Acids, Bases And Salts
26/02/2012Acids, Bases and SaltsAcids, Bases and Salts(H bd Unit(HebdenU it 4 – page 109‐182)109 182)Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)We will cover the following topics:1. Definition of Acids and Bases2. Bronsted-Lowry Acids and BasesCHEM 0012 Lecture Notes21
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Arrhenius Definition of Acids and BasesAn acid is a substance that reacts with water to producephydronium ions, H3O .A base is a substance that produces hydroxide ions, OH-,in water.Hydroxide ionOH-When an acid and base reacts, an ionic compound is produced asone of the products. We call ionic compounds “salts”.CHEM 0012 Lecture Notes3Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Arrhenius Theory of Acid and BasesSupport for the Arrhenius concept comes from measurements of H of neutralization of any strong acid and base. Consider thefollowing reactions:NaOH(aq) HCl(aq) NaCl(aq) H2O( ) H -56 kJ/molLiOH(aq) HBr(aq) LiBr(aq) H2O( ) H -56 kJ/molIf we write the net ionic equation for both of these reactions wesee that they are the sameH (aq) OH-(aq) H2O( )CHEM 0012 Lecture Notes42
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Monoprotic and Polyprotic acids1. Monoprotic acids – capable off ionizing 1 H ion per moleculeof acid.Strong acid 100% dissociation into ionsExample:HCl (aq) H2O ( ) H3O (aq) Cl- (aq)CH3COOH (aq) H2O ( ) ֖ H3O (aq) CH3COO- (aq)Weak acid partial dissociation into ionsCHEM 0012 Lecture Notes5Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Monoprotic and Polyprotic acids2. Polyproticypacids – capablepof ionizingg more than one H ion ppermolecule of acid.Example of a Diprotic acid:H2SO4 (aq) H2O ( ) H3O (aq) HSO4- (aq)HSO4- (aq) H2O ( ) H3O (aq) SO42- (aq)Example of a Triprotic acid:H3PO4 (aq) H2O ( ) H3O (aq) H2PO4 - (aq)H2PO4 - (aq) H2O ( ) H3O (aq) HPO42- (aq)You should beable to writeacid dissociationreactions.Pay attention tothe charges onall the ions, andbalance thereactions.HPO4 2- (aq) H2O ( ) H3O (aq) PO43- (aq)CHEM 0012 Lecture Notes63
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Monoprotic and Polyprotic bases1. Monoprotic bases – capable off ionizing 1 OHO - ion per moleculeof base.Strong base 100% dissociation into ionsExample:NaOH (aq) Na (aq) OH- (aq)Nitrogeng compoundspare bases because theyy dissolve in waterto produce OH ions.NH3 (aq) H2O ( ) ֖ NH4 (aq) OH- (aq)CH3NH2 (aq) H2O ( ) ֖ CH3NH3 (aq) OH- (aq)Weak base partial dissociation into ionsCHEM 0012 Lecture Notes7Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Monoprotic and Polyprotic bases2. Polyprotic bases – capable off ionizing more than one OHO - ionper molecule of base.Example:You should beCa(OH)2 (aq) Ca2 (aq) 2 OH- (aq)Al(OH)3 (aq) Al3 (aq) 3 OH- (aq)able to writebasedissociationreactions.Pay attention tothe charges onall the ions, andbalance thereactions.CHEM 0012 Lecture Notes84
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)In general,1 Ioni1.Ionizationation of an acid in wateraterHA (aq) H2O ( ) H3O (aq) A- (aq)2. Ionization of a base in waterB (aq)( ) H2O ( ) BH (aq)( ) OH- (aq)( )orB(OH)x (aq) Bx (aq) x OH- (aq)CHEM 0012 Lecture Notes9Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)BrØnsted-Lowry Acids and BasesWhen neneutralizationtrali ation reaction occoccursrs in aqaqueouseo ssolution, Arrhenius’ definition of acid and baseworks well.HCl (aq) NH3 (aq) NH4Cl (aq) H2O( )Hydrochloric ammonia ammoniumacid(base)chlorideCHEM 0012 Lecture NotesRecall thatArrhenius Definition ofAcid and BaseAn acid as a substancethat reacts with waterto produce H3O .A base that reactswith water to produceOH‐.105
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)BrØnsted-Lowry Acids and BasesThis same neneutralizationtrali ation reaction can occoccurr whenhen it is not in anaqueous medium. Therefore, Arrhenius’s definition of an acid anda base is too restrictive.Example: Neutralization reaction of reactants in gas phaseHCl (g) NH3 (g) NH4Cl (s)Hydrogen ammonia smoke containingchloridegastiny crystalsgasof ammonium chlorideWe need a broader definition!CHEM 0012 Lecture Notes11Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)BrØnsted-Lowry Acids and BasesWhat is in common betbetweeneen the gaseogaseouss and aqaqueouseo s reactions?1. Both involve a transfer of a H from one reactant to another.In solution, HCl is completely ionized and the H ion istransferred from HCl to NH3.NH3 (aq) H3O (aq) Cl- (aq) NH4 (aq) Cl- (aq) H2O ( )In gas phase,NH3 (g) HCl (g) NH4 Cl- (s)CHEM 0012 Lecture Notes126
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)BrØnsted-Lowry Acids and Bases ViewVie acidacid-basebase reactions as simplysimpl the transfer of H (protons)from one species to another.BrØnsted-Lowry Acids and Bases DefinitionsAcid is a proton donor.Base is a proton acceptoracceptor.HCl (g) NH3 (g) NH4 Cl- (s)This species donatesa proton to NH3,therefore, it is an acid.This species acceptsa proton, therefore,it is a base.CHEM 0012 Lecture Notes13Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)BrØnsted-Lowry Acids and BasesIn generalgeneral,HAH donorACID B BH H acceptorBASEH donorACID AH acceptorBASECONJUGATE ACID-BASE PAIRSTwo species that differ by H are called a conjugate pair.There is a whole table ofCHEMBr0012Ønsted-LowryAcids and Bases.14Lecture Notes7
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)WEAKWSTRONGGBrØnsted-Lowry Acids and Bases15STRONGWEAKStrenngth of acidStrength of baseCHEM 0012 Lecture NotesAcids, Bases and SaltsHebden – Unit 4 (page 109‐182)BrØnsted-Lowry Conjugate Acids-Bases PairsAcidH2ONH4 HCO3H3O N2H4H3O NH3H2CO3HPO42--H H BaseOHNH3CO32H2ON2H3H2ONH2HCO3PO43-CHEM 0012 Lecture Notes168
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)We will cover the following topics:1. Amphiprotic Substance2. Amphoteric CompoundsCHEM 0012 Lecture Notes17Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)1. Amphiprotic SubstanceA substance that can act either as a pproton acceptorp or a pprotondonor.All amphiprotic substances contain a hydrogen atom.Example 1 – Water, H2OH2O ( ) HCl (aq) H3O (aq) Cl- (aq)baseacidH2O ( ) NH3 (aq) NH4 (aq) OH- (aq)acidbaseCHEM 0012 Lecture Notes189
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)1. Amphiprotic SubstanceA substance that can act either as a pproton acceptorp or a pprotondonor.All amphiprotic substances contain a hydrogen atom.Example 2 – Bicarbonate, HCO3You shouldbe able towrite theseequations.HCO3- (aq) H3O (aq) H2CO3 (aq) H2O ( )baseacidHCO3- (aq) OH- (aq) CO32- (aq) H2O ( )acidbaseCHEM 0012 Lecture Notes19Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)1. Amphiprotic SubstanceA substance that can act either as a pproton acceptorp or a pprotondonor.All amphiprotic substances contain a hydrogen atom.Example 3 – hydrogen sulfate ion, HSO4You shouldbe able towrite theseequations.HSO4- (aq) H3O (aq) H2SO4 (aq) H2O ( )baseacidHSO4- (aq) OH- (aq) SO42- (aq) H2O ( )acidbaseCHEM 0012 Lecture Notes2010
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)2. Amphoteric Substance A compoundpthat can react as either an acid or a base. “Ampho-” is Greek, it means “both”. Metals have amphoteric oxides. (eg – ZnO, Al(OH)3)Example 1 – Zinc oxide, ZnOReacts with acid: ZnO(aq) 2H3O (aq) Zn2 (aq) 3H2O( )acts as a baseReacts with base:ZnO (aq) 2 OH- (aq) H2O ( ) [Zn(OH)4]2- (aq)acts as an acidzincate ionCHEM 0012 Lecture Notes21Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)2. Amphoteric Substance A compoundpthat can react as either an acid or a base. “Ampho-” is Greek, it means “both”. Metals have amphoteric oxides. (eg – ZnO, Al(OH)3)Example 2 – Water, H2OReacts with acid: H2O ( ) HCl (aq) H3O (aq) Cl- (aq)acts as a baseReacts with base: H2O ( ) NH3 (aq) NH4 (aq) OH- (aq)acts as an acidCHEM 0012 Lecture Notes2211
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)2. Amphoteric Substance A compoundpthat can react as either an acid or a base. “Ampho-” is Greek, it means “both”. Metals have amphoteric oxides. (eg – ZnO, Al(OH)3)Example 3 – Aluminum hydroxide, Al(OH)3Reacts with acid:Al(OH)3 (aq) 3HCl (aq) AlCl3 (aq) 3 H2O ( )acts as a baseReacts with base:Al(OH)3 (aq) OH- (aq) [Al(OH)4] - (aq)acts as an acid CHEM 0012 Lecture Notesaluminate ion23Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Strong acidsAn acid which dissociates 100% into its ions in a water solution.Strong acid 100% dissociation into ionsHCl (aq) H2O ( ) H3O (aq) Cl- (aq)The [H ] (or [H3O ]) concentration of a 0.10 M HCl solution is0.10 M.For monoprotic strong acids [acid] [H ]A common notation to express [H ] is pH, wherepH -log [H ] -log 0.10 1.00CHEM 0012 Lecture Notes2412
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Recall the pH scalepH - log [H ]10-10 M0.1 M0.01 M 0.001 M10-9 M10-11 MFor an increase in 1 pH unit, the solution’s [H ] decreases 10x.CHEM 0012 Lecture Notes25Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)KaStrong acidsThese are strong acidsacids.Dissociation is a single arrow to produce ions.CHEM 0012 Lecture Notes2613
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Weak acidsAn acid which dissociates less than100% into its ions in a waterWeak acid 100% dissociation into ionsions.solutionsolution.Use double arrows to indicate this.CH3COOH (aq) H2O ( )H3O (aq) CH3COO- (aq)The [H ] (or [H3O ]) concentration of a 0.10 M CH3COOHsolution is LESS THAN 0.10 M.Therefore,pH 1.00In weak acids [acid] [H ] CHEM 0012 Lecture Notes27Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Weak acidsAn acid which dissociates less than100% into its ions in a watersolutionsolution.HA (aq) H2O (l)H3O (aq) A- (aq)CHEM 0012 Lecture Notes2814
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)KaWeak acids.These are weak acids exceptthe bottom two.These last two are too weak to act as acids in water.Note the single arrows pointing backward because theforward dissociation never occurs.CHEM 0012 Lecture Notes29Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Illustration of Strong andWeak AcidsGraphic representationof the behavior of acidsof different strengths inaqueous solution.(a) A strong acid.(b) A weakk acid.idCHEM 0012 Lecture Notes3015
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Illustration of Strong and Weak Acids(a)(b)(a) A strong acid HA is completely ionized in water.(b) A weak acid HB exists mostly as undissociated HBmolecules in water.Note that the water moleculesareLecturenot shownin this figure.CHEM 0012Notes31Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Strong basesA base which dissociates 100% into its ions in a water solution.Strong base 100% dissociation into ionsNaOH (aq) Na (aq) OH- (aq)The [OH-] concentration of a 0.10 M NaOH solution is 0.10 M.For NaOH, [base] [OH-]A common notation to express [OH-] is pOH, wherepOH -log [OH-] -log 0.10 1.00CHEM 0012 Lecture Notes3216
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)pH and pOH scales[H ] [OH-]NEUTRAL[H ] [OH-][OH-] [H ]basicacidicConvert between pH and pOH:pH pOH 14 at 25 CCHEM 0012 Lecture Notes33Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Strong basesThese are strong bases.Any substance which dissociates completely to produce OH-, O2-,or NH2- is a strong basebase.Examples: Group 1 hydroxides: LiOH, NaOH, KOH, RbOH, CsOHGroup 2 hydroxides: Mg(OH)2, Ba(OH)2, Sr(OH)2CHEM 0012 Lecture Notes3417
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Strong bases ForFor NaOH, [OH-] [base] For Ba(OH)2, [OH-] 2 x [base]Salts which produce O2- are strong bases.Example: CaO (s) Ca 2 (aq) O2- (aq)O2- (aq) H2O ( ) 2 OH- (aq)CHEM 0012 Lecture Notes35Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Weak basesA base which dissociates less than100% into its ions in a waterWeak bases 100% dissociation into ionsions.solutionsolution.Use double arrows to indicate this.NH3 (aq) H2O ( )NH4 (aq) OH- (aq)The [OH-] concentration of a 0.10 M NH3 solution isLESS THAN 0.10 M.Therefore,pOH 1.00In weak bases [base]CHEM 0012 Lecture Notes [OH ]-3618
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Weak basesA base which dissociates less than100% into its ions in a watersolutionsolution.B (aq) H2O ( )BH (aq) OH- (aq)CHEM 0012 Lecture Notes37Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)KaWeak basesConjugate bases of strong acids are VERY weak bases.CHEM 0012 Lecture NotesThese are weak basesbases, foundon the right side of the table.3819
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Amphiprotic Species Found on both sides off the table (eg( – HSOSO4-) Can act as acids or as bases When found on the left, it is an acid.KaAcidStrengthincreasesHCO3- is a weaker acid than phenol and a stronger acidthan hydrogen peroxide.CHEM 0012 Lecture Notes39Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Amphiprotic Species Found on both sides off the table (eg( – HSOSO4-) Can act as acids or as bases When found on the right, it is a base.KaBaseStrengthincreasesHCO3- is a weaker base than citrate ion and a stronger basethan Al(H2O)5(OH)2 .CHEM 0012 Lecture Notes4020
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)WEAKWSTRONGGBrØnsted-Lowry Acids and Bases41STRONGWEAKStrenngth of acidStrength of baseCHEM 0012 Lecture NotesAcids, Bases and SaltsHebden – Unit 4 (page 109‐182)We will work with the reference tableRELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASESto determine the Acid-Base Equilibria and Relative Strengths ofAcids and Bases.By examining the relative strengths of the acids on both sides ofthe equilibrium, we can determine which side of the equilibrium isfavoured.CHEM 0012 Lecture Notes4221
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)1. When H2CO3 and SO32- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?2 (aq)H2CO3 (aq)( ) SO32( )This can onlydonate a H ion. It is anACID.HCO3- (aq)( ) HSO3- (aq)( )This ion canonly act as aBASE, accepta H ion.As a result HCO3‐ isi thethconjugatebase ofH2CO3.HSO3‐ is theconjugateacid of SO3.CHEM 0012 Lecture Notes43Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)1. When H2CO3 and SO32- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?H2CO3 (aq) SO322- (aq)acidbaseHCO3- (aq) HSO3- (aq)conjugate baseconjugate acidCompare the Ka of the two acidsH2CO3 is a slightly stronger acid than HSO3-.The equilibrium will favour the products.CHEM 0012 Lecture Notes4422
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)1. When H2CO3 and SO32- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?֖2 (aq)( ) SO32( )H2CO3 (aq)acidbase( ) HSO3- (aq)( )HCO3- (aq)conjugate baseconjugate acidWhat is the value of K for this equilibrium?Since K 1, equilibrium favors productsCHEM 0012 Lecture Notes45Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)2. When H2PO4- and CO32- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?2 (aq)H2PO4- (aq)( ) CO32( )This is anamphiprotic ion.It can donate oraccept a H ion.֖2 (aq)HCO3- (aq)( ) HPO42( )This ion canonly act as aBASE, accepta H ion.After considering,in this mixture,H2PO4‐ will act asan acid.As a result HCOCO3‐ isi thehconjugateacid ofCO32‐.CHEM 0012 Lecture Notes2 isHPOO42‐i thehconjugatebase ofH2PO4‐.4623
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)2. When H2PO4- and CO32- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?H2PO4- (aq) CO322- (aq)acid֖baseHCO3- (aq) conjugate acidHPO422- (aq)conjugate baseCompare the Ka of the two acidsH2PO4- is a stronger acid than HCO3-.The equilibrium will favour the products.CHEM 0012 Lecture Notes47Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)3. When HSO4- and NH3 are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?HSO4- (aq) This is anamphiprotic ion.It can donate oraccept a H ion.NH3 (aq)֖NH4 (aq)This can onlyact as aBASE, accepta H ion.After considering,in this mixture,HSO4‐ will act asan acid. SO42- (aq)As a result NH4 is theconjugateacid of NH3.CHEM 0012 Lecture NotesSO42‐ is theconjugatebase ofHSO4‐.4824
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)3. When HSO4- and NH3 are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?HSO4- (aq)( ) NH3 (aq)( )acidbase֖NH4 (aq)( ) conjugate acid2 (aq)SO42( )conjugate baseCompare the Ka of the two acidsHSO4- is a stronger acid than NH4 .The equilibrium will favour the products.CHEM 0012 Lecture Notes49Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)4. When HSO4- and H2PO4- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?Both HSO4- and H2PO4- are amphiprotic ionsions.Which will play the role of an acid? Let’s compare their Ka values.HSO4- is a stronger acid than H2PO4-.HSO4- will act as an acid donating protons to H2PO4-.After considering, in this mixture, HSO4‐ willact as an acid. H2PO42‐ will act as the base.CHEM 0012 Lecture Notes5025
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)4. When HSO4- and H2PO4- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?֖HSO4- (aq) H2PO4- (aq)Ka of HSO4‐ isbigger. It hasthe highertendency toddonatet H . Ka of H2PO4‐ issmaller.Comparatively,it has lesstendencyy todonate H .After considering, inthis mixture, HSO4‐will act as an acid.H3PO4 (aq) SO422- (aq)As a result H3PO4 is theconjugateacid of H2PO4‐.SO42‐ is theconjugatebase ofHSO4‐.CHEM 0012 Lecture Notes51Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)4. When HSO4- and H2PO4- are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?HSO4- (aq)( ) H2PO4- (aq)( )acidbase֖2 (aq)H3PO4 (aq)( ) SO42( )conjugate acid conjugate baseCompare the Ka of the two acidsHSO4- is a stronger acid than H3PO4 .The equilibrium will favour the products.CHEM 0012 Lecture Notes5226
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)5. When CH3COOH and NH3 are mixed, an equilibrium is set up.Which side of the equilibrium is favoured?֖ CH3COO- (aq) NH4 (aq)conjugate base conjugate acidCH3COOH (aq) NH3 (aq)acidbaseCompare the Ka of the two acidsCH3COOH H CH3COONH4 H NH31.8x1018x10-55.6x10-10CH3COOH is a stronger acid than NH4 .The equilibrium will favour the products.CHEM 0012 Lecture Notes53Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)6. Consider an amino acid, an equilibrium is set up between theamine group, R-NH2, and the carboxylic acid group, R-COOH .Which side of the equilibrium is favoured?H2NCHRCOOH (aq)base֖acid H NCHRCOO3conjugate acid(aq)conjugate baseCompare the Ka of the two acidsCH3COOH ֖ H CH3COONH4 ֖ H NH31.8x1018x10-55.6x10-10CH3COOH is a stronger acid than NH4 .The equilibrium will favour the products(i.e. a double chargedspecies).CHEM 0012 Lecture Notes5427
26/02/2012Acids, Bases and SaltsHebden – Unit 4 (page 109‐182)Direction of Reaction ExamplePredict the direction favored in each of the following acid-basereactions That isreactions.is, does the reaction tend to go more in the forwardor in the reverse direction?a) NH4 OH- ֖ H2O NH3Forwardb) HSO4- NO3- ֖ HNO3 SO42c) HSO3 CH3-COO-֖ SO3 CH3COOH2-ReverseReversed) CH3COOH Cr(H2O)5(OH)2 ֖ Cr(H2O)63 CH3COO-Reversee) HNO2 ClO4 ֖ HClO4 NO2Reverse-f)-H2CO3 CO32- ֖ HCO3- HCO3-Forward55Acids, Bases and SaltsHebden – Unit 4 (page 109‐182) In aqueous soluti
Acids, Bases and Salts Hebden – Unit 4 (page 109‐182) We will cover the following topics: 1. Amphiprotic Substance 2. Amphoteric Compounds CHEM 0012 Lecture Notes 17 Acids, Bases and Salts Hebden – Unit 4 (page 109‐182) 1. Amphiprotic Substance A substance that can act either as a pppproton acceptor or a proton donor.
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
_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
Chapter 2 Page 8 Strength of acids and bases: Strength of acids and bases depends on the no. of H ions and OH– ions produced respectively. a. Strong acids give rise to more H ions. eg. HCl, H 2 SO 4, HNO 3. b. Weak Acids give less H ions eg. CH 3 COOH, H 2 CO 3 (Carbonic acid) c. Strong bases give rise to more OH– ions. eg. NaOH, KOH, Ca(OH)
Acids, Bases and Salts 96 Learning Objectives After completing this lesson, students will be able to know about formation, properties and uses of acids, bases and salts know about how they play a vital role in our daily life understand how to identify the nature of a solution by using indicators and pH paper
Chap 3 aCids, Bases and salts page 39 t pdf o v a i o To Purchase Hard Book of From Amazon Click Here. For More Details Whatsapp at 8905629969 ChAptER 2 Bcids, Bases and Salts 3.1 acids Acids are chemical compounds which have sour taste, consist of hydrogen (H), and turn blue litmus solution red. On the basis of their sources,
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
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