1. Tutorial on Acid Base, pH scale and IonicProduct Constant of Water Kw Prepared by Lawrence Kok http://lawrencekok.blogspot.com

2. Definition of Acid and BasesWater/aqueous medium1 Arrhenius acid - substance dissociates in water to produce H+ ions.Arrhenius base substance dissociates in water to produce OH- ions.All Arrhenius acid are Bronsted Lowry acid and water must be presentArrhenius acidH+ Arrhenius base OH-HCI H+ + CI- NaOH Na+ + OH-HCI + H2O H3O+ + CI- NH3 + H2O NH4+ + OH- CO32- + H2O HCO3- + OH-2Brnsted-Lowry Acid - substance that donates proton/proton donorWater/aqueous medium Bronsted-Lowry Base substance that accepts proton/proton acceptor Other solvent medium possible One species donate proton one species accept protongain Hgain HH2O (base) - H3O+ (conjugate acid)Acid +Base Conjugate Base + Conjugate AcidHCI + H2O CI- + H3O+ lose HHCI (acid) - CI- (conjugate base)lose H3Lewis Acid - substance that accepts electron/electron acceptor, empty orbital/electron deficient Lewis Base substance that donates electron/electron donor, lone pair electron Lewis Base - donate electron pair forming dative/coordinate bond with Lewis acid HCI accept e- H2O donate e- HCI + H2O CI- + H3O+Lewis acid Lewis basehttp://4photos.net/en/image:44-225901-Water_droplets_on_blue_backdrop__images 3. Properties of Acids and BasesPhysical PropertiesPhysical PropertiesPhysical properties of AcidsPhysical properties of Acids Substance dissolves in water producehydrogen/H+ or hydronuim /H3O+ HCI H+ + CI- Conduct electricity free moving ions Sour, pH < 7 Turns blue litmus red Turns phenolphthalein colourless Turns methyl orange to red 4. Properties of Acids and BasesPhysical PropertiesPhysical PropertiesPhysical properties of AcidsPhysical properties of BasesPhysical properties of AcidsPhysical properties of Bases Substance dissolves in water produce Substance dissolves in water produce hydroxide/OH- ionhydrogen/H+ or hydronuim /H3 O+ HCI H+ + CI- NaOH Na+ + OH- Conduct electricity free moving ions Conduct electricity free moving ions Bitter, pH > 7 Sour, pH < 7 Turns red litmus blue Turns blue litmus red Turns phenolphthalein colourless Turns phenolphthalein pink Turns methyl orange to red Turns methyl orange to yellow 5. Properties of Acids and Bases Physical PropertiesChemical Properties Physical Properties Physical properties of AcidsPhysical properties of Bases Physical properties of AcidsPhysical properties of Bases Substance dissolves in water produce Substance dissolves in water producehydroxide/OH- ionhydrogen/H+ or hydronuim /H3 O+ HCI H+ + CI- NaOH Na+ + OH- Conduct electricity free moving ions Conduct electricity free moving ions Bitter, pH > 7 Sour, pH < 7 Turns red litmus blue Turns blue litmus red Turns phenolphthalein colourless Turns phenolphthalein pink Turns methyl orange to red Turns methyl orange to yellow Chemical Properties Chemical properties of Acids / BasesAcid + Metal (above H) Salt + H2 gas2HCI + Mg MgCI2 + H2Acid + Base Salt + Water + product.Bases are - Metal Hydroxide, Metal Oxide, Metal CarbonatesAcid + Metal Hydroxide Salt + WaterAcid + Metal Oxide Salt + WaterAcid + Metal Carbonate Salt + Water + Carbon DioxideAcid + Ammoniaaq and Amines Salt + waterHCI + NH4OH NH4CI + H2OHCI + CH3NH2 CH3NH3 + CI- 6. Properties of Acids and Bases Physical PropertiesChemical Properties Physical Properties Physical properties of AcidsPhysical properties of Bases Physical properties of AcidsPhysical properties of Bases Substance dissolves in water produce Substance dissolves in water producehydroxide/OH- ionhydrogen/H+ or hydronuim /H3 O+ HCI H+ + CI- NaOH Na+ + OH- Conduct electricity free moving ions Conduct electricity free moving ions Bitter, pH > 7 Sour, pH < 7 Turns red litmus blue Turns blue litmus red Turns phenolphthalein colourless Turns phenolphthalein pink Turns methyl orange to red Turns methyl orange to yellow Chemical Properties Chemical properties of Acids / BasesAcid + Metal (above H) Salt + H2 gas2HCI + Mg MgCI2 + H2Acid + Base Salt + Water + product.Bases are - Metal Hydroxide, Metal Oxide, Metal CarbonatesAcid + Metal Hydroxide Salt + WaterAcid + Metal Oxide Salt + WaterAcid + Metal Carbonate Salt + Water + Carbon DioxideAcid + Ammoniaaq and Amines Salt + waterHCI + NH4OH NH4CI + H2OHCI + CH3NH2 CH3NH3 + CI- 7. Physical/Chemical Properties of Acids and BasesPhysical properties of Acids/BasesPhysical properties of Acids Electrolytes, produces H3O+, hydronium ion Conduct electricity Sour, pH < 7 Turns litmus red, Turns phenolphthalein colourless Turns methyl orange to redPhysical properties of Bases Bitter, pH > 7 Turns litmus blue Turns phenolphthalein pink Turns methyl orange to yellow 8. Physical/Chemical Properties of Acids and BasesPhysical properties of Acids/Bases Chemical properties of Acids / BasesPhysical properties of AcidsAcid with Metal Salt + H2 gas2HCI + Mg MgCI2 + H2 Electrolytes, produces H3O+, hydronium ion Conduct electricityAcid with Base (Neutralization) Salt + Water Sour, pH < 7Bases are - Metal Hydroxide, Metal Oxide, Metal Carbonates Turns litmus red,Acid + Metal Hydroxide Turns phenolphthalein colourlessAcid + Metal Oxide Turns methyl orange to redAcid + Metal CarbonatePhysical properties of Bases Bitter, pH > 7Acid with Ammonia(aq) and Amines Salt + water Turns litmus blueHCI + NH4OH NH4CI + H2O Turns phenolphthalein pink Turns methyl orange to yellow HCI + CH3NH2 CH3NH3 + CI- 9. Physical/Chemical Properties of Acids and BasesPhysical properties of Acids/Bases Chemical properties of Acids / BasesPhysical properties of AcidsAcid with Metal Salt + H2 gas2HCI + Mg MgCI2 + H2 Electrolytes, produces H3O+, hydronium ion Conduct electricityAcid with Base (Neutralization) Salt + Water Sour, pH < 7Bases are - Metal Hydroxide, Metal Oxide, Metal Carbonates Turns litmus red,Acid + Metal Hydroxide Turns phenolphthalein colourlessAcid + Metal Oxide Turns methyl orange to redAcid + Metal CarbonatePhysical properties of Bases Bitter, pH > 7Acid with Ammonia(aq) and Amines Salt + water Turns litmus blueHCI + NH4OH NH4CI + H2O Turns phenolphthalein pink Turns methyl orange to yellow HCI + CH3NH2 CH3NH3 + CI- Bases 10. Physical/Chemical Properties of Acids and BasesPhysical properties of Acids/Bases Chemical properties of Acids / BasesPhysical properties of AcidsAcid with Metal Salt + H2 gas2HCI + Mg MgCI2 + H2 Electrolytes, produces H3O+, hydronium ion Conduct electricityAcid with Base (Neutralization) Salt + Water Sour, pH < 7Bases are - Metal Hydroxide, Metal Oxide, Metal Carbonates Turns litmus red,Acid + Metal Hydroxide Turns phenolphthalein colourlessAcid + Metal Oxide Turns methyl orange to redAcid + Metal CarbonatePhysical properties of Bases Bitter, pH > 7Acid with Ammonia(aq) and Amines Salt + water Turns litmus blueHCI + NH4OH NH4CI + H2O Turns phenolphthalein pink Turns methyl orange to yellow HCI + CH3NH2 CH3NH3 + CI- Bases Acid + AlkaliAcid + Metal Hydroxide Acids + Metal OxideAcid + Metal Carbonate 11. Physical/Chemical Properties of Acids and BasesPhysical properties of Acids/Bases Chemical properties of Acids / BasesPhysical properties of AcidsAcid with Metal Salt + H2 gas2HCI + Mg MgCI2 + H2 Electrolytes, produces H3O+, hydronium ion Conduct electricityAcid with Base (Neutralization) Salt + Water Sour, pH < 7Bases are - Metal Hydroxide, Metal Oxide, Metal Carbonates Turns litmus red,Acid + Metal Hydroxide Turns phenolphthalein colourlessAcid + Metal Oxide Turns methyl orange to redAcid + Metal CarbonatePhysical properties of Bases Bitter, pH > 7Acid with Ammonia(aq) and Amines Salt + water Turns litmus blueHCI + NH4OH NH4CI + H2O Turns phenolphthalein pink Turns methyl orange to yellow HCI + CH3NH2 CH3NH3 + CI-Acid + Metal Hydroxide (Alkali) Salt + Water Acid + Metal Hydroxide (Insoluble) Salt + WaterLiOH + HCI LiCI + H2OCa(OH)2 + 2HCI CaCI2 + 2H2ONaOH + HNO3 NaNO3 + H2OFe(OH)2 + 2HNO3 Fe(NO3)2 + 2H2OKOH + H2SO4 K2SO4 + H2OMg(OH)2 + H2SO4 MgSO4 + 2H2O Bases Acid + AlkaliAcid + Metal Hydroxide Acids + Metal OxideAcid + Metal CarbonateAcid + Metal Oxide Salt + WaterAcid +Metal Carbonate Salt, Water + CO2CaO + 2HCI CaCI2 + H2O CaCO3 + 2HCI CaCI2 + H2O + CO2CuO + 2HCI CuCI2 + H2O CuCO3 + 2HCI CuCI2 + H2O + CO2 12. Strong Acid / BaseWeak Acid / Base VsStrong acid ionise/dissociate completely producing H+ ion Weak acid ionise/dissociate partially producing H+ ionStrong base ionise/dissociate completely producing OH- ionWeak base ionise/dissociate partially producing OH- ionAll are in ions state, NO molecule left Most in undissociated molecule formStrong electrolyte with high conductivity Poor electrolyte with low conductivity 13. Strong Acid / BaseWeak Acid / Base VsStrong acid ionise/dissociate completely producing H+ ion Weak acid ionise/dissociate partially producing H+ ionStrong base ionise/dissociate completely producing OH- ionWeak base ionise/dissociate partially producing OH- ionAll are in ions state, NO molecule left Most in undissociated molecule formStrong electrolyte with high conductivity Poor electrolyte with low conductivity Monoprotic acid - 1 mole H+ ionsWeak acid dissociate partially produce few H+ ion HCI H+ + CI-CH3COOH H+ + CH3COO- HBr H+ + Br(1 mole) (0.01 mole) (1 mole) (1 mole)Diprotic acid - 2 mole H+ ions H2SO4 2H+ + SO42-Weak base dissociate partially produce few OH- ion (1 mole)(2 mole)NH3 + H2O NH4+ + OH-C2H5NH2 + H2O C2H5NH3 + OH- + Monoprotic base - Accept 1 mole H+ ions by 1mole OH-CO32-+ H2O HCO3- + OH- Na(OH) Na+ + OH (1 mole) (1 mole)Ba(OH)2 Ba2+ + 2OHWeak triprotic acid dissociate partially produce few H+ ion(1 mole)(2 mole)H3PO4 H+ + H2PO4-Diprotic base - Accept 2 mole H+ ions by 2 mole OH- H2PO4- H+ + HPO42-HPO42- H+ + PO43-H3PO4 3H+ + PO43- 14. Strong Acid / Base Weak Acid / BaseVsStrong acid ionise/dissociate completely producing H+ ion Weak acid ionise/dissociate partially producing H+ ionStrong base ionise/dissociate completely producing OH- ionWeak base ionise/dissociate partially producing OH- ionAll are in ions state, NO molecule left Most in undissociated molecule formStrong electrolyte with high conductivity Poor electrolyte with low conductivity Monoprotic acid - 1 mole H+ ions Weak acid dissociate partially produce few H+ ionHCI H+ + CI- CH3COOH H+ + CH3COO-HBr H+ + Br (1 mole) (0.01 mole) (1 mole)(1 mole)Dissociate completelyNo molecules left All ions formDissociate partiallyFew ions Molecules left formDiprotic acid - 2 mole H+ ionsH2SO4 2H+ + SO42- Weak base dissociate partially produce few OH- ion(1 mole)(2 mole)NH3 + H2O NH4+ + OH-C2H5NH2 + H2O C2H5NH3 + OH- + Monoprotic base - Accept 1 mole H+ ions by 1mole OH-CO32-+ H2O HCO3- + OH-Na(OH) Na+ + OH(1 mole) (1 mole)Dissociate partially Few ionsDissociate completely formMolecules leftNo molecules leftAll ions form Ba(OH)2 Ba2+ + 2OH Weak triprotic acid dissociate partially produce few H+ ion (1 mole)(2 mole) H3PO4 H+ + H2PO4- Diprotic base - Accept 2 mole H+ ions by 2 mole OH-H2PO4-H+ + HPO42-HPO42-H+ + PO43-H3PO4 3H+ + PO43- 15. Strong Acid / Base Weak Acid / BaseVsStrong acid ionise/dissociate completely producing H+ ion Weak acid ionise/dissociate partially producing H+ ionStrong base ionise/dissociate completely producing OH- ionWeak base ionise/dissociate partially producing OH- ionAll are in ions state, NO molecule left Most in undissociated molecule formStrong electrolyte with high conductivity Poor electrolyte with low conductivity Monoprotic acid - 1 mole H+ ions Weak acid dissociate partially produce few H+ ionHCI H+ + CI- CH3COOH H+ + CH3COO-HBr H+ + Br (1 mole) (0.01 mole) (1 mole)(1 mole)Dissociate completelyNo molecules left All ions formDissociate partiallyFew ions Molecules left formDiprotic acid - 2 mole H+ ionsH2SO4 2H+ + SO42- Weak base dissociate partially produce few OH- ion(1 mole)(2 mole)NH3 + H2O NH4+ + OH-C2H5NH2 + H2O C2H5NH3 + OH- + Monoprotic base - Accept 1 mole H+ ions by 1mole OH-CO32-+ H2O HCO3- + OH-Na(OH) Na+ + OH(1 mole) (1 mole)Dissociate partially Few ionsDissociate completely formMolecules leftNo molecules leftAll ions form Ba(OH)2 Ba2+ + 2OH Weak triprotic acid dissociate partially produce few H+ ion (1 mole)(2 mole) H3PO4 H+ + H2PO4- Diprotic base - Accept 2 mole H+ ions by 2 mole OH-H2PO4-H+ + HPO42-HPO42-H+ + PO43-H3PO4 3H+ + PO43- Example of Strong Acid/BaseExample of Weak Acid/BaseStrong Acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4 Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, HNO2, H3PO4Strong Base - LiOH, KOH, NaOH, CsOH, Ca(OH)2, Ba(OH)2 Weak Base - NH3, C2H5NH2 , CH3NH2, (CH3)2NH, C3H5O2NH2 16. Strong Acid / Base Weak Acid / BaseVsStrong acid ionise/dissociate completely producing H+ ionWeak acid ionise/dissociate partially producing H+ ionStrong base ionise/dissociate completely producing OH- ion Weak base ionise/dissociate partially producing OH- ionAll are in ionic ions stateMost in undissociated molecule formStrong electrolyte with high conductivity Poor electrolyte with low conductivity Monoprotic acid - produce 1 mole H+ ionsWeak acid dissociate partially produce few H+ ion HCI H+ + CI- CH3COOHH+ + CH3COO- HBr H+ + Br (1 mole) (0.01 mole) (1 mole) (1 mole)Weak bases dissociate partially produce few OH- ionDiprotic acid - 2 mole of H+Diprotic base - 2 mole of OH-H2SO4 2H+ + SO42-Ba(OH)2 Ba2+ + 2OH NH3 + H2O NH4+ + OH- C2H5NH2 + H2O C2H5NH3 + OH-+(1 mole) (2 mole)(1 mole)(2 mole) CO32-+ H2O HCO3- + OH- Example Strong Acid/Base Example Weak Acid/BaseStrong acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, HNO2, H3PO4Strong base - LiOH, KOH, NaOH, CsOH, Ca(OH)2, Ba(OH)2Weak Base - NH3, C2H5NH2 , CH3NH2, (CH3)2NH, C3H5O2NH2Concentrated Acid / BaseVsDiluted Acid / BaseConcentrated Acid High number of moles/amt of solutes per dm3 Diluted Acid Low number of moles/amt of solutes per dm31 M HCI 1 mole of HCI molecules in 1 dm30.1M HCI 0.1 mole of HCI molecules in 1 dm310 M HCI 10 moles of HCI molecules in 1 dm3 0.01M HCI 0.01 moles of HCI molecules in 1 dm3Concentrated Acid may not be a Strong AcidDiluted Acid may be a Strong Acid10M CH3COOH Concentrated Acid but Weak Acid 0.01M HCI Diluted Acid but Strong Acid 10M CH3COOH - CONCENTRATED WEAK acid because 10M acid molecule will dissociate partially forming few H+ ions0.01M HCI - DILUTED STRONG acid because all 0.01M acid molecule dissociate fully forming H+ ions 17. pH measurement of Acidity of solution pH is the measure of acidity of a solution in logarithmic scalepH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration Acidic pH < 7 Alkaline pH > 7 18. pH measurement of Acidity of solution pH is the measure of acidity of a solution in logarithmic scalepH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration Acidic pH < 7 Alkaline pH > 7 pH with Conc H+pH = -log [H+][H+] = 0.0000001MpH = -log [0.0000001]pH = -log1010-7pH = 7 (Neutral) pOH with Conc OH-pOH = -log [OH-] [OH-] = 0.0000001M pOH = -log [0.0000001] pOH = -log1010-7 pOH = 7 pH + pOH = 14 pH + 7 = 14 pH = 7 (Neutral) 19. pH measurement of Acidity of solution pH is the measure of acidity of a solution in logarithmic scalepH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration Acidic pH < 7 Alkaline pH > 7 pOH with Conc OH-pH with Conc H+ pOH = -log [OH-]pH = -log [H+][OH-] = 0.1M[H+] = 0.0000001M pOH = -log[0.1]pH = -log [0.0000001] pOH = 1pH = -log1010-7 pH + pOH = 14pH = 7 (Neutral)pH + 1 = 14pH = 13 (Alkaline) pOH with Conc OH-pOH = -log [OH-]pH with Conc H+ [OH-] = 0.0000001MpH = -log [H+] pOH = -log [0.0000001][H+] = 0.01M pOH = -log1010-7pH = -log [0.01] pOH = 7pH = -log1010-2 pH + pOH = 14pH = 2 (Acidic) pH + 7 = 14 pH = 7 (Neutral) 20. pH measurement of Acidity of solution pH is the measure of acidity of a solution in logarithmic scalepH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration Acidic pH < 7Alkaline pH > 7 pOH with Conc OH-pH with Conc H+pOH = -log [OH-]pH = -log [H+] [OH-] = 0.1M[H+] = 0.0000001MpOH = -log[0.1]pH = -log [0.0000001]pOH = 1pH = -log1010-7pH + pOH = 14pH = 7 (Neutral) pH + 1 = 14 pH = 13 (Alkaline)pOH with Conc OH- pOH = -log [OH-]pH with Conc H+[OH-] = 0.0000001MpH = -log [H+]pOH = -log [0.0000001][H+] = 0.01MpOH = -log1010-7pH = -log [0.01]pOH = 7pH = -log1010-2pH + pOH = 14pH = 2 (Acidic)pH + 7 = 14pH = 7 (Neutral) Conc H+ increase by 10x pH decrease by 1 unit Conc OH- increase by 10x pH increase by 1 unit 21. pH measurement of Acidity of solution pH is the measure of acidity of a solution in logarithmic scalepH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration Acidic pH < 7Alkaline pH > 7 pOH with Conc OH-pH with Conc H+pOH = -log [OH-]pH = -log [H+] [OH-] = 0.1M[H+] = 0.0000001MpOH = -log[0.1]pH = -log [0.0000001]pOH = 1pH = -log1010-7pH + pOH = 14pH = 7 (Neutral) pH + 1 = 14 pH = 13 (Alkaline)pOH with Conc OH- pOH = -log [OH-]pH with Conc H+[OH-] = 0.0000001MpH = -log [H+]pOH = -log [0.0000001][H+] = 0.01MpOH = -log1010-7pH = -log [0.01]pOH = 7pH = -log1010-2pH + pOH = 14pH = 2 (Acidic)pH + 7 = 14pH = 7 (Neutral) Conc H+ increase by 10x pH decrease by 1 unit Conc OH- increase by 10x pH increase by 1 unit Easier using pH scale than Conc [H+] Conc H+ increase 10x from 0.0001(10-4) to 0.001(10-3)- pH change by 1 unit from pH 4 to 3 pH 3 is (10x) more acidic than pH 4 1 unit change in pH is 10 fold change in Conc [H+] 22. pH measurement of Acidity of solution pH is the measure of acidity of a solution in logarithmic scalepH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration Acidic pH < 7Alkaline pH > 7 pOH with Conc OH-pH with Conc H+pOH = -log [OH-]pH = -log [H+] [OH-] = 0.1M[H+] = 0.0000001MpOH = -log[0.1]pH = -log [0.0000001]pOH = 1pH = -log1010-7pH + pOH = 14pH = 7 (Neutral) pH + 1 = 14 pH = 13 (Alkaline)pOH with Conc OH- pOH = -log [OH-]pH with Conc H+[OH-] = 0.0000001MpH = -log [H+]pOH = -log [0.0000001][H+] = 0.01MpOH = -log1010-7pH = -log [0.01]pOH = 7pH = -log1010-2pH + pOH = 14pH = 2 (Acidic)pH + 7 = 14pH = 7 (Neutral) Conc H+ increase by 10x pH decrease by 1 unit Conc OH- increase by 10x pH increase by 1 unit Easier using pH scale than Conc [H+] Conc H+ increase 10x from 0.0001(10-4) to 0.001(10-3)- pH change by 1 unit from pH 4 to 3 Easier scale pH 3 is (10x) more acidic than pH 4 1 unit change in pH is 10 fold change in Conc [H+] 23. pH measurement of Acidity of solutionH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kc = [H3O+][OH]/[H2O]2Kw - dissociation constant water Kc [H2O]2 = [H3O+][OH] - ionic product waterDissociation H2O small, conc [H2O] is constantKc [H2O]2 is constant called Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25CKw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 24. pH measurement of Acidity of solutionH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kc = [H3O+][OH]/[H2O]2Kw - dissociation constant water Kc [H2O]2 = [H3O+][OH]- ionic product waterDissociation H2O small, conc [H2O] is constantKc [H2O]2 is constant called Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25CKw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7Formula for acid/base calculationpH = -log10[H+]pOH = -log10[OH-]pH + pOH = 14Kw = [H+][OH-] 25. pH measurement of Acidity of solutionH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kc = [H3O+][OH]/[H2O]2Kw - dissociation constant water Kc [H2O]2 = [H3O+][OH]- ionic product waterDissociation H2O small, conc [H2O] is constantKc [H2O]2 is constant called Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25CKw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7Using conc [H+]pH = -log10[H+]Formula for acid/base calculationpH = -log10[H+]pOH = -log10[OH-]pH + pOH = 14Kw = [H+][OH-] 26. pH measurement of Acidity of solution H2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kc = [H3O+][OH]/[H2O]2Kw - dissociation constant water Kc [H2O]2 = [H3O+][OH]- ionic product water Dissociation H2O small, conc [H2O] is constant Kc [H2O]2 is constant called Kw = [H3O+][OH] Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH] 1.0 x 10-14 = [H3O+][OH]Alkaline 1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7]Conc [H+] = 1 x 10-12[H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7pH = -lg[H+]pH = -lg [10-12]pH = 12Using conc [H+]pH = -log10[H+]AcidicConc [H+] = 1 x 10-2pH = -lg[H+]pH = -lg [10-2]pH = 2 Formula for acid/base calculation pH = -log10[H+]pOH = -log10[OH-]pH + pOH = 14Kw = [H+][OH-] 27. pH measurement of Acidity of solution H2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kc = [H3O+][OH]/[H2O]2Kw - dissociation constant water Kc [H2O]2 = [H3O+][OH]- ionic product water Dissociation H2O small, conc [H2O] is constant Kc [H2O]2 is constant called Kw = [H3O+][OH] Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH] 1.0 x 10-14 = [H3O+][OH]Alkaline 1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7]Conc [H+] = 1 x 10-12[H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7pH = -lg[H+]pH = -lg [10-12]pH = 12Using conc [H+] Using conc [OH-]pH = -log10[H+] pOH = -log10[OH-]AcidicConc [H+] = 1 x 10-2pH = -lg[H+]pH = -lg [10-2]pH = 2 Formula for acid/base calculation pH = -log10[H+]pOH = -log10[OH-]pH + pOH = 14Kw = [H+][OH-] 28. pH measurement of Acidity of solution H2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kc = [H3O+][OH]/[H2O]2Kw - dissociation constant water Kc [H2O]2 = [H3O+][OH]- ionic product water Dissociation H2O small, conc [H2O] is constant Kc [H2O]2 is constant called Kw = [H3O+][OH] Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH] 1.0 x 10-14 = [H3O+][OH] AlkalineAlkaline 1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7]Conc [OH-] = 1 x 10-2Conc [H+] = 1 x 10-12[H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7pOH = -log10[OH-]pH = -lg[H+] = -log1010-2pH = -lg [10-12]pOH = 2pH = 12pH + pOH = 14pH + 2 = 14pH = 12Using conc [H+] Using conc [OH-]pH = -log10[H+] pOH = -log10[OH-] AcidicAcidicConc [OH-] = 1 x 10-12 -2Conc [H+] = 1 x 10pOH = -log10[OH-]pH = -lg[H+] = -log1010-12pH = -lg [10-2] pOH = 12pH = 2pH + pOH = 14pH + 12 = 14pH = 2 Formula for acid/base calculation pH = -log10[H+]pOH = -log10[OH-]pH + pOH = 14Kw = [H+][OH-] 29. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 30. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7H2O + H2O H3O+ + OH H = +57kJ/molKw - Dissociation water is endothermic and Temp dependentH2O + H2O H3O+ + OH H = +57kJ/molKw = [H3O+][OH]Temp increases, equilibrium shift to right (endo), so more ions form, Kw increases 31. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 H2O + H2O H3O+ + OH H = +57kJ/mol Kw - Dissociation water is endothermic and Temp dependent H2O + H2O H3O+ + OH H = +57kJ/mol Kw = [H3O+][OH] Temp increases, equilibrium shift to right (endo), so more ions form, Kw increases Temp - shift to right more H+/OH- Kw 32. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 H2O + H2O H3O+ + OH H = +57kJ/mol Kw - Dissociation water is endothermic and Temp dependent H2O + H2O H3O+ + OH H = +57kJ/mol Kw = [H3O+][OH] Temp increases, equilibrium shift to right (endo), so more ions form, Kw increases Temp - shift to right more H+/OH- Kw Temp - Kw H+ ion - pH 33. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 H2O + H2O H3O+ + OH H = +57kJ/mol Kw - Dissociation water is endothermic and Temp dependent H2O + H2O H3O+ + OH H = +57kJ/mol Kw = [H3O+][OH] Temp increases, equilibrium shift to right (endo), so more ions form, Kw increases Temp - shift to right more H+/OH- Kw Temp - Kw H+ ion - pH At 25C, Kw - 1.0 x 10-14 Kw = [H+][OH] 1.0 x 10-14 = [H+][OH] [H+][OH] = [10-7][10-7] pH = -lg[H+] pH = -lg [1.0 x 10-7] Neutral pH = 7 At 25C - pH 7 is NEUTRAL Conc of [H+] and [OH] the same [H+] = [OH-] = 1.00 x 10-7 34. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 H2O + H2O H3O+ + OH H = +57kJ/mol Kw - Dissociation water is endothermic and Temp dependent H2O + H2O H3O+ + OH H = +57kJ/mol Kw = [H3O+][OH] Temp increases, equilibrium shift to right (endo), so more ions form, Kw increases Temp - shift to right more H+/OH- Kw Temp - Kw H+ ion - pH At 25C, Kw - 1.0 x 10-14 At 50C, Kw - 9.3 x 10-14 Kw = [H+][OH]Kw = [H+][OH] 1.0 x 10-14 = [H+][OH]9.3 x 10-14 = [H+][OH] [H+][OH] = [10-7][10-7] [H+]2 = 9.3 x 10-14 pH = -lg[H+] [H+] = 3.05 x 10-7 pH = -lg [1.0 x 10-7] pH = -lg[3.05 x 10-7] Neutral pH = 7 Neutral pH = 6.5 At 25C - pH 7 is NEUTRALAt 50C - pH 6.5 is NEUTRAL Conc of [H+] and [OH] the same Conc of [H+] and [OH] the same [H+] = [OH-] = 1.00 x 10-7 [H+] = [OH-] = 3.05 x 10-7 35. Dissociation Constant or Ionic Product Constant Water, KwH2O dissociate forming H3O+ and OH- (equilibrium exist) H2O + H2O H3O+ + OH Kw = [H3O+][OH]/[H2O]2Dissociation H2O is small, conc [H2O] is constant - Kw = [H3O+][OH]Kw = 1.0 x 10-14 mol2 dm-6 - dissociation constant water at -25C Kw = [H3O+][OH]1.0 x 10-14 = [H3O+][OH]1.0 x 10-14 = [1.0 x 10-7][1.0 x 10-7][H3O+]= 1.0 x 10-7, [OH-] = 1.0 x 10-7 H2O + H2O H3O+ + OH H = +57kJ/mol Kw - Dissociation water is endothermic and Temp dependent H2O + H2O H3O+ + OH H = +57kJ/mol Kw = [H3O+][OH] Temp increases, equilibrium shift to right (endo), so more ions form, Kw increases Temp - shift to right more H+/OH- Kw Temp - Kw H+ ion - pH Relationship Temp / Kw /Neutral pH At 25C, Kw - 1.0 x 10-14 At 50C, Kw - 9.3 x 10-14 Kw = [H+][OH]Kw = [H+][OH] 1.0 x 10-14 = [H+][OH]9.3 x 10-14 = [H+][OH] [H+][OH] = [10-7][10-7] [H+]2 = 9.3 x 10-14 pH = -lg[H+] [H+] = 3.05 x 10-7 pH = -lg [1.0 x 10-7] pH = -lg[3.05 x 10-7] Neutral pH = 7 Neutral pH = 6.5 At 25C - pH 7 is NEUTRALAt 50C - pH 6.5 is NEUTRAL Conc of [H+] and [OH] the same Conc of [H+] and [OH] the same [H+] = [OH-] = 1.00 x 10-7 [H+] = [OH-] = 3.05 x 10-7 36. Acid/base CalculationFormula acid/base calculation pH = -log10[H+]pOH = -log10[OH-]pH + pOH = 14 Kw = [H+][OH-] What is the pH for [H+] = 10-12 MWhat is the pH for [OH-] = 0.1 MWhat is the conc of H+ in solution with pH 3?Calculate conc of OH- and pH for 0.001 HCI. HCI H+ + CI- (100% dissociate)0.0010.001Calculate conc of OH- when 3.o x 10-4 [H+] was added to pure waterHCI H+ + CI- (100% dissociate) -43.o x 103.o x 10-4What is the pH of 1.0M NaOH ?NaOH Na+ + OH- (100% dissociate)1M1M 1M 37. Acid/base CalculationFormula acid/base calculation pH = -log10[H+]pOH = -log10[OH-] pH + pOH = 14Kw = [H+][OH-] What is the pH for [H+] = 10-12 M What is the pH for [OH-] = 0.1 M What is the conc of H+ in solution with pH 3? pH = -lg[H+]pOH = -lg[OH-] pH = -lg[H+] pH = -lg [10-12]pOH = -lg [0.1] 3 = -lg[H+] pH = 12 pOH = 1[H+] = 10 pH pH + pOH = 14[H+] = 10 -3 pH = 14 1 = 13Calculate conc of OH- and pH for 0.001 HCI. HCI H+ + CI- (100% dissociate)0.001 0.001Kw = [H+][OH]= 10-14 (assume all H+ from HCI and H+ from water is negligible) [0.001][OH-]= 10-14 [OH-] = 10-14/0.001 = 10 -11pH = -log1o[H]+ =-log10o.oo1pH = 3Calculate conc of OH- when 3.o x 10-4 [H+] was added to pure waterHCI H+ + CI- (100% dissociate) -43.o x 103.o x 10-4Kw = [H+][OH] = 10-14 (assume all H+ from HCI and H+ from water is negligible)[OH] = 10-14 = 10 -14= 3.3 x 10 -11 M+ -4 [H ]3.o x 10What is the pH of 1.0M NaOH ?NaOH Na+ + OH- (100% dissociate)1M 1M1MKw = [H3O+][OH] = 10-14 (assume all OH- from NaOH and OH- from water is negligible)[H+] = 10-14 = 10 -14 = 1.0 x 10 -14[OH] 1.0pH = -log [H+]pH = -log [1.0 x 10 -14]pH = 14 38. Questions on Acids and Base1 Which list contains only strong acids ?A. CH3COOH, H2CO3, H3PO4B. HCI, HNO3, H2CO3C. CH3COOH, HNO3, H2SO4D. HCI, HNO3, H2SO42 When equal volume of four 1M solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?A. CH3COOH < HNO3 < CH3CH2NH2 < KOHB. HNO3 < CH3COOH < CH3CH2NH2 < KOHC. CH3CH2NH2 < HNO3 < CH3COOH < KOHD. KOH < CH3CH2NH2 < CH3COOH < HNO33 100ml of NaOH solution of pH 12 is mixed with 900ml of water. What is the pH of resulting solution?A. 1B. 3C. 11D. 134 Solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement is correct ?A. Acid A is stronger than acid BB. [A] > [B]C. Concentration of H+ ions in A is higher than BD. Concentration of H+ ions in B is twice the concentration of H+ in A5pH of a solution changes from pH =2 to pH =5. What happens to the concentration of H+ ions during this pH change? A. Decrease by factor of 1000 B. Increase by factor of 1000 C. Decrease by factor of 100 D. Increase by a factor of 1006List two ways to distinguish between strong and weak acid/base 39. Questions on Acids and Base1 Which list contains only strong acids ?A. CH3COOH, H2CO3, H3PO4B. HCI, HNO3, H2CO3C. CH3COOH, HNO3, H2SO4D. HCI, HNO3, H2SO42 When equal volume of four 1M solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?A. CH3COOH < HNO3 < CH3CH2NH2 < KOHB. HNO3 < CH3COOH < CH3CH2NH2 < KOHC. CH3CH2NH2 < HNO3 < CH3COOH < KOHD. KOH < CH3CH2NH2 < CH3COOH < HNO33 100ml of NaOH solution of pH 12 is mixed with 900ml of water. What is the pH of resulting solution?A. 1B. 3C. 11D. 134 Solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement is correct ?A. Acid A is stronger than acid BB. [A] > [B]C. Concentration of H+ ions in A is higher than BD. Concentration of H+ ions in B is twice the concentration of H+ in A5pH of a solution changes from pH =2 to pH =5. What happens to the concentration of H+ ions during this pH change?A. Decrease by factor of 1000 B. Increase by factor of 1000 C. Decrease by factor of 100 D. Increase by a factor of 1006List two ways to distinguish between strong and weak acid/base By Conductivity measurement By pH measurement1M Strong Acid Ionise completely More H+ ion Conductivity higher 1M Strong Acid Ionise completely More H+ ion pH lower 1M Weak Acid Ionise partially Less H+ ion Conductivity lower 1M Weak Acid Ionise partially Less H+ ion pH higher 40. Video on Acid/ Base Click here on pH varies with temperatureClick here on pKa and pKb calculationClick here on pH calculationClick here on Bronsted Lowry/ Lewis Acid/BaseClick here on Lewis Acid/Base 41. AcknowledgementsThanks to source of pictures and video used in this presentationThanks to Creative Commons for excellent contribution on licenseshttp://creativecommons.org/licenses/Prepared by Lawrence KokCheck out more video tutorials from my site and hope you enjoy this tutorialhttp://lawrencekok.blogspot.com