Chap 10-Acids & Bases
5/20/15Chapter 10Acids & Bases1CHAPTER OUTLINE § § § § § § General PropertiesArrhenius Acids & BasesBrønsted-Lowery Acids & BasesStrength of Acids & BasesIonization of WaterpH Scale21
5/20/15GENRAL PROPERTIES OF ACIDS & BASES q Many common substances in our daily lives areacids and bases.q Oranges, lemons and vinegar are examples ofacids. In addition, our stomachs contain acidsthat help digest foods.q Antacid tablets taken for heartburn andammonia cleaning solutions are examples ofbases.3GENRAL PROPERTIES OF ACIDS & BASES q General properties associated with acids includethe following:Ø sour tasteØ change color of litmus from blue to redØ react with metals to produce H2 gasØ react with bases to produce salt & water42
5/20/15GENRAL PROPERTIES OF ACIDS & BASES q General properties associated with bases includethe following:Ø bitter tasteØ slippery, soapy feelingØ change color of litmus from red to blueØ react with acids to produce salt & water5ARRHENIUS ACIDS & BASES Accordingq The mostto thecommonArrheniusdefinitiondefinition,of acids and baseswas formulatedby theSwedishchemistSvanteionsq Acidsare substancesthatproducehydronium Arrheniusin 1884.(H3O ) in aqueous solution.HCl (g) H2O (l)H3O (aq) Cl– (aq)Commonly written asHCl (g)H2OH (aq) Cl– (aq)63
5/20/15ARRHENIUS ACIDS & BASES According to the Arrhenius definition,q Bases are substances that produce hydroxide ion(OH-) in aqueous solution.NaOH (s)H2ONH3 (aq) H2O (l)Na (aq) OH– (aq)NH4 (aq) OH – (aq)7BRØNSTED-LOWRY ACIDS & BASES q TheAccordingArrheniusto Brønsted-Lowrydefinition of acidsdefinition,and basesanislimitedacidis atoprotonaqueousdonor,solutions.and a base is a protonA substance that can act as a Brønsted-Lowry acidacceptor.q baseA broaderdefinitionacids amphiprotic.and bases wasand(such aswater) isofcalleddeveloped by Brønsted and Lowry in the early20th century.BaseAcidAcidBaseNHHCl(g) H2O (l) NHH3O4 (aq) OHCl– –(aq)(aq)3 (aq)84
5/20/15BRØNSTED-LOWRY ACIDS & BASES q In Brønsted-Lowry definition, any pair ofmolecules or ions that can be inter-convertedby transfer of a proton is called conjugateacid-base pair.HCl (g) H2O (l) H3O (aq) Cl– OWRY ACIDS & BASES NH3 (aq) H2O (l) NH4 (aq) OH– (aq)BaseAcidConjugateacidConjugatebase105
5/20/15Example 1: Identify the conjugate acid-base pairs for eachreaction shown below:H2O AcidCl! HCl OH!BaseConjugateacidConjugatebase11Example 1: Identify the conjugate acid-base pairs for eachreaction shown below:C6H5OH C2H5O! C6H5O! C2H5OHAcidBaseConjugatebaseConjugateacid126
5/20/15Example 2: Write the formula for the conjugate acid for eachbase shown:HS H H2S!NH3 H NH4 CO32! H HCO3!13Example 3: Write the formula for the conjugate base for eachacid shown:HI - H I!CH3OH - H CH3O!HNO3 - H NO3!147
5/20/15ACID & BASE STRENGTH q AccordingStrong acidsto andthe Arrheniusbases are thosedefinition,that ionizethestrengthcompletelyof acidsin water.and bases is based on theof theirwater.electrolytes.q amountStrong acidsandionizationbases areinstrongH 2ONaOH(s) ææææNa (aq)(aq) ClOH(aq)HCl (aq)æÆ H(aq)1001M1001M1001M15ACID & BASE STRENGTH q Weak acids and bases are those that ionizepartially in water.q Weak acids and bases are weak electrolytes.H 2O ææÆHCHOH(aq) C2 H 3 OOHæÆ ææNH(aq) HO(l)NH(aq)2322 (aq) ææ324 (aq)1001M 1 0.01M 1 0.01M168
5/20/15IONIZATION OF STRONG vs. WEAK ACIDS IonizescompletelyIonizespartially17COMMON ACIDS Strong AcidsWeak AcidsHClHydrochloric acidHC2H3O2Acetic acidHBrHydrobromic acidH2CO3Carbonic acidHIHydroiodic acidH3PO4Phosphoric acidHNO3Nitric acidHFHydrofluoric acidH2SO4Sulfuric acidHCNHydrocyanic acidH2SHydrosulfuric acid189
5/20/15COMMON BASES Strong BasesWeak BasesLiOHLithium hydroxideNH3AmmoniaNaOHSodium hydroxideCO(NH2)2UreaCa(OH)2Calcium hydroxideKOHPotassium hydroxideBa(OH)2Barium hydroxide19COMPARISON OF ACIDS & BASES 2010
5/20/15IONIZATION OF WATER q Water can act both as an acid and a base.q In pure water, one water molecule donates aproton to another water molecule to produceions.H2OAcid H2O BaseH3O Conjugateacid OH–Conjugatebase21IONIZATION OF WATER andOHq nsthe transferhaveofofHH3protonsObetweenOH– –ions.are3O andwatermoleculestogether,producesthe ion-productequal numbersconstantq multipliedAn increasein theconcentrationof oneof ofthe –H(KO)isandformed.OHions.ions3w will cause an equilibrium shift that causesq aThenumberproduceddecreasein oftheionsotherone. in pure water isvery small, as indicated below:[H3O ] [OH–] 1.0 x 10-7 MKw [H3O ][OH–] [1.0x10-7][1.0x10-7] 1.0x10-142211
5/20/15ACIDIC & BASIC SOLUTIONS q When [H3O ] isandgreater[OH–]thanare equal[OH–]ininaasolution, it is acidic.neutral.q For example, if [H3O ] is 1.0 x 10–4 M, then[OH–] would be 1.0 x 10–10 M.Kw1.0 x 10[OH ] [H 3O ] 1.0 x 10144 1.0 x 1010M23ACIDIC & BASIC SOLUTIONS q When [OH-] is greater than [H3O ] in asolution, it is basic.q For example, if [OH-] is 1.0 x 10–6 M, then[H3O ] would be 1.0 x 10–8 M.-14Kw1.0x10-8[H 3O ] 1.0x10M[OH ] 1.0 x 10-6 2412
5/20/15ACIDIC & BASIC SOLUTIONS BasicAcidicNeutral[H3O ] [OH-][H3O ] [OH-][H3O ] [OH-]25Example 1: Calculate the [OH–] in a solution with [H3O ] 2.3x10–4 M.Classify the solution as acid or basic.[OH-] Kw1.0x10-14 4.3x10-11 -4[H3O ]2.3x10Solutionis acidic[H3O ] 1.0x10-7[OH-] 1.0x10-72613
5/20/15Example 2: Calculate the [H3O ] in a solution with [OH-] 3.8x10–6 M.Classify the solution as acid or basic.[H3O ] Kw1.0x10-14 2.6x10-9 -6[OH ]3.8x10Solutionis basic[OH-] 1.0x10-7[H3O ] 1.0x10-727Example 3: Calculate the [OH–] in a solution with [H3O ] 5.8x10–8 M.Classify the solution as acid or basic.[OH-] Kw1.0x10-14 1.7x10-7 -8[H3O ]5.8x10Solutionis basic[H3O ] 1.0x10-7[OH-] 1.0x10-72814
5/20/15Example 4: Calculate the [H3O ] in a solution with [OH-] 1.3x10–2 M.Classify the solution as acid or basic.[H3O ] Kw1.0x10-14 7.7x10-13 -2[OH ]1.3x10Solutionis basic[OH-] 1.0x10-7[H3O ] 1.0x10-729pH SCALE q The acidity of a solution is commonlymeasured on a pH scale.q The pH scale ranges from 0-14, where acidicsolutions are less than 7 and basic solutionsare greater than 7.pH -log [H3O ]3015
5/20/15pH SCALE Acidic solutionspH 7H3O 1x10-7Neutral solutionspH 7H3O 1x10-7Basic solutionspH 7H3O 1x10-731Example 1: The [H3O ] of a liquid detergent is 1.4x10–9 M.Calculate its pH.Solutionis basicpH -log [H3O ] -log [1.4x10-9] -(-8.85)pH 8.852 significantfiguresThe number of decimal places in a logarithm is equal tothe number of significant figures in the measurement.3216
5/20/15Example 2: The pH of black coffee is 5.3. Calculate its[H3O ]. Solutionis acidic[H3O ] antilog (-pH) 10 –pH 10 -5.3[H3O ] 5 x 10-61 significantfigure33Example 3: The [H3O ] of a solution is 3.5 x 10–3 M. Calculateits pH.Solutionis acidicpH -log [H3O ] -log [3.5x10-3] -(-2.46)pH 2.462 significantfigures3417
5/20/15Example 4: The pH of tomato juice is 4.1. Calculate its[H3O ].Solutionis acidic[H3O ] antilog (-pH) 10 –pH 10 -4.1[H3O ] 8 x 10-51 significantfigure35Example 5: The [OH!] of a cleaning solution is 1.0 x 10!5 M.What is the pH of this solution?2 sigfigs–]Kw [H3O ][OHSolutionis basic[H3O ] Kw 1.0 x 10 [OH ] 1.0 x 10pH !log[H3O ]145 1.0 x 10!9 M 9.00!9!log(1.0x10 )3618
5/20/15Example 6: The pH of a solution is 11.50. Calculate the[H3O ]Solutionfor this solution.is basic[H3O ] antilog (-pH) 10 –pH 10 -11.50[H3O ] 3.2 x 10-1237THE END3819
5/20/15 2 3 GENRAL PROPERTIES! OF 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 taken for
2. Describe the common properties of acids and bases 3. Identify acids and bases using indicators, pH papers 4. Name some common lab acids and bases, acids at and bases at home 5. Describe reactions of acids with metals, bases and carbonates 6. Describe the application of acids, bases and p
Preparing the living compartment (inside)P.4 Chap. III CArrYInG PASSEnGErS P.5 Chap. IV LoADS AnD LoADED wEIGHt P.6 Chap. V wInDowS AnD SKYLIGHtS P.8 Chap. VI DrIVInG P. 10 Chap. VII tYrES P.11 Chap. VIII SIGnALInG, lights P.12 Chap. IX PArKInG mAnEuVErS P. 14 Chap. X tHE CAmPEr DrIVEr'S CHArtEr P. 16 Chap. XI oPErAtIon oF APPLIAnCES P.17
_7. Which statement describes an alternate theory of acids and bases? (1) Acids and bases are both H acceptors. (2) Acids and bases are both H donors. (3) Acids are H acceptors, and bases are H donors. (4) Acids are H donors, and bases are H acceptors. _8. Which substance is the
Properties of Acids and Bases Return to the Table of contents Slide 5 / 208 What is an Acid? Acids release hydrogen ions into solutions Acids neutralize bases in a neutralization reaction. Acids corrode active metals. Acids turn blue litmus to red. Acids taste sour. Properties of Acids Slide 6 / 208 Properties
Acids, Bases, and pH The hydrohalic acids (HX (aq)), where X represents a halogen) include HF, HCl, HBr, and HI. Only HF is a weak acid. The rest are strong acids. What factors account for this difference? 8.1 Explaining the Properties of Acids and Bases 8.2 The Equilibrium of Weak Acids and Bases 8.3
Unit 11 Objectives: Acids & Bases Acid-Base Nomenclature Content Objectives: I can name ionic compounds containing acids, and bases, using (IUPAC) nomenclature rules. I can write the chemical formulas of acids and bases. Criteria for Success: I can identify an acid as a binary acid or an oxyacid. I can name common binary acids, oxyacids, and bases given their chemical formula.
Unit 14 – Acids & Bases 1 Worksheets - Honors BRONSTED - LOWRY ACIDS & BASES WORKSHEET According to Bronsted-Lowry theory, an acid is a proton (H 1) donor, and a base is a proton acceptor. Label the Bronsted-Lowry acids (A), bases (B), conjugate acids (CA), and conjugate bases (CB) in the
properties of acids and bases. 5. Describe the colors that form in acidic and basic solutions with litmus paper and phenolphthalein. 6. Explain the difference between strong acids or bases and weak acids or bases. 7. Memorize the strong acids and bases. 8. Define the terms polyprotic and amphiprotic. 9. Perform calculations using the following .
