Acids And Bases - NJCTL

Slide 32 / 208Slide 33 / 208Acid and Base StrengthAcidH 3 O (aq) Cl- (aq)conj. acidconj. baseAcid strength increasesConversely, HCl is a muchstronger acid than thehydronium ion, soequilibrium lies very far tothe rightNegligibleWeakAn alternative way to consider equilibrium isthat it will favor thereaction AWAY from the stronger acid.K 1Slide 34 / 208CH3 COOH (aq) H2 O (l)NegligibleSlide 36 / 208Acetic acid is a weak acid. This means that only a smallpercent of the acid will dissociate.The double headed arrow is used only in weak acid orweak base dissociation equations.CH3 COOH (aq) H2 O (l)H 3 O (aq) CH3 COO- (aq)A single arrow is used for strong acid or strong baseswhich dissociate completely.NaOHNa (aq) OH- 33PO4OHO2HCH3-Base strength increasesAcid strength increasesWeakIf you look for the stronger If you look for the strongerbase:acid:BaseStrongNegligibleDoes equilibrium lie to the left (K 1) or to the right (K 1)?HClH2SO4HNO3H3O HSO4H3PO4HFHC2H3O2H2CO3H 2SH2PO4 NH4HCO32HPO4H 2OOHH2CH4Weak100%ionizedin H2OH 3 O (aq) CH3 COO- (aq)Since the hydroniumion is a stronger acidthan acetic acid,equilibrium lies to theleft (K 1).StrongAcidH 3 O (aq) CH3 COO- (aq)Acid and Base Strength100%protonatedin H2OAcid and Base StrengthConsider this equilibrium between acetic acid and acetate ion:Equilib lies away from the Equilib favors this baseaccepting a proton.stronger O3PO43OHO2HCH3-Slide 35 / 208Acid and Base StrengthCH3 COOH (aq) H2 O (l)BaseBase strength increasesIn this example, H 2 O is amuch stronger base thanCl-, so the proton movesfrom HCl to H 2 OHClH2SO4HNO3H3O HSO4H3PO4HFHC2H3O2H2CO3H 2SH2PO4 NH4HCO3HPO42H 2OOHH2CH4Negligible100%ionizedin H2OStrongIn other words, a stronger base will "hold onto" its proton whereasa strong acid easily releases its proton(s).HCl (aq) H2 O (l)acidbaseH 3 O (aq) Cl- (aq)conj. acidconj. baseWeakHCl (aq) H2 O (l)acidbaseIn any acid-base reaction, equilibriumwill favor the reaction inwhich the proton moves toward the stronger base.100%protonatedin H2OSlide 37 / 20812 Strong acids have Acid and Base Strength

Slide 37 (Answer) / 208Slide 38 / 20813 HBr, hydrobromic acid is a strong acid. This meansthat it .AAnswer12 Strong acids have conjugatebases.strongBweakCneutralDnegativeAB[This object is a pulltab]aqueous solutions of HBr contain equalconcentrations of H and OH-Bdoes not dissociate at all when it is dissolved inwaterCcannot be neutralized by a baseDdissociates completely to H and Br- when itdissolves in waterSlide 38 (Answer) / 208Slide 39 / 20814 For the following reaction, determine which sideof the equilibrium is favored.13 HBr, hydrobromic acid is a strong acid. This meansthat it .H3PO4 H2O H2PO4- H3O dissociates completely to H and Br when itdissolves in waterCNeither side is favored-Slide 39 (Answer) / 20815 For the following reaction, determine which sideof the equilibrium is favored.H3 O HSO4 - H2 O H2 SO4100%protonatedin H2OBthe left sideCNeither side is favored100%ionizedin H2OHClH2SO4HNO3H3O HSO4H3PO4HFHC2H3O2H2CO3H 2SH2PO4NH4 HCO3HPO42H O4NH32CO3PO43OHO2HCH3Base strength increasesthe right sideAcid strength increasesWeakAnswerBase strength increasesStrongNegligibleAcid strength increasesWeakNeither side is favoredStrongCAcidANegligiblethe left side100%Cl- is theequilibriumHClthat is favoredionizedH2SOHSO4side wherethe4 strongerbasein H2OHNO3 the proton.NO3has accepted H 3OH2O2HSO4SO4H3PO4H2PO4HF object is a pullF[Thistab]HC2H3O2C2H3O2H2CO3HCO3H 2SHSH2PO4HPO42NH4 NH3HCO3CO3223HPO4PO4H 2OOH2OHOH2HCH4CH3WeakBH2PO4 is Acida stronger baseBasethanH2O and the side of the-StrongNegligibleB H3PO4 H2O HThe2PO4 H3Oleft side is favored becausethe right side100%protonatedin H2OSlide 40 / 20814 For the following reaction, determine which sideof the equilibrium is H32CO33PO4OH2OHCH3Weak the left sideBaseBase strength increasesDBAcid strength increasescannot be neutralized by a basethe right sideNegligibletab]CAWeakdoes not dissociate at all when it is dissolved inwater[This object is a pullHClH2SO4HNO3 H 3OHSO4H3PO4HFHC2H3O2H2CO3H 2SH2PO4NH4 HCO32HPO4H 2OOHH2CH4StrongNegligibleAnswerAcid100%ionizedin H2OWeakBaqueous solutions of HBr contain equalD- acids and basesStrongconcentrations of H and OHdissociate completely.100%protonatedin H2OStrongANegligible

Slide 40 (Answer) / 208Slide 41 / 20816 For the following reaction, determine which sideof the equilibrium is favored.Neither side isBase strength increasesStrongNegligibleAcid strength 4NH4 HCO3HPO42H 2OOHH2CH4Bthe left sideCNeither side is favoredWeakHC2H3O2H2CO3Weak[This object is a pulltab] H2S -the right side100%ionizedin H2O100%protonatedin H2ONegligibleSlide 41 (Answer) / 208Acid strength increasesCAnswerthe left sideAcidANegligibleBBaseA100%Theright side HClis favored becauseClionizedHHSO4H2O is a stronger2SO4 base thanin H2ONO3HSOthe 3side of the4 andHNOH 3O2Oequilibrium thatis favoredisHthe2HSOSO44side where redHFF-Weakthe right sideHClH2SO4HNO3H3O HSO4H3PO4HFHC2H3O2H2CO3H 2SH2PO4 NH4HCO3HPO42H PO4NH32CO3PO43OHO2HCH3-StrongNegligibleAcidAH3O NO3Base strength increasesHNO3 H2OWeakH3 O HSO4 - H2 O H2 SO4100%protonatedin H2OSlide 42 / 20816 For the following reaction, determine which sideof the equilibrium is favored.Acid ABaseThe right side is favored becausethe right sideBthe left sideCNeither side is favoredStrongNegligibleAcid strength increases100%HCl base thanCl NO3H2O is a strongerionizedH2SOHSO4of 4the equilibriumin andH2O the sideHNO3NO3that is favored is the side whereH 3OH2O- has acceptedthe C2H3O2[Thisobjectis a pullH2COHCO33tab]H 2SHS2H2PO4HPO4 NH4NH32HCO3CO3HPO42PO43H 2OOHOHO2H2HCH4CH3-WeakWeakAnswerABase strength increasesH3O NO3-Amphoteric SubstancesStrongHNO3 H2OReturn to the Tableof Contents100%protonatedin H2ONegligibleSlide 43 / 208Slide 44 / 208Amphoteric SubstancesAmphoteric SubstancesIf a substance can act both as an acid and base, it is knownas amphoteric. For example, water can act as a base oracid depending on the situation.Another term for amphoteric is amphiprotic.For each of the following substances, write two equations,one showing it as a Bronsted-Lowry acid and anothershowing it as a Bronsted-Lowry base.HCl H2OCl- H3O Above, water accepts a proton, thus acting as a base.NH3 H2OHCO3 -NH4 OH -Above, water donates a proton, thus acting as an acid.HSO4 -H2 OStrong15 For the following reaction, determine which sideof the equilibrium is favored.

Slide 45 / 208A substance that is capable of acting as both an acidand as a base is .17A substance that is capable of acting as both an acidand as a base is bleSlide 46 / 208Answer17Slide 45 (Answer) / 208C[This object is a pulltab]Slide 47 / 20818 Write the equations and equilibrium expressions for HSwhen it is acting like a Brønsted-Lowry acid and when itStudents type their answers hereis actinglike a Brønsted-Lowry base.Strong Acids and BasesReturn to the Table ofContentsSlide 48 / 208Strong AcidsRecall, strong acids completely ionize in solution.The seven strong acids chloric acidhydrobromic acidhydroiodic acidnitric acidsulfuric acidchloric acidperchloric acidMemorize this list.Slide 49 / 208Strong AcidsThe seven strong acids are strong electrolytes because they are100% ionized. In other words, these compounds exist totally as ionsin aqueous solution.For the monoprotic strong acids (acids that donates only one protonper molecule of the acid), the hydronium ion concentration equals theacid concentration.[Acid] [H3O ]So, if you have a solution of 0.5 M HCl, then [H3O ] 0.5 M

Slide 50 / 208Strong BasesAll strong bases are group of compounds called "metal hydroxides."Slide 51 / 20819 What is the hydroxide ion concentration of a0.22 M calcium hydroxide solution?A0.11B0.22Only the heavier alkaline earth metals in Group II form strongbases: Ca(OH)2, Sr(OH) 2, and Ba(OH)2.C0.44D0.88Again, these substances dissociate completely in aqueoussolution. In other words, NaOH exists entirely as Na ions and OHions in water.ENot enough information.All alkali metals in Group I form hydroxides that are strongbases: LiOH, NaOH, KOH, etc.Slide 51 (Answer) / 20819 What is the hydroxide ion concentration of a0.22 M calcium hydroxide solution?0.11B0.22C0.44D0.88ENot enoughAnswerASlide 52 / 20820 What is the concentration of H in a 25ml solution of0.05M HCl when diluted to final volume of 100ml?CCalcium hydroxide's formula isCa(OH)2. For every 1 mole ofCa(OH)2 there are 2 moles of OH-.If you have a 0.22M solution ofCa(OH)2 then the concentration ofOH- is 2x as much or 0.44M.information.[This object is a pulltab]Slide 52 (Answer) / 208Answer20 What is the concentration of H in a 25ml solution of0.05M HCl when diluted to final volume of 100ml?To determine the new concentrationyou can use the formula M1V1 M2V2M1 .05M, V1 25 ml and V2 100 mlM2 M1V1/V2M2 .05M x 25 ml /100 mlM2 0.0125M HClThe concentration of H equals theconcentration of the HCl solution andtherefore equals 0.0125M.[This object is a pulltab]Slide 53 / 20821 What is the [H ] ion concentration of a 50 ml solutionof 0.025M H2 SO4 , when diluted with 150 ml of water?

Slide 53 (Answer) / 208Using M1V1 M2V2. You are given:M1 0.025M, V1 50 ml and V2 100 ml.M2 M1V1/V2M2 0.025M x 50 ml/100 mlM2 0.0125MFor every 1 mole of H2SO4 there are 2moles of H .If you have a 0.0125M solution of H2SO4then the concentration of H is 2x as muchor 0.0250M22 A solution of 25 ml of 0.1M HCl and 50 ml of 0.5MHNO3 are mixed together. What is the [H ] ionconcentration of the resulting solution?AnswerAnswer21 What is the [H ] ion concentration of a 50 ml solutionof 0.025M H2 SO4 , when diluted with 150 ml of water?Slide 54 / 208[This object is a pulltab]Slide 55 / 208Slide 56 / 208Auto-ionization of WaterAs we have seen, water is amphoteric, meaning that itcan act as either an acid or a base.Auto-ionization of WaterIn pure water, a few molecules act as bases and a fewact as acids, in a process referred to as autoionization.HOHReturn to theTable of contents HHOThis value is known as the equilibrium constant, K and will bediscussed in more depth later in this unit.All concentrations are in M, molarity, asdesignated by brackets,[ ].K H2 O (l) H 2 O (l)K H 3 O (aq) OH- (aq)[H3O ] x [OH-][H2 O] x [H2 O]H 3 O (aq) OH- (aq)Slide 58 / 208Ion-Product ConstantAutoionization of WaterWhen there is an equilibrium state, the ratio of products toreactants yields a constant.HThe double headed arrow indicates that both theforward and reverse reactions occur simultaneously.Slide 57 / 208H 3 O (aq) OH- (aq)H OHHH2 O (l) H 2 O (l)H2 O (l) H 2 O (l)OIn most dilute acid and base solutions, the concentration ofundissociated water, remains more or less a constant.We can thus disregard the denominator in the equilibriumexpression.K [H3 O ] x [OH-][H2 O] x [H2 O]becomes Kw [H3O ] x [OH-]

Slide 59 / 208Ion-Product ConstantSlide 60 / 20823 The magnitude of K w indicates th at .Kw [H3 O ] x [OH ] -This special equilibrium constant, Kw is referred to asthe ion-product constant for water.At 25 C, Kw 1.0 x 10-14 . Since this is such a smallnumber, we conclude that pure water contains relativelyvery few ions.Awater ionizes to a very small extentBthe autoionization of water is exothermicCwater ionizes very quicklyDwater ionizes very slowlySlide 60 (Answer) / 20823 The magnitude of K w indicates th at .B24 The ion-product constant for water, Kw isrepresented bywater ionizes to a very small extentA[H2O]2K is aofverysmall numberthat means thethe autoionizationwateris exothermicamount of reactants is much greater thanB[H3O ] x [OH-]AAnswerASlide 61 / 208wthe amount of products. Water ionizes tovery small extent.Cwater ionizes very quicklyC[H3 O ] [OH -]Dwater ionizes very slowlyD[H3 O ] - [OH -][This object is a pulltab]Slide 61 (Answer) / 20824 The ion-product constant for water, Kw isrepresented bySlide 62 / 20825 What is the [H ] ion concentration of a solution with an[OH-] ion concentration of 1 x 10-9?Try to solve without a calculator![H2O]2B[H3O ] x [OH-]C[H3 O ] [OH -]D[H3 O ] - [OH -]AnswerAA 1 x 10 -14BKw [H3O ] x [OH-]B 1 x 10 5C 1 x 10 -5[This object is a pulltab]D 1.23 x 10 -5E 1 x 10 -7

Slide 62 (Answer) / 20825 What is the [H ] ion concentration of a solution with an[OH-] ion concentration of 1 x 10-9?Slide 63 / 20826 What is the [OH-] ion concentration of a solution with an[H ] ion concentration of 1 x 10-4?Try to solve without a calculator!Try to solve without a calculator!A 1 x 10A 1 x 10 -14CKw [H ][OH-][H ] Kw /[OH-][H ] 1 x 10 -14/ 1 x 10 -9[H ] 1x 10 -5Answer-14B 1 x 10 5C 1 x 10 -5[This object is a pulltab]D 1.23 x 10 -5E 1 x 10 -7B 1 x 10 10C 1 x 10 5D 1.23 x 10 -9E 1 x 10 -10Slide 63 (Answer) / 20826 What is the [OH-] ion concentration of a solution with an[H ] ion concentration of 1 x 10-4?Try to solve without a calculator!EKw [H ][OH-][H ] Kw /[OH-][H ] 1 x 10 -14/ 1 x 10 -4[H ] 1x 10 -10AnswerA 1 x 10 -14B 1 x 10 10C 1 x 10 5[This object is a pulltab]D 1.23 x 10 -9E 1 x 10 -10Slide 64 / 20827 What is the [OH-] ion concentration of a solution with an[H ] ion concentration of 1.23 x 10-9?A 1 x 10 -14B 4.34 x 10 -6C 1.23 x 10 5D 1.23 x 10 -5E 8. 13 x 10 -6Slide 64 (Answer) / 208Slide 65 / 20827 What is the [OH-] ion concentration of a solution with an[H ] ion concentration of 1.23 x 10-9?B 4.34 x 10 -6C 1.23 x 10 5D 1.23 x 10 -5E 8. 13 x 10 -6AnswerA 1 x 10 -14EKw [H ][OH-][H ] Kw /[OH-][H ] 1 x 10 -14/ 1.23 x 10 -9[H ] 8.13 x 10 -6pH[This object is a pulltab]Return to theTable of contents

Slide 66 / 208Slide 67 / 208pHpHIt is a measure of hydrogen ion concentration, [H ] in asolution, where the concentration is measured inmoles H per liter, or molarity.pH is defined as the negative base-10 logarithm of theconcentration of hydronium ion.pH -log [H 3 O ]The pH scale ranges from 0-14.pH is defined as the negative base-10 logarithm of theconcentration of hydronium ion.Hydrogen ionconcentration, [H ]in moles/LiterpH1.0 x 10-111.0 x 10-22pH -log [H 3O ]101.0 x 10-10Is the relationship between [H ] and pH a direct or an inverse one?Slide 68 / 208Slide 69 / 208pHBecause of the base-10 logarithm, each 1.0-point valueon the pH scale differs by a value of ten.A solution with pH 9 has a hydrogen ion concentration, [H ],that is ten times more than a pH 10 solution.A solution with pH 8 has a hydrogen ion concentration, [H ],that is 10 2 or 100 times more than a pH 10 solution.A solution with pH 7 has a hydrogen ion concentration, [H ],that is 10 3 or 1000 times more than a pH 10 solution.Slide 70 / 20828 The molar concentration of hydronium ion, [H3 O ],in pure water at 25 C is .A0A0B1B1C7C7D10-7E10-14-7D10E10-14Answer28 The molar concentration of hydronium ion, [H3 O ],in pure water at 25 C is .Slide 70 (Answer) / 208DIf the solution is neutral theconcentration of [H3O ] [OH-] and each has aconcentration of1x10 -7.[This object is a pulltab]

Slide 71 / 208Slide 71 (Answer) / 20829 A solution with pH 3 has a hydrogen ionconcentration that is than a solutionwith pH 5.A2x moreA2x moreBBC2x less100x moreC2x less100x moreD100x lessD100x lessAnswer29 A solution with pH 3 has a hydrogen ionconcentration that is than a solutionwith pH 5.CThe solution with a pH of 3 has ahydrogen ion concentration is 100x more than a solution with a pH of5, because pH is a log functionand the difference is1 x 10 3 vs 1 x 105 which is 100 xmore.[This object is a pulltab]Slide 72 / 208Slide 72 (Answer) / 20830 A solution with pH 14 has a hydrogen ionconcentration that is than asolution with pH 11.A3x moreA3x moreBC3x less1000x moreBC3x less1000x moreD1000x lessD1000x lessSlide 73 / 208Answer30 A solution with pH 14 has a hydrogen ionconcentration that is than asolution with pH 11.DThe solution with a pH of 14 has ahydrogen ion concentration is1000 x less because pH is a logfunction and the difference is1 x 10 14 vs 1 x 10 11 which is 1000x less.[This object is a pulltab]Slide 74 / 208pHpHTherefore, in pure waterpH -log [H3 O ] 7.00pH -log (1.0 # 10-7 ) 7.00ACIDBASE[H ] [OH-]There are excesshydrogen ions insolution.[H ] [OH-]There are excesshydroxide ions insolution.An acid has a higher [H3 O ] than pure water, so its pH is 7.A base has a lower [H3 O ] than pure water, so its pH is 7.Solution typeSolution typeAcidicNeutralBasicAcidicNeutralBasic[H ](M) 1.0x10 -7 1.0x10 -7 1.0x10 -7[OH-] (M) 1.0x10 -7 1.0x10 -7 1.0x10 -7pH value 7.00 7.00 7.00[H ](M) 1.0x10 -7 1.0x10 -7 1.0x10 -7[OH-] (M) 1.0x10 -7 1.0x10 -7 1.0x10 -7pH value 7.00 7.00 7.00

Slide 75 / 208pHMore basicThese are thepH values forseveral commonsubstances.1413Bleach12Soapy water11AmmoniaSlide 76 / 20831 For a basic solution, the hydrogen ionconcentration is than thehydroxide ion concentration.Milk of MagnesiaAgreater than9Baking soda8Sea waterB7Distilled waterCless thanequal to6UrineDNot enough information.5Black coffee10More acidic4Tomato juice3Orange juice2Lemon juiceGastric acid10Slide 76 (Answer) / 208Agreater thanBless thanAnswer31 For a basic solution, the hydrogen ionconcentration is than thehydroxide ion concentration.BIn a basic solution theconcentration of hydrogen ion isless than the concentration ofhydroxide ion.Cequal toDNot enough information.Slide 77 / 20832 For an acidic solution, the hydroxide ionconcentration is than thehydrogen ion concentration.Agreater thanBless thanequal toCDNot enough information.[This object is a pulltab]Slide 77 (Answer) / 208Agreater thanBless thanequal toCDAnswer32 For an acidic solution, the hydroxide ionconcentration is than thehydrogen ion concentration.BIn an acidic solution, theconcentration of hydroxide ion isless than the concentration ofhydrogen ion.Not enough information.[This object is a pulltab]Slide 78 / 20833 Which solution below has the highestconcentration of hydroxide ions?ApH 3.21BpH 7.00CpH 8.93DpH 12.6

Slide 78 (Answer) / 208ApH 3.21BpH 7.00CpH 8.93DpH 12.6Answer33 Which solution below has the highestconcentration of hydroxide ions?DThe smaller the pH the more acidicthe solution. The larger the pH themore basic the solution. Thesolution with the highestconcentration of hydroxide ion, themost basic solution, has thelargest pH in this case 12.6.[This object is a pulltab]Slide 79 / 2083

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