Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius
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 15. Properties of Acids. Structure of Acids 7/3/08. Acid and Bases
Chapter 15 Acid and Bases Properties of Acids! Sour taste! React with active metals! React with carbonates, producing CO 2! Change color of vegetable dyes!blue litmus turns red! React with bases to form
More informationAcids and Bases. Reading Assignments: Acids. Bases. Chapter 15 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005
Reading Assignments: Chapter 15 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Or Related topics in other textbooks. Acids and Bases Consultation outside lecture room: Office Hours: Tuesday & Thursday
More informationChapter 6. Acids, Bases, and Acid-Base Reactions
Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
More informationAspects of Bonding & Acid Strength
Aspects of Bonding & Acid Strength CHEM 110/ 2014 Slide 1 of 35 Intramolecular Bonding The bonding between molecules/atoms in the solid state Ionic bonding Covalent bonding Metallic bonding e.g. sodium
More informationAcids Bases and Salts Acid
Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic
More information1 Chapter 19 Acids, Bases, and Salts
1 Chapter 19 Acids, Bases, and Salts ACID-BASE THEORIES Acids and bases are all around us and part of our everyday life (ex. bodily functions, vinegar, carbonated drinks, citrus fruits, car batteries,
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 informationChapter 16: Acids and Bases I. Chem 102 Dr. Eloranta
Chapter 16: Acids and Bases I Chem 102 Dr. Eloranta Acids and Bases Acids Sour taste (vinegar) Dissolve many metals Ability to neutralize bases Strong or Weak Bases Bitter taste (caffeine, poisons from
More informationChapter 16: Acid Base Equilibria Chapter 16 Acid-Base Equilibria Learning Standards & Objectives;
Chapter 16: Acid Base Equilibria Chapter 16 Acid-Base Equilibria Learning Standards & Objectives; Chapter 16 AP16-1,2-01 AP16-1,2-02 AP16-1,2-03 AP16-3,4-01 AP16-3,4-02 AP16-5-01 AP16-6,7-01 AP16-6,7-02
More informationLecture 7. Acids. non-metals form anions. metals form cations H+ - Professor Hicks Inorganic Chemistry (CHE152) + anion. molecular compounds
Lecture 7 Professor icks Inorganic Chemistry (CE152) Acids + + anion + - anion substances that release + ions when dissolved Strong acids Cl NO 3 2 SO 4 + Cl - + NO - 3 2 + SO 2-4 hydrochloric acid nitric
More informationAqueous Equilibria: Acids and Bases
/3/014 Aqueous Equilibria: Acids and Bases Ch. 16 What is an? What is a? There are actually multiple definitions Arrhenius: Dealt with species in aqueous solutions. Most basic definition of acis. Acid:
More informationChapter 16. Dr Ayman Nafady
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 Dr Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions
More informationContents and Concepts
Learning Objectives Chapter 15 Acid Base Concepts Arrhenius Concept of Acids and Base a. Define and according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define and according
More informationChapter 16 Acid Base Equilibria
Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar
More informationACIDS AND BASES. Note: For most of the acid-base reactions, we will be using the Bronsted-Lowry definitions.
DEFINITIONS: ACIDS AND BASES Arrhenius Definition An acid in aqueous solution produces H + ions. A base in aqueous solution produces OH - ions. Bronsted Lowry Theory An acid is a proton donor A base is
More informationHA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H
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 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 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 informationUnit 12: Acids & Bases. Aim: What are the definitions and properties of an acid and a base? Properties of an Acid. Taste Sour.
Unit 12: Acids & Bases Aim: What are the definitions and properties of an acid and a base? Mar 23 12:08 PM Properties of an Acid 3. Are electrolytes. (Dissociate and conduct electricity when aq) 2. Turns
More informationReactions in Aqueous Solutions I: Acids, Bases & Salts
10 Reactions in Aqueous Solutions I: Acids, Bases & Salts CHAPTER GOALS 1. Properties of Aqueous Solutions of Acids and Bases 2. The Arrhenius Theory 3. The Hydronium Ion (Hydrated Hydrogen Ion) 4. The
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin
Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Acids and Bases Properties of Acids An acid is any substance that releases hydrogen ions, H +, into water.
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationWeak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
More information20 ACIDS AND BASES Standard Curriculum
20 ACIDS AND BASES Standard Curriculum Conceptual Curriculum Concrete concepts More abstract concepts or math/problem-solving Core content Extension topics Honors Curriculum Core honors content Options
More informationUNIT #11: Acids and Bases ph and poh Neutralization Reactions Oxidation and Reduction
NAME: UNIT #11: Acids and Bases ph and poh Neutralization Reactions Oxidation and Reduction 1. SELF-IONIZATION OF WATER a) Water molecules collide, causing a very small number to ionize in a reversible
More informationChapter Menu Chapter Menu
Chapter Menu Chapter Menu Section 18.1 Section 18.3 Section 18.4 Introduction to Acids and Bases Hydrogen Ions and ph Neutralization Section 18.1 Intro to Acids and Bases Objectives: Compare the Arrhenius,
More informationA is capable of donating one or more H+
Slide 1 / 48 1 According to the Arrhenius concept, an acid is a substance that. A is capable of donating one or more H+ B C D E causes an increase in the concentration of H+ in aqueous solutions can accept
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 informationTalk n Acids & Bases... Lady Dog! Definitions
Talk n Acids & Bases... Lady Dog! Definitions So far in this course, we have looked at processes in chemistry that deal with, or are best explained by, ionic salts or molecules. Now we will turn our attention
More informationPart One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow
CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many
More information11/15/11. Chapter 16. HA(aq) + H 2 O(l) H 3 O + (aq) + A (aq) acid base conjugate conjugate
Chapter 16 Table of Contents Chapter 16 16.1 16.2 16.3 16.4 16.5 16.6 Buffered Solutions Copyright Cengage Learning. All rights reserved 2 Models of Arrhenius: Acids produce H + ions in solution, bases
More informationWhat are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced
What are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced materials? Historically, classified by their observable
More informationg. Looking at the equation, one can conclude that H 2 O has accepted a proton from HONH 3 HONH 3
Chapter 14 Acids and Bases I. Bronsted Lowry Acids and Bases a. According to Brønsted- Lowry, an acid is a proton donor and a base is a proton acceptor. Therefore, in an acid- base reaction, a proton (H
More informationAcids and Bases. Feb 28 4:40 PM
Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to
More information11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1
11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing
More informationChapter Outline. Ch 8: Aqueous Solutions: Chemistry of the Hydrosphere. H 2 S + Cu 2+ CuS(s) + 2H + (Fe, Ni, Mn also) HS O 2 HSO 4
Ch 8: Aqueous Solutions: Chemistry of the Hydrosphere H 2 S + Cu 2+ CuS(s) + 2H + (Fe, Ni, Mn also) HS - + 2 O 2 HSO 4 - + energy (supports life) Figure taken from Principles of Biochemistry, 2nd Ed. By
More informationAP Chemistry CHAPTER 16 STUDY GUIDE Acid-Base Equilibrium
AP Chemistry CHAPTER 16 STUDY GUIDE AcidBase Equilibrium 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept
More informationChemistry 201: General Chemistry II - Lecture
Chemistry 201: General Chemistry II - Lecture Dr. Namphol Sinkaset Chapter 17 Study Guide Concepts 1. There are multiple definitions for acids and bases. 2. An Arrhenius acid is a substance that produces
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 informationChapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1
Chapter 16 Acids and Bases Copyright Cengage Learning. All rights reserved 1 Section 16.1 Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH ions.
More informationReactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
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 2: Acids and Bases
hapter 2: Acids and Bases 32 hapter 2: Acids and Bases Problems 2.1 Write each acid- reaction as a proton-transfer reaction. Label which reactant is the acid and which the, as well as which product is
More informationCHAPTER 18 ACID-BASE EQUILIBRIA
CAPTER 18 ACID-BASE EQUILIBRIA FOLLOW UP PROBLEMS 18.1A Plan: Examine the formulas and classify each as an acid or base. Strong acids are the hydrohalic acids Cl, Br, and I, and oxoacids in which the number
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 informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
More informationCHAPTER 17: ACIDS AND BASES
INTRODUCTION CHAPTER 17: ACIDS AND BASES In this chapter you will learn about the properties of acids and bases. You know about some of the properties of acids already. Substances such as lemon juice and
More informationWhat is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
More informationObjectives. Base Chemistry
May 09, 2014 Objectives AcidAcid Base Chemistry Base Chemistry Chapter 19 Properties of Acids Aqueous solutions of acids taste sour. Change the color of acid/base indicators Many will conduct electrical
More 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 informationEXPERIMENT 11 Acids, Bases, and ph
EXPERIMENT 11 Acids, Bases, and ph INTRODUCTION The concept of acidity and alkalinity dates from ancient times. The word acid is derived from the Latin word acidus, meaning sour. A common acid, acetic
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationAcids and Bases. Properties, Reactions, ph, and Titration
Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some
More informationAcid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated.
Physical Properties Acid and Bases Chemistry 30 Acids Corrosive when concentrated Have a sour taste Bases Corrosive when concentrated Have a bitter taste Often have a sharp odour Chemical Properties Indicators
More informationChapter 16 Acids and Bases. Chapter 16 Acids and Bases
. Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases
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 informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
More informationAcid-base Chemistry. Unit 11.1: Into to acid base chemistry. Unit 11. Name:
Name: Acid-base Chemistry Unit 11 ( F i ve cla s s peri o ds) Unit 11.1: Into to acid base chemistry 1) Self-ionization of water a) Water molecules collide and the extremely electronegative oxygen can
More informationChemistry SAT II Review Page 1
Chemistry SAT II Review Page 1 Acids and Bases Properties of acids and bases are caused by ions 1. Hydronium ions (H 3 O + ) cause acid properties 2. Hydroxide ions (OH ) cause base properties Water -
More informationEquations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14
Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More informationAcids and Bases. CHEM 102 T. Hughbanks. In following equilibrium, will reactants or products be favored? Strong acid (HCl) + Strong base (NaOH)
Acids and Bases According to the Brønsted Lowry theory, all acid base reactions can be written as equilibria involving the acid and base and their conjugates. CEM 102 T. ughbanks All proton transfer reactions
More informationChemistry 102 Chapter 15 ACID-BASE CONCEPTS
General Properties: ACID-BASE CONCEPTS ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink Neutralization
More informationAP*Chemistry The Chemistry of Acids and Bases
Dr. Valverde s AP Chemistry Class Chapters 14 and 15 Review: Acids and Bases AP*Chemistry The Chemistry of Acids and Bases "ACID"--Latin word acidus, meaning sour. (lemon) "ALKALI"--Arabic word for the
More informationUnit 24 Acids and Bases (Chapter 7)
Unit 24 Acids and Bases (Chapter 7) Properties of Acids and Bases (7.1) Theories of Acids and Bases (7.2) Arrhenius Theory Brønsted-Lowry Theory Salts (7.2) Acidic and Basic Anhydrides (7.3) Properties
More informationChapter In each case the conjugate base is obtained by removing a proton from the acid: (a) OH (b) I (c)
Practice Exercises 16.1 Conjugate acid base pairs (a), (c), and (f) (b) The conjugate base of I is I (d) The conjugate base of N 2 is N 2 and the conjugate base of N 4 is N 3 (e) The conjugate acid of
More informationACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY
ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationAqueous Equilibria, Part 1 AP Chemistry Lecture Outline
Aqueous Equilibria, Part 1 AP Chemistry Lecture Outline Name: Acids and Bases Arrhenius...acids increase the when dissolved in H 2 O....bases increase the when dissolved in H 2 O. e.g., HCl and NaOH Bronsted-Lowry
More informationDefinition Arrhenius ( ) acid and base (1887) Acid A molecule ionizes in water to form a solution
1 Acids and bases Definition Arrhenius (1859-197) acid and base (1887) Acid A molecule ionizes in water to form a solution containing H ions Base A molecule ionizes in water to form a solution containing
More information