1. Tutorial on Indicators and Salt Hydrolysis. Prepared by Lawrence Kok http://lawrencekok.blogspot.com

2. Acid Base Indicators IndicatorsIndicatorpKa pH ColourColour Organic dye of weak acid/weak base with pKa/pKb value rangeAcidBase Detect equivalence point in titration HIn as indicator have 2 different colours in acidic/alkaline mediumMethyl orange 3.46 3.2- 4.4 REDYellowBromophenol Blue4.10 3.0- 4.6Yellow BlueHIn H+ + In-(red) (blue)Bromocresol Green 4.90 3.8- 5.4Yellow Blue Methyl Red 5.00 4.8- 6.0Red YellowacidbaseBromothymol Blue7.30 6.0- 7.6Yellow Blue Phenol Red 8.00 6.6- 8.2Yellow Red Phenolphthalein9.508.2-ColourlessPink Presence of acid, H+ Presence of base, OH- 10.0 HIn H+ + In- HIn H+ + In-(H+ ions ) - Equilibrium shift to left(H+ions ) - Equilibrium shift to right More [HIn ] red , [HIn] > [In-] More [In- ] blue, [In-] > [HIn] 3. Acid Base Indicators IndicatorsIndicatorpKa pH ColourColour Organic dye of weak acid/weak base with pKa/pKb value rangeAcidBase Detect equivalence point in titration HIn as indicator have 2 different colours in acidic/alkaline mediumMethyl orange 3.46 3.2- 4.4 REDYellowBromophenol Blue4.10 3.0- 4.6Yellow BlueHIn H+ + In-(red) (blue)Bromocresol Green 4.90 3.8- 5.4Yellow Blue Methyl Red 5.00 4.8- 6.0Red YellowacidbaseBromothymol Blue7.30 6.0- 7.6Yellow Blue Phenol Red 8.00 6.6- 8.2Yellow Red Phenolphthalein9.508.2-ColourlessPink Presence of acid, H+ Presence of base, OH- 10.0 HIn H+ + In- HIn H+ + In-(H+ ions ) - Equilibrium shift to left(H+ions ) - Equilibrium shift to right More [HIn ] red , [HIn] > [In-] More [In- ] blue, [In-] > [HIn] HIn HIn H+ + In- In- 4. Acid Base Indicators IndicatorsIndicatorpKa pH ColourColour Organic dye of weak acid/weak base with pKa/pKb value rangeAcidBase Detect equivalence point in titration HIn as indicator have 2 different colours in acidic/alkaline mediumMethyl orange 3.46 3.2- 4.4 REDYellowBromophenol Blue4.10 3.0- 4.6Yellow BlueHIn H+ + In-(red) (blue)Bromocresol Green 4.90 3.8- 5.4Yellow Blue Methyl Red 5.00 4.8- 6.0Red YellowacidbaseBromothymol Blue7.30 6.0- 7.6Yellow Blue Phenol Red 8.00 6.6- 8.2Yellow Red Phenolphthalein9.508.2-ColourlessPink Presence of acid, H+ Presence of base, OH- 10.0 HIn H+ + In- HIn H+ + In-(H+ ions ) - Equilibrium shift to left(H+ions ) - Equilibrium shift to right More [HIn ] red , [HIn] > [In-] More [In- ] blue, [In-] > [HIn] HIn HIn H+ + In- In- Presence of acid, H+[HIn] > [In-]RED 5. Acid Base Indicators IndicatorsIndicatorpKa pH ColourColour Organic dye of weak acid/weak base with pKa/pKb value rangeAcidBase Detect equivalence point in titration HIn as indicator have 2 different colours in acidic/alkaline medium Methyl orange3.46 3.2- 4.4 REDYellow Bromophenol Blue 4.10 3.0- 4.6Yellow BlueHIn H+ + In-(red) (blue) Bromocresol Green4.90 3.8- 5.4Yellow Blue Methyl Red 5.00 4.8- 6.0Red Yellowacidbase Bromothymol Blue 7.30 6.0- 7.6Yellow Blue Phenol Red 8.00 6.6- 8.2Yellow RedPhenolphthalein 9.508.2-ColourlessPink Presence of acid, H+ Presence of base, OH- 10.0 HIn H+ + In- HIn H+ + In-(H+ ions ) - Equilibrium shift to left(H+ions ) - Equilibrium shift to right More [HIn ] red , [HIn] > [In-] More [In- ] blue, [In-] > [HIn] HIn HIn H+ + In- In- Presence of acid, H+ Presence of base, OH-[HIn] > [In-][In-] > [HIn]REDBLUE 6. Acid Base IndicatorsIndicatorsIndicatorpKapH ColourColour Organic dye of weak acid/weak base with pKa/pKb valuerangeAcidBase Detect equivalence point in titration HIn as indicator have 2 different colours in acidic/alkaline medium Methyl orange3.463.2- 4.4 REDYellowBromophenol Blue4.103.0- 4.6 Yellow Blue HIn H+ + In- (red) (blue) Bromocresol Green4.903.8- 5.4Yellow BlueMethyl Red 5.00 4.8- 6.0 Red Yellow acid baseBromothymol Blue 7.30 6.0- 7.6 Yellow BluePhenol Red 8.00 6.6- 8.2 Yellow Red Phenolphthalein 9.50 8.2-Colourless PinkPresence of acid, H+Presence of base, OH- 10.0HIn H+ + In-HIn H+ + In- (H+ ions ) - Equilibrium shift to left (H+ions ) - Equilibrium shift to right More [HIn ] red , [HIn] > [In-]More [In- ] blue, [In-] > [HIn]HInHIn H+ + In-In-Presence of acid, H+ Presence of base, OH- [HIn] > [In-][HIn] = [In-] [In-] > [HIn] REDRED + BlUEBLUE HIn H+ + In- (red) (blue) Ka = (H+)(In-)(HIn)(HIn) = (H+) (In-)Ka [HIn] = [In-] x log H+ = KaEquivalence Pointboth sides-lgH+ = -lg KaStart to change colourpH = pKaHIn = In- pH = pKa Two colours red/blue will have equal conc,Click here on indicator notes from chem guide Indicator have colour in bet red and blue (start to change colour)Click here on detail acid/base notes 7. Acid Base Indicators Indicators change colour at its pKa but it cannot be detected by our eyes IndicatorpKapH ColourColour pH range Indicator changes colour over a range of pH rangeAcidBase Methyl orange, pKa is 3.46 but change colour in the range of pH (3.2-4.4) pH range (pH = pKa 1) seen by our eyeMethyl orange 3.463.2- 4.4 RED Yellow Indicator must only change colour at equivalence point Bromophenol Blue4.10 3.0- 4.6 YellowBlue End point of indicator must correspond/coincide with equivalence point Colour change must occur rapidly at equivalence pointBromocresol Green 4.903.8- 5.4YellowBlue Indicator usually change colour over a region of 2 pH units centered on pKaMethyl Red 5.00 4.8- 6.0Red Yellow Bromothymol Blue7.30 6.0- 7.6 YellowBluePhenol Red 8.00 6.6- 8.2 YellowPinkPhenolphthalein9.50 8.2- 10.0ColourlessPink Equivalence PointEnd PointAmt of acid = Amt baseIndicator change(Neutralization) colour 8. Acid Base Indicators Indicators change colour at its pKa but it cannot be detected by our eyes IndicatorpKapH Colour Colour pH range Indicator changes colour over a range of pH rangeAcid Base Methyl orange, pKa is 3.46 but change colour in the range of pH (3.2-4.4) pH range (pH = pKa 1) seen by our eyeMethyl orange 3.463.2- 4.4 RED Yellow Indicator must only change colour at equivalence point Bromophenol Blue4.10 3.0- 4.6 YellowBlue End point of indicator must correspond/coincide with equivalence point Colour change must occur rapidly at equivalence pointBromocresol Green 4.903.8- 5.4YellowBlue Indicator usually change colour over a region of 2 pH units centered on pKaMethyl Red 5.00 4.8- 6.0Red Yellow Bromothymol Blue7.30 6.0- 7.6 YellowBlueMethyl Orange IndicatorPhenol Red 8.00 6.6- 8.2 YellowPinkIndicatorpKapHColourColourPhenolphthalein9.50 8.2- 10.0ColourlessPink range AcidBase Equivalence PointEnd PointMethyl orange3.46 3.2- 4.4 REDYellowAmt of acid = Amt baseIndicator change(Neutralization) colourAcidBase pH 3.2 pH 4.4pH 14pH 1 Phenol Red IndicatorpKapHColourColourrange AcidBase Phenol Red 8.006.6- 8.2 YellowPinkAcidBase pH 1pH 6.6pH 8.2 pH 14 9. Acid Base Indicators Indicators change colour at its pKa but it cannot be detected by our eyesIndicator pKapH Colour Colour pH range Indicator changes colour over a range of pH rangeAcid Base Methyl orange, pKa is 3.46 but change colour in the range of pH (3.2-4.4) pH range (pH = pKa 1) seen by our eyeMethyl orange 3.463.2- 4.4 RED Yellow Indicator must only change colour at equivalence point Bromophenol Blue4.10 3.0- 4.6 YellowBlue End point of indicator must correspond/coincide with equivalence point Colour change must occur rapidly at equivalence pointBromocresol Green 4.903.8- 5.4YellowBlue Indicator usually change colour over a region of 2 pH units centered on pKa Methyl Red5.00 4.8- 6.0Red Yellow Bromothymol Blue7.30 6.0- 7.6 YellowBlueMethyl Orange Indicator Phenol Red8.00 6.6- 8.2 YellowPinkIndicatorpKapHColourColour Phenolphthalein 9.50 8.2- 10.0ColourlessPink range AcidBase Equivalence PointEnd PointMethyl orange3.46 3.2- 4.4 REDYellowAmt of acid = Amt baseIndicator change(Neutralization) colourAcid Base pH 3.23.46pH 4.4 pH 14pH 1Indicator change colour at its pKaIndicator do not change colour at pH 7 Phenol Red IndicatorpKapHColourColourrange AcidBase Phenol Red 8.006.6- 8.2 YellowPinkAcidBase 8 pH 1 pH 6.6pH 8.2pH 14Indicator changes colour at its pKaIndicator do not change colour at pH 7 10. Acid Base Indicators Indicators change colour at its pKa but it cannot be detected by our eyesIndicatorpKa pH Colour Colour pH range Indicator changes colour over a range of pH rangeAcid Base Methyl orange, pKa is 3.46 but change colour in the range of pH (3.2-4.4) pH range (pH = pKa 1) seen by our eyeMethyl orange 3.463.2- 4.4 RED Yellow Indicator must only change colour at equivalence pointBromophenol Blue 4.10 3.0- 4.6 YellowBlue End point of indicator must correspond/coincide with equivalence point Colour change must occur rapidly at equivalence pointBromocresol Green4.90 3.8- 5.4YellowBlue Indicator usually change colour over a region of 2 pH units centered on pKa Methyl Red5.00 4.8- 6.0Red Yellow Bromothymol Blue7.30 6.0- 7.6 YellowBlueMethyl Orange Indicator Phenol Red 8.006.6- 8.2 YellowPinkIndicatorpKapHColourColour Phenolphthalein 9.50 8.2- 10.0ColourlessPink range AcidBase Equivalence PointEnd PointMethyl orange3.46 3.2- 4.4 REDYellowAmt of acid = Amt baseIndicator change(Neutralization) colourAcidBase pH 3.23.46pH 4.4 pH 14pH 1 pH range(3.2 4.4)pH range changes colour over a range of pHIndicator change colour at its pKaIndicator do not change colour at pH 7 Phenol Red IndicatorpKapHColourColourrange AcidBase Phenol Red 8.006.6- 8.2 Yellow PinkAcidBase 8 pH 1 pH 6.6pH 8.2pH 14 pH range(6.6 8.0)Indicator changes colour at its pKa pH range changes colour over a range of pHIndicator do not change colour at pH 7 11. Acid Base Indicators HIn Indicator IndicatorColourpKapH range Colour AcidBase HIn RED 4.53.5 5.5BLUE Indicator change Range of pH indicator colour at pKachange colour 4.5pH 1pH 3.5pH 5.5 pH 14 HIn HIn H+ + In- In- 12. Acid Base Indicators HIn IndicatorIndicatorColourpKapH range ColourAcidBase HInRED 4.53.5 5.5BLUEIndicator change Range of pH indicatorcolour at pKachange colour4.5pH 1 pH 3.5pH 5.5 pH 14 HInHIn H+ + In- In- pH 3.5, eye detects it REDConc [Hin] > [In-] by 10x[HIn] = 10[In-] 1 [HIn] > [In-] by 10xKa = (H+)(In-) [HIn] =10(HIn) [In-]1H+ = Ka x (HIn) = Ka x 10(In-)H + = 10Ka-lgH+ = -lg 10 - lgKapH = -1 + pKapH = -1 + 4.5pH = 3.5 13. Acid Base Indicators HIn IndicatorIndicatorColourpKapH range ColourAcidBase HInRED 4.53.5 5.5BLUEIndicator change Range of pH indicatorcolour at pKachange colour4.5pH 1 pH 3.5pH 5.5 pH 14 HInHIn H+ + In- In- pH 3.5, eye detects it RED pH 5.5, eye detects it BLUEConc [Hin] > [In-] by 10x Conc [Hin] < [In-] by 10x[HIn] = 10 [HIn] = 1[In-] 1[In-]10 [HIn] > [In-] by 10x [In-] > [HIn] by 10xKa = (H+)(In-) Ka = (H+)(In-) [HIn] =10[HIn] = 1(HIn) [In-]1 (HIn) [In-]10H+ = Ka x (HIn) = Ka x 10H+ = Ka x (HIn) = Ka x 1/10(In-)(In-)H + = 10KH + = K /10a a-lgH+ = -lg 10 - lgKa-lgH+ = - lgKa - lg10-1pH = -1 + pKapH = pKa + 1pH = -1 + 4.5pH = 4.5 + 1 = 5.5pH = 3.5 pH = 5.5, 14. Acid Base Indicators HIn IndicatorIndicatorColourpKapH rangeColourAcid Base HInRED 4.5 3.5 5.5BLUEIndicator changeRange of pH indicatorcolour at pKa change colour 4.5pH 1 pH 3.5 pH 5.5 pH 14 HInHIn H+ + In-In- pH 3.5, eye detects it RED [HIn] = [In-] pH 5.5, eye detects it BLUERED + BLUEConc [Hin] > [In-] by 10xConc [Hin] < [In-] by 10x[HIn] = 10 [HIn] = 1[HIn] = 1[In-] 1[In-] 1[In-]10 [HIn] > [In-] by 10x [HIn] = [In-][In-] > [HIn] by 10xKa = (H+)(In-) [HIn] =10HIn H+ + In-Ka = (H+)(In-) [HIn] = 1(HIn) [In-]1(red)(Blue) (HIn) [In-]10 Ka = (H+)(In-)H+ = Ka x (HIn) = Ka x 10(HIn)[HIn] = 1 H+ = Ka x (HIn) = Ka x 1/10 [In-]1(In-) (H +) = (HIn) (In-)H + = 10K -)H + = K /10aKa(In a-lgH+ = -lg 10 - lgKa H+ = Ka -lgH+ = - lgKa - lg10-1pH = -1 + pKa -lgH+ = -lg KapH = pKa + 1pH = -1 + 4.5 pH = pKapH = 4.5 + 1 = 5.5pH = 3.5pH = 4.5 (pKa of indicator) pH = 5.5, pH = 4.5 pKa of HIn, indicator change colour (end point) from red to blue Red turn blue but cannot be detected by our eyes Indicator change colour over a region of 2 pH units centerd on pKa 15. Titration curves Strong Acid with Strong Base HCI+ NaOH NaCI + H2OM = 0.1M M = 0.1M Mole ratio 1: 1Titration between strong acid(flask) with strong base(burette) NaOH V = 25ml V = 25mlHCI + NaOH NaCI + H2O M = 0.1MV = 25ml Rapid jump in pH (2.7 11.3) Rapid change at equivalence point (25ml base) Equivalence point amt acid = amt base HCI End point indicator change colour M = 0.1M Equvalence point must coincide with end point at 25ml V = 25ml pH at equivalence point = 7 Neutral salt, NaCI - neutral 2.7 1V = 25mlNaOHNaOH M = 0.1MM = 0.1M V = 0 mlV = 24 ml added HCIHCI M = 0.1M M = 0.1M V = 25ml V = 1ml left pH = 1 pH = 2.7Acidic medium Indicator pKa pH rangeColourAcid Methyl orange 3.46 3.2- 4.4REDBromophenol Blue 4.10 3.0- 4.6YellowBromocresol Green4.90 3.8- 5.4Yellow Methyl Red5.00 4.8- 6.0 RedBromothymol Blue 7.30 6.0- 7.6Yellow Phenol Red8.00 6.6- 8.0Yellow Phenolphthalein 9.508.2- 10.0Colourless 16. Titration curves Strong Acid with Strong BaseHCI + NaOH NaCI + H2OM = 0.1MM = 0.1MMole ratio 1: 1Titration between strong acid(flask) with strong base(burette)NaOHV = 25mlV = 25mlHCI + NaOH NaCI + H2OM = 0.1M V = 25ml Rapid jump in pH (2.7 11.3) Rapid change at equivalence point (25ml base) 11.3 Equivalence point amt acid = amt baseHCI End point indicator change colourM = 0.1M Equvalence point must coincide with end point at 25mlV = 25ml pH at equivalence point = 7 7 Neutral salt, NaCI - neutral 2.7 1 V = 25ml NaOHNaOHNaOH NaOHM = 0.1MM = 0.1M M = 0.1M M = 0.1M V = 25ml addedV = 26ml V = 0 ml V = 24 ml added HCI HCIHCIM = 0.1M NaOH M = 0.1M M = 0.1M V = 0ml left V = 1ml left V = 25ml V = 1ml leftpH = 7pH = 11.3 pH = 1 pH = 2.7Acidic medium Indicator pKa pH range Colour Acid Methyl orange 3.463.2- 4.4REDBromophenol Blue 4.103.0- 4.6YellowBromocresol Green4.903.8- 5.4Yellow Methyl Red5.004.8- 6.0 RedBromothymol Blue 7.306.0- 7.6Yellow Phenol Red8.006.6- 8.0Yellow Phenolphthalein 9.508.2- 10.0 Colourless 17. Titration curves Strong Acid with Strong Base HCI+ NaOH NaCI + H2O M = 0.1M M = 0.1MMole ratio 1: 1Titration between strong acid(flask) with strong base(burette)NaOH V = 25ml V = 25mlHCI + NaOH NaCI + H2OM = 0.1M V = 25ml Rapid jump in pH (2.7 11.3) Rapid change at equivalence point (25ml base) 11.3 Equivalence point amt acid = amt base HCI End point indicator change colour M = 0.1M Equvalence point must coincide with end point at 25ml V = 25ml pH at equivalence point = 7 7 Neutral salt, NaCI - neutral 2.7 1 V = 25ml NaOHNaOHNaOH NaOHM = 0.1MM = 0.1M M = 0.1M M = 0.1M V = 25ml addedV = 26ml V = 0 ml V = 24 ml addedHCI HCIHCI M = 0.1MNaOH M = 0.1M M = 0.1MV = 0ml leftV = 1ml left V = 25ml V = 1ml left pH = 7pH = 11.3 pH = 1 pH = 2.7Basic mediumAcidic medium Indicator pKa pH range ColourIndicatorpKa pH rangeColour Acid Base Methyl orange 3.463.2- 4.4RED Methyl orange 3.46 3.2- 4.4YellowBromophenol Blue 4.103.0- 4.6YellowBromophenol Blue4.10 3.0- 4.6 BlueBromocresol Green4.903.8- 5.4YellowBromocresol Green 4.90 3.8- 5.4 Blue 25ml base added: Methyl Red5.004.8- 6.0 Red Equivalence point reachMethyl Red 5.00 4.8- 6.0Yellow Indicator change colourBromothymol Blue 7.306.0- 7.6YellowBromothymol Blue7.30 6.0- 7.6 Blue Phenol Red8.006.6- 8.0Yellow Phenol Red 8.00 6.6- 8.0 Red Phenolphthalein 9.508.2- 10.0 Colourless Phenolphthalein9.508.2- 10.0 Pink 18. Titration curves Strong Acid with Strong BaseTitration between strong acid(flask) with strong base(burette)Indicator pKa pH range Colour Colour HCI + NaOH NaCI + H2O Change ChangeAcid Base 11.3 NaOHM = 0.1MMethyl orange 3.46 3.2- 4.4REDYellowV = 25mlBromophenol Blue4.10 3.0- 4.6 Yellow Blue 7Bromocresol Green 4.90 3.8- 5.4 Yellow Blue Methyl Red 5.00 4.8- 6.0 Red Yellow 2.7HCI Bromothymol Blue7.30 6.0- 7.6 Yellow Blue1 M = 0.1M V = 25ml V = 25ml Phenol Red 8.00 6.6- 8.0 Yellow RedEquivalence point occurs when 25ml base addedPhenolphthalein9.50 8.2- 10.0 ColourlessPink pH rise sharply (2.7 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (2.7 11.3) suitable Equivalence Point and End Point coincide when 25ml base added. 19. Titration curves Strong Acid with Strong BaseTitration between strong acid(flask) with strong base(burette) IndicatorpKapH range ColourColour HCI + NaOH NaCI + H2OChangeChange AcidBase 11.3 NaOHM = 0.1MMethyl orange 3.463.2- 4.4 REDYellowV = 25mlBromophenol Blue 4.10 3.0- 4.6 YellowBlue 7 Bromocresol Green4.903.8- 5.4 YellowBlue Methyl Red 5.004.8- 6.0 RedYellow 2.7HCIBromothymol Blue 7.306.0- 7.6 YellowBlue1 M = 0.1M V = 25ml V = 25ml Phenol Red 8.006.6- 8.0 YellowRedEquivalence point occurs when 25ml base addedPhenolphthalein9.50 8.2- 10.0Colourless Pink pH rise sharply (2.7 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (2.7 11.3) suitable Equivalence Point and End Point coincide when 25ml base added. Indicator change colour at equivalent point (25ml) when pH jumps from 2.7 11.3 pKa indicator within (2.7 11.3) 20. Titration curves Strong Acid with Strong BaseTitration between strong acid(flask) with strong base(burette)IndicatorpKapH range ColourColour HCI + NaOH NaCI + H2O ChangeChangeAcidBase11.3NaOH M = 0.1MMethyl orange 3.463.2- 4.4 REDYellow V = 25ml Bromophenol Blue 4.10 3.0- 4.6 YellowBlue7 Bromocresol Green4.903.8- 5.4 YellowBlueMethyl Red 5.004.8- 6.0 RedYellow2.7 HCIBromothymol Blue 7.306.0- 7.6 YellowBlue1M = 0.1MV = 25ml V = 25mlPhenol Red 8.006.6- 8.0 YellowRedEquivalence point occurs when 25ml base added Phenolphthalein9.50 8.2- 10.0Colourless Pink pH rise sharply (2.7 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (2.7 11.3) suitable Equivalence Point and End Point coincide when 25ml base added.Indicator change colour at equivalent point (25ml) when pH jumps from 2.7 11.3 pKa indicator within (2.7 11.3) Methyl Orange can be used as Indicator11.32.71V = 25ml Methyl Orange change colour at 3.2 4.4 at equivalence point, 25ml. Indicator pKapH rangeAcid BaseMethyl orange3.463.2- 4.4 REDYellow 21. Titration curves Strong Acid with Strong BaseTitration between strong acid(flask) with strong base(burette)IndicatorpKa pH range ColourColour HCI + NaOH NaCI + H2OChangeChange AcidBase11.3NaOH M = 0.1MMethyl orange 3.463.2- 4.4 RED Yellow V = 25ml Bromophenol Blue 4.10 3.0- 4.6YellowBlue7 Bromocresol Green4.903.8- 5.4YellowBlueMethyl Red 5.004.8- 6.0RedYellow2.7 HCIBromothymol Blue 7.306.0- 7.6YellowBlue1M = 0.1MV = 25ml V = 25mlPhenol Red 8.006.6- 8.0YellowRedEquivalence point occurs when 25ml base added Phenolphthalein9.508.2- 10.0Colourless Pink pH rise sharply (2.7 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (2.7 11.3) suitable Equivalence Point and End Point coincide when 25ml base added.Indicator change colour at equivalent point (25ml) when pH jumps from 2.7 11.3 pKa indicator within (2.7 11.3) Methyl Orange can be used as Indicator Phenollphthalein can be used as Indicator11.3 11.32.72.71 1V = 25mlV = 25ml Methyl Orange change colour at 3.2 4.4Phenolphthalein change colour at 8.2- 10 at equivalence point, 25ml.at equivalence point, 25ml Indicator pKapH rangeAcid Base Indicator pKa pH range Acid BaseMethyl orange3.463.2- 4.4 REDYellowPhenolphthalein 9.5 8.2 - 10Colourless PINK 22. Titration curves Weak Acid with Strong Base CH3COOH + NaOH CH3COONa + H2OM = 0.1MM = 0.1M Mole ratio 1: 1Titration between strong acid(flask) with strong base(burette) NaOH V = 25mlV = 25mlCH3COOH + NaOH CH3COONa + H2O M = 0.1MV = 25ml Rapid jump in pH (6.11 11.3) Rapid change at equivalence point (25ml base) Equivalence point amt acid = amt baseCH3COOH End point indicator changes colourM = 0.1M Equvalence point must coincide with end point at 25mlV = 25ml pH at equivalence point = 9 Basic salt, CH3COONa - basic 6.112.87 V = 25ml NaOH NaOHM = 0.1M M = 0.1MV = 0 ml V = 24 ml added CH3COOH CH3COOH M = 0.1MM = 0.1M V = 25ml V = 1ml pH = 2.87pH = 6.11 Acidic mediumIndicator pKapH rangeColourAcid Methyl orange3.463.2- 4.4REDBromophenol Blue4.103.0- 4.6 YellowBromocresol Green 4.903.8- 5.4 YellowMethyl Red5.004.8- 6.0 RedBromothymol Blue7.306.0- 7.6 YellowPhenol Red8.006.6- 8.0 Yellow Phenolphthalein9.508.2- 10.0 Colourless 23. Titration curves Weak Acid with Strong Base CH3COOH +NaOH CH3COONa + H2O M = 0.1M M = 0.1M Mole ratio 1: 1Titration between strong acid(flask) with strong base(burette)NaOH V = 25ml V = 25mlCH3COOH + NaOH CH3COONa + H2OM = 0.1M V = 25ml Rapid jump in pH (6.11 11.3) Rapid change at equivalence point (25ml base) 11.3 Equivalence point amt acid = amt base CH3COOH End point indicator changes colour M = 0.1M Equvalence point must coincide with end point at 25ml V = 25ml 9 pH at equivalence point = 9 Basic salt, CH3COONa - basic 6.112.87V = 25mlNaOHNaOH NaOHNaOHM = 0.1MM = 0.1MM = 0.1MM = 0.1M V = 25ml addedV = 26mlV = 0 mlV = 24 ml added CH3COOH CH3COOH CH3COOH M = 0.1M NaOH M = 0.1MM = 0.1MV = 0ml left V = 1ml left V = 25ml V = 1mlpH = 9pH = 11.3 pH = 2.87pH = 6.11 Acidic mediumIndicator pKapH range Colour Acid Methyl orange3.46 3.2- 4.4REDBromophenol Blue4.10 3.0- 4.6 YellowBromocresol Green 4.90 3.8- 5.4 YellowMethyl Red5.00 4.8- 6.0 RedBromothymol Blue7.30 6.0- 7.6 YellowPhenol Red8.00 6.6- 8.0 Yellow Phenolphthalein9.508.2- 10.0Colourless 24. Titration curves Weak Acid with Strong Base CH3COOH+ NaOH CH3COONa + H2O M = 0.1M M = 0.1M Mole ratio 1: 1Titration between strong acid(flask) with strong base(burette) NaOHV = 25ml V = 25mlCH3COOH + NaOH CH3COONa + H2O M = 0.1MV = 25ml Rapid jump in pH (6.11 11.3) Rapid change at equivalence point (25ml base) 11.3 Equivalence point amt acid = amt baseCH3COOH End point indicator changes colourM = 0.1M Equvalence point must coincide with end point at 25mlV = 25ml 9 pH at equivalence point = 9 Basic salt, CH3COONa - basic 6.112.87V = 25mlNaOHNaOH NaOHNaOHM = 0.1MM = 0.1MM = 0.1MM = 0.1M V = 25ml addedV = 26mlV = 0 mlV = 24 ml added CH3COOH CH3COOH CH3COOH M = 0.1M NaOH M = 0.1MM = 0.1MV = 0ml left V = 1ml left V = 25ml V = 1mlpH = 9 pH = 11.3 pH = 2.87pH = 6.11 Basic medium Acidic mediumIndicator pKapH range Colour IndicatorpKapH range Colour AcidBase Methyl orange3.46 3.2- 4.4RED Methyl orange3.463.2- 4.4YellowBromophenol Blue4.10 3.0- 4.6 Yellow Bromophenol Blue 4.103.0- 4.6 BlueBromocresol Green 4.90 3.8- 5.4 Yellow Bromocresol Green4.903.8- 5.4 Blue25ml base added:Methyl Red5.00 4.8- 6.0 Red Equivalence point reach Methyl Red5.004.8- 6.0Yellow Indicator change colourBromothymol Blue7.30 6.0- 7.6 Yellow Bromothymol Blue 7.306.0- 7.6 BluePhenol Red8.00 6.6- 8.0 YellowPhenol Red8.006.6- 8.0 Red Phenolphthalein9.508.2- 10.0Colourless Phenolphthalein 9.508.2- 10.0Pink 25. Titration curve Weak Acid with Strong Base Titration between weak acid (flask) with strong base(burette) IndicatorpKapH range Colour Colour CH3COOH + NaOH CH3COONa + H2OChange Change Acid Base 11.3 NaOH Methyl orange 3.463.2- 4.4REDYellowM = 0.1MV = 25ml Bromophenol Blue 4.103.0- 4.6 Yellow BlueBromocresol Green 4.903.8- 5.4 Yellow Blue 6.11Methyl Red5.004.8- 6.0 Red Yellow2.87CH3COOHBromothymol Blue 7.306.0- 7.6 Yellow BlueM = 0.1M V = 25ml V = 25mlPhenol Red8.006.6- 8.0 Yellow Red Equivalence point occurs when 25ml base added Phenolphthalein9.508.2- 10.0 ColourlessPink pH rise sharply (6.11 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (6.11 11.3) suitable Equivalence Point and End Point coincide when 25ml base added. 26. Titration curve Weak Acid with Strong Base Titration between weak acid (flask) with strong base(burette)IndicatorpKa pH rangeColour Colour CH3COOH + NaOH CH3COONa + H2O Change ChangeAcid Base 11.3 NaOHMethyl orange3.46 3.2- 4.4 RED YellowM = 0.1MV = 25ml Bromophenol Blue 4.10 3.0- 4.6YellowBlueBromocresol Green4.903.8- 5.4YellowBlue 6.11Methyl Red5.00 4.8- 6.0 Red Yellow2.87CH3COOHBromothymol Blue 7.30 6.0- 7.6YellowBlueM = 0.1M V = 25ml V = 25mlPhenol Red 8.006.6- 8.0YellowRed Equivalence point occurs when 25ml base addedPhenolphthalein 9.50 8.2- 10.0 ColourlessPink pH rise sharply (6.11 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (6.11 11.3) suitableIndicator change colour at equivalent point (25ml) when pH jumps from 6.11 11.3 Equivalence Point and End Point coincide when 25ml base added. pKa indicator within (6.11 11.3) 27. Titration curve Weak Acid with Strong Base Titration between weak acid (flask) with strong base(burette) IndicatorpKa pH rangeColour Colour CH3COOH + NaOH CH3COONa + H2OChange Change Acid Base 11.3 NaOH Methyl orange3.46 3.2- 4.4 RED YellowM = 0.1MV = 25mlBromophenol Blue 4.10 3.0- 4.6YellowBlue Bromocresol Green4.903.8- 5.4YellowBlue 6.11 Methyl Red5.00 4.8- 6.0 Red Yellow2.87CH3COOH Bromothymol Blue 7.30 6.0- 7.6YellowBlueM = 0.1M V = 25ml V = 25ml Phenol Red 8.006.6- 8.0YellowRed Equivalence point occurs when 25ml base added Phenolphthalein 9.50 8.2- 10.0 ColourlessPink pH rise sharply (6.11 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (6.11 11.3) suitable Indicator change colour at equivalent point (25ml) when pH jumps from 6.11 11.3 Equivalence Point and End Point coincide when 25ml base added. pKa indicator within (6.11 11.3)Methyl Orange cannot be used as Indicator 11.36.112.87 V = 25ml Methyl Orange change colour at 3.2 4.4 before equivalence point, 25ml. Indicator pKapH rangeAcid Base Methyl orange 3.463.2- 4.4 REDYellow 28. Titration curve Weak Acid with Strong Base Titration between weak acid (flask) with strong base(burette) Indicator pKapH range ColourColour CH3COOH + NaOH CH3COONa + H2O ChangeChangeAcidBase 11.3 NaOH Methyl orange3.463.2- 4.4RED YellowM = 0.1MV = 25mlBromophenol Blue4.103.0- 4.6YellowBlue Bromocresol Green 4.903.8- 5.4 YellowBlue 6.11 Methyl Red5.00 4.8- 6.0RedYellow2.87CH3COOH Bromothymol Blue 7.30 6.0- 7.6YellowBlueM = 0.1M V = 25ml V = 25ml Phenol Red8.00 6.6- 8.0YellowRed Equivalence point occurs when 25ml base added Phenolphthalein 9.50 8.2- 10.0Colourless Pink pH rise sharply (6.11 11.3) Indicator MUST change colour at equivalence point Indicator with pKa falls in pH range (6.11 11.3) suitable Indicator change colour at equivalent point (25ml) when pH jumps from 6.11 11.3 Equivalence Point and End Point coincide when 25ml base added. pKa indicator within (6.11 11.3)Methyl Orange cannot be used as Indicator Phenollphthalein can be used as Indicator 11.311.36.11 6.112.872.87 V = 25mlV = 25ml Methyl Orange change colour at 3.2 4.4Phenolphthalein change colour at 8.2- 10 before equivalence point, 25ml.at equivalence point, 25ml Indicator pKapH rangeAcid BaseIndicatorpKapH range Acid Base Methyl orange 3.463.2- 4.4 REDYellowPhenolphthalein9.5 8.2 - 10Colourless PINK 29. Titration curves Strong Acid with Weak BaseHCI+NH4OH NH4CI + H2OM = 0.1MM = 0.1M NH4OH Mole ratio 1: 1Titration between strong acid(flask) with weak base(burette) M = 0.1MV = 25mlV = 25mlHCI + NH4OH NH4CI + H2OV = 25ml Rapid jump in pH (2.7 7.8) Rapid change at equivalence point (25ml base) Equivalence point amt acid = amt baseHCI End point indicator change colourM = 0.1M Equvalence point must coincide with end point at 25mlV = 25ml pH at equivalence point = 5.3 Acidic salt, NH4CI acidic2.7 1V = 25ml NH4OH NH4OH M = 0.1MM = 0.1M V = 0 mlV = 24 ml added HCIHCI M = 0.1M M = 0.1M V = 25ml V = 1ml left pH = 1 pH = 2.7Acidic medium Indicator pKa pH range Colour Acid Methyl orange 3.46 3.2- 4.4 REDBromophenol Blue 4.10 3.0- 4.6YellowBromocresol Green4.90 3.8- 5.4Yellow Methyl Red5.00 4.8- 6.0RedBromothymol Blue 7.30 6.0- 7.6Yellow Phenol Red8.00 6.6- 8.0Yellow Phenolphthalein 9.50 8.2- 10.0Colourless 30. Titration curves Strong Acid with Weak Base HCI + NH4OH NH4CI + H2O M = 0.1MM = 0.1M NH4OH Mole ratio 1: 1Titration between strong acid(flask) with weak base(burette) M = 0.1M V = 25mlV = 25mlHCI + NH4OH NH4CI + H2OV = 25ml Rapid jump in pH (2.7 7.8) Rapid change at equivalence point (25ml base) Equivalence point amt acid = amt baseHCI End point indicator change colour7.8 M = 0.1M Equvalence point must coincide with end point at 25mlV = 25ml pH at equivalence point = 5.3 5.3 Acidic salt, NH4CI acidic2.7 1 V = 25mlNH4OH NH4OH NH4OH NH4OHM = 0.1MM = 0.1M M = 0.1MM = 0.1M V = 25ml addedV = 26ml V = 0 mlV = 24 ml addedHCI HCIHCI M = 0.1M NaOH M = 0.1M M = 0.1MV = 0ml left V = 1ml left V = 25ml V = 1ml leftpH = 5.3 pH = 7.8 pH = 1 pH = 2.7Acidic medium Indicator pKa pH range Colour Acid Methyl orange 3.46 3.2- 4.4 REDBromophenol Blue 4.10 3.0- 4.6YellowBromocresol Green4.90 3.8- 5.4Yellow Methyl Red5.00 4.8- 6.0RedBromothymol Blue 7.30 6.0- 7.6Yellow Phenol Red8.00 6.6- 8.0Yellow Phenolphthalein 9.50 8.2- 10.0Colourless 31. Titration curves Strong Acid with Weak BaseHCI + NH4OH NH4CI+ H2OM = 0.1MM = 0.1MNH4OH Mole ratio 1: 1Titration between strong acid(flask) with weak base(burette)M = 0.1MV = 25mlV = 25mlHCI + NH4OH NH4CI + H2O V = 25ml Rapid jump in pH (2.7 7.8) Rapid change at equivalence point (25ml base) Equivalence point amt acid = amt baseHCI End point indicator change colour7.8 M = 0.1M Equvalence point must coincide with end point at 25mlV = 25ml pH at equivalence point = 5.3 5.3 Acidic salt, NH4CI acidic2.7 1 V = 25ml NH4OH NH4OH NH4OH NH4OH M = 0.1MM = 0.1M M = 0.1MM = 0.1MV = 25ml addedV = 26ml V = 0 mlV = 24 ml added HCI HCIHCIM = 0.1M NaOH M = 0.1M M = 0.1M V = 0ml left V = 1ml left V = 25ml V = 1ml left pH = 5.3pH = 7.8 pH = 1 pH = 2.7Basic mediumAcidic medium Indicator pKa pH range ColourIndicatorpKapH range Colour Acid Base Methyl orange 3.46 3.2- 4.4 REDMethyl orange3.463.2- 4.4 YellowBromophenol Blue 4.10 3.0- 4.6YellowBromophenol Blue 4.103.0- 4.6BlueBromocresol Green4.90 3.8- 5.4YellowBromocresol Green4.903.8- 5.4Blue25ml base added: Methyl Red5.00 4.8- 6.0Red Equivalence point reachMethyl Red5.004.8- 6.0 Yellow Indicator change colourBromothymol Blue 7.30 6.0- 7.6YellowBromothymol Blue 7.306.0- 7.6Blue Phenol Red8.00 6.6- 8.0Yellow Phenol Red8.006.6- 8.0Red Phenolphthalein 9.50 8.2- 10.0ColourlessPhenolphthalein 9.508.2- 10.0 Pink 32. Titration curves Strong Acid with Weak BaseTitration between strong acid(flask) with weak base(burette) Indicator pKapH range Colour ColourHCI + NH4OH NH4CI + H2OChange ChangeAcid BaseNH4OHM = 0.1M Methyl orange 3.463.2- 4.4REDYellowV = 25ml7.8 Bromophenol Blue4.103.0- 4.6 Yellow Blue5.3 Bromocresol Green 4.903.8- 5.4 Yellow Blue 2.71HCIMethyl Red 5.004.8- 6.0 Red YellowV = 25mlM = 0.1MV = 25ml Bromothymol Blue7.306.0- 7.6 Yellow BlueEquivalence point occurs when 25ml base added Phenol Red 8.006.6- 8.0 Yellow Red pH rise sharply (2.7 7.8) Indicator MUST change colour at equivalence point Phenolphthalein9.508.2- 10.0 ColourlessPink Indicator with pKa falls in pH range (2.7 7.8) suitable Equivalence Point and End Point coincide when 25ml base added 33. Titration curves Strong Acid with Weak BaseTitration between strong acid(flask) with weak base(burette) IndicatorpKapH range ColourColourHCI + NH4OH NH4CI + H2O ChangeChange AcidBaseNH4OHM = 0.1MMethyl orange3.46 3.2- 4.4 REDYellowV = 25ml7.8Bromophenol Blue 4.10 3.0- 4.6Yellow Blue5.3 Bromocresol Green4.903.8- 5.4Yellow Blue 2.71HCI Methyl Red 5.004.8- 6.0 RedYellowV = 25mlM = 0.1MV = 25ml Bromothymol Blue7.30 6.0- 7.6Yellow BlueEquivalence point occurs when 25ml base addedPhenol Red 8.006.6- 8.0Yellow Red pH rise sharply (2.7 7.8) Indicator MUST change colour at equivalence pointPhenolphthalein9.508.2- 10.0 Colourless Pink Indicator with pKa falls in pH range (2.7 7.8) suitable Equivalence Point and End Point coincide when 25ml base added Indicator change colour at equivalent point (25ml ) when pH jumps from (2.7 7.8) pKa of indicator within (2.7 7.8) 34. Titration curves Strong Acid with Weak BaseTitration between strong acid(flask) with weak base(burette)IndicatorpKapH range ColourColourHCI + NH4OH NH4CI + H2OChangeChangeAcidBaseNH4OHM = 0.1M Methyl orange3.46 3.2- 4.4 REDYellowV = 25ml 7.8 Bromophenol Blue 4.10 3.0- 4.6Yellow Blue 5.3Bromocresol Green4.903.8- 5.4Yellow Blue2.71HCIMethyl Red 5.004.8- 6.0 RedYellow V = 25ml M = 0.1MV = 25mlBromothymol Blue7.30 6.0- 7.6Yellow BlueEquivalence point occurs when 25ml base added Phenol Red 8.006.6- 8.0Yellow Red pH rise sharply (2.7 7.8) Indicator MUST change colour at equivalence point Phenolphthalein9.508.2- 10.0 Colourless Pink Indicator with pKa falls in pH range (2.7 7.8) suitable Equivalence Point and End Point coincide when 25ml base addedIndicator change colour at equivalent point (25ml ) when pH jumps from (2.7 7.8) pKa of indicator within (2.7 7.8) Phenolphthalein cannot be used as Indicator 7.8 2.71 V = 25mlPhenolphthalein change colour at 8.2- 10after equivalence point, 25ml . IndicatorpKapH rangeAcid Base Phenolphthalein9.5 8.2 - 10ColourlessPINK 35. Titration curves Strong Acid with Weak BaseTitration between strong acid(flask) with weak base(burette)IndicatorpKapH rangeColourColourHCI + NH4OH NH4CI + H2O ChangeChange AcidBaseNH4OHM = 0.1M Methyl orange3.463.2- 4.4RED YellowV = 25ml 7.8 Bromophenol Blue 4.103.0- 4.6 YellowBlue 5.3Bromocresol Green 4.903.8- 5.4 YellowBlue2.71HCIMethyl Red5.004.8- 6.0 RedYellow V = 25ml M = 0.1MV = 25mlBromothymol Blue7.306.0- 7.6 YellowBlueEquivalence point occurs when 25ml base added Phenol Red8.006.6- 8.0 YellowRed pH rise sharply (2.7 7.8) Indicator MUST change colour at equivalence point Phenolphthalein 9.50 8.2- 10.0Colourless Pink Indicator with pKa falls in pH range (2.7 7.8) suitable Equivalence Point and End Point coincide when 25ml base addedIndicator change colour at equivalent point (25ml ) when pH jumps from (2.7 7.8) pKa of indicator within (2.7 7.8) Phenolphthalein cannot be used as IndicatorMethyl Orange can be used as Indicator 7.87.8 2.72.71 V = 25ml V = 25mlPhenolphthalein change colour at 8.2- 10Methyl Orange change colour at 3.2 4.4after equivalence point, 25ml . at equivalence point, 25ml. IndicatorpKapH rangeAcid BaseIndicator pKapH range Acid Base Phenolphthalein9.5 8.2 - 10ColourlessPINK Methyl orange3.46 3.2- 4.4 REDYellow 36. Titration curves Weak Acid with Weak Base CH3COOH + NH4OH CH3COONH4 + H2OM = 0.1MM = 0.1M NH4OHMole ratio 1: 1Titration between weak base(burette) with weak acid(flask) M = 0.1MV = 25mlV = 25ml CH3COOH + NH4OH CH3COONH4 + H2O V = 25ml No sharp rise in pH at equivalence point (25ml base) Equivalence point amt acid = amt base End point indicator changes colourCH3COOH Equvalence point must coincide with end point at 25ml M = 0.1M pH at equivalence point = 7 V = 25ml Neutral salt, CH3COONH4 neutral 6.112.87V = 25mlNH4OH NH4OHM = 0.1MM = 0.1MV = 0 mlV = 24 ml added CH3COOH CH3COOH M = 0.1MM = 0.1MV = 25ml V = 1ml left pH = 2.87 pH = 6.11 Acidic mediumIndicator pKa pH range ColourAcid Methyl orange3.46 3.2- 4.4 RED Bromophenol Blue 4.10 3.0- 4.6Yellow Bromocresol Green4.90 3.8- 5.4YellowMethyl Red5.00 4.8- 6.0Red Bromothymol Blue 7.30 6.0- 7.6YellowPhenol Red8.00 6.6- 8.0YellowPhenolphthalein 9.50 8.2- 10.0Colourless 37. Titration curves Weak Acid with Weak BaseCH3COOH+ NH4OH CH3COONH4 + H2O M = 0.1M M = 0.1M NH4OHMole ratio 1: 1Titration between weak base(burette) with weak acid(flask) M = 0.1M V = 25ml V = 25ml CH3COOH + NH4OH CH3COONH4 + H2O V = 25ml No sharp rise in pH at equivalence point (25ml base) Equivalence point amt acid = amt base 7.8 End point indicator changes colourCH3COOH Equvalence point must coincide with end point at 25ml M = 0.1M pH at equivalence point = 7 V = 25ml 7 Neutral salt, CH3COONH4 neutral 6.112.87V = 25mlNH4OH NH4OHNH4OH NH4OH M = 0.1MM = 0.1MM = 0.1MM = 0.1MV = 25ml addedV = 26mlV = 0 mlV = 24 ml addedCH3COOH CH3COOH CH3COOH M = 0.1M NH4OH M = 0.1MM = 0.1M V = 0ml left V = 1ml leftV = 25ml V = 1ml left pH = 7pH = 7.8 pH = 2.87 pH = 6.11 Acidic mediumIndicator pKa pH range ColourAcid Methyl orange3.46 3.2- 4.4 RED Bromophenol Blue 4.10 3.0- 4.6Yellow Bromocresol Green4.90 3.8- 5.4YellowMethyl Red5.00 4.8- 6.0Red Bromothymol Blue 7.30 6.0- 7.6YellowPhenol Red8.00 6.6- 8.0YellowPhenolphthalein 9.50 8.2- 10.0Colourless 38. Titration curves Weak Acid with Weak BaseCH3COOH+ NH4OH CH3COONH4 + H2O M = 0.1M M = 0.1M NH4OHMole ratio 1: 1Titration between weak base(burette) with weak acid(flask) M = 0.1M V = 25ml V = 25ml CH3COOH + NH4OH CH3COONH4 + H2O V = 25ml No sharp rise in pH at equivalence point (25ml base) Equivalence point amt acid = amt base 7.8 End point indicator changes colour CH3COOH Equvalence point must coincide with end point at 25mlM = 0.1M pH at equivalence point = 7V = 25ml 7 Neutral salt, CH3COONH4 neutral 6.112.87V = 25mlNH4OHNH4OHNH4OH NH4OH M = 0.1M M = 0.1MM = 0.1MM = 0.1MV = 25ml added V = 26mlV = 0 mlV = 24 ml addedCH3COOH CH3COOH CH3COOH M = 0.1MNH4OH M = 0.1MM = 0.1M V = 0ml leftV = 1ml leftV = 25ml V = 1ml left pH = 7 pH = 7.8 pH = 2.87 pH = 6.11 Basic medium Acidic mediumIndicator pKa pH range ColourIndicatorpKapH range ColourAcid Base Methyl orange3.46 3.2- 4.4 REDMethyl orange3.463.2- 4.4Yellow Bromophenol Blue 4.10 3.0- 4.6YellowBromophenol Blue 4.103.0- 4.6 Blue Bromocresol Green4.90 3.8- 5.4YellowBromocresol Green4.903.8- 5.4 Blue 25ml base added:Methyl Red5.00 4.8- 6.0Red Equivalence point reachMethyl Red5.004.8- 6.0Yellow Indicator change colour Bromothymol Blue 7.30 6.0- 7.6YellowBromothymol Blue 7.306.0- 7.6 BluePhenol Red8.00 6.6- 8.0Yellow Phenol Red8.006.6- 8.0 RedPhenolphthalein 9.50 8.2- 10.0ColourlessPhenolphthalein 9.508.2- 10.0Pink 39. Titration curves Weak Acid with Weak BaseTitration between weak base(burette) with weak acid(flask)IndicatorpKapH range Colour Colour CH3COOH + NH4OH CH3COONH4 + H2O Change ChangeAcid Base NH4OH Methyl orange 3.463.2- 4.4REDYellow7.8M = 0.1M V = 25mlBromophenol Blue 4.103.0- 4.6 Yellow Blue7 6.11Bromocresol Green 4.903.8- 5.4 Yellow Blue2.87 Methyl Red5.004.8- 6.0 Red Yellow CH3COOH Bromothymol Blue7.306.0- 7.6 Yellow Blue V = 25mlM = 0.1MV = 25ml Phenol Red8.006.6- 8.0 Yellow Red Equivalence point occurs when 25ml base added No sharp rise in pHPhenolphthalein9.508.2- 10.0 ColourlessPink Indicator MUST change colour at equivalence point No Indicator suitable 40. Titration curves Weak Acid with Weak BaseTitration between weak base(burette) with weak acid(flask) Indicator pKa pH rangeColour Colour CH3COOH + NH4OH CH3COONH4 + H2O Change ChangeAcid Base NH4OHMethyl orange 3.463.2- 4.4 REDYellow7.8M = 0.1M V = 25mlBromophenol Blue4.103.0- 4.6Yellow Blue7 6.11Bromocresol Green4.903.8- 5.4Yellow Blue2.87Methyl Red5.004.8- 6.0Red Yellow CH3COOHBromothymol Blue7.306.0- 7.6Yellow Blue V = 25mlM = 0.1MV = 25mlPhenol Red8.006.6- 8.0Yellow Red Equivalence point occurs when 25ml base added No sharp rise in pH Phenolphthalein9.50 8.2- 10.0 ColourlessPink Indicator MUST change colour at equivalence point No Indicator suitable No indicators are suitable as no sharp rise in pH 41. Titration curves Weak Acid with Weak BaseTitration between weak base(burette) with weak acid(flask) Indicator pKa pH rangeColour Colour CH3COOH + NH4OH CH3COONH4 + H2O Change ChangeAcid BaseNH4OH Methyl orange 3.463.2- 4.4 REDYellow7.8 M = 0.1MV = 25mlBromophenol Blue4.103.0- 4.6Yellow Blue7 6.11Bromocresol Green4.903.8- 5.4Yellow Blue2.87Methyl Red5.004.8- 6.0Red Yellow CH3COOHBromothymol Blue7.306.0- 7.6Yellow Blue V = 25mlM = 0.1MV = 25mlPhenol Red8.006.6- 8.0Yellow Red Equivalence point occurs when 25ml base added No sharp rise in pH Phenolphthalein9.50 8.2- 10.0 ColourlessPink Indicator MUST change colour at equivalence point No Indicator suitable No indicators are suitable as no sharp rise in pHPhenolphthalein cannot be used as Indicator7.87 6.11 2.87 V = 25mlPhenolphthalein change colour at 8.2- 10after equivalence point, 25ml .Indicator pKa pH range Acid Base Phenolphthalein9.58.2 - 10 ColourlessPINK 42. Titration curves Weak Acid with Weak BaseTitration between weak base(burette) with weak acid(flask) Indicator pKapH rangeColourColour CH3COOH + NH4OH CH3COONH4 + H2OChangeChange AcidBaseNH4OH Methyl orange 3.463.2- 4.4RED Yellow7.8 M = 0.1MV = 25mlBromophenol Blue4.103.0- 4.6 YellowBlue7 6.11Bromocresol Green4.903.8- 5.4 YellowBlue2.87Methyl Red5.004.8- 6.0 RedYellow CH3COOHBromothymol Blue7.306.0- 7.6 YellowBlue V = 25mlM = 0.1MV = 25mlPhenol Red8.006.6- 8.0 YellowRed Equivalence point occurs when 25ml base added No sharp rise in pH Phenolphthalein9.508.2- 10.0 Colourless Pink Indicator MUST change colour at equivalence point No Indicator suitable No indicators are suitable as no sharp rise in pHPhenolphthalein cannot be used as Indicator Methyl Orange cannot be used as Indicator7.87.877 6.116.11 2.872.87 V = 25ml V = 25mlPhenolphthalein change colour at 8.2- 10 Methyl Orange change colour at 3.2 4.4after equivalence point, 25ml .before equivalence point, 25ml.Indicator pKa pH range Acid Base Indicator pKapH rangeAcid Base Phenolphthalein9.58.2 - 10 ColourlessPINKMethyl orange3.463.2- 4.4 REDYellow 43. Salt HydrolysisAcid + Base Salt + Water (Neutralization)Salt produced can be Neutral, pH 7, No hydrolysis Acidic, pH < 7, Cation hydrolysis Basic, pH > 7, Anionic hydrolysisWater hydrolysis chemical reaction involving water in producing H+ and OH- ionsNeutral SaltAcidic Salt Basic SaltStrongStrong Weak Strong StrongWeak Base Acid Base AcidBaseAcid(NaOH)(HCI) (NH4OH) (HCI)(NaOH)(CH3COOH) NaOH + HCI NaCI + H2O NH4OH + HCI NH4CI + H2O NaOH + CH3COOH CH3COONa + H2O Na+=CI-NH4+CI- Na+CH3COO-Strong baseStrong acid Weak base Strong acidStrong base Weak acid NaOH= HCINH4OH < HCINaOH> CH3COOH Neutral Salt Acidic SaltBasic SaltNaCI dissolves in water Water hydrolysis CH3COO- - conjugate base NH4+ - conjugate acidNaCI No water hydrolysis NH4+ - Cation hydrolysisCH3COO- - Anion hydrolysispH = 7 NH4+ + H2O H3O+ + NH3 CH3COO- + H2O CH3COOH + OH- Acid (proton donor) Base (proton acceptor) pH < 7 pH > 7Salt ProducedExamples Nature of salt Strong acid + Strong base NaCI, Na2SO4, KNO3 Neutral (No hydrolysis) Strong Acid + Weak baseNH4CI, (NH4)2SO4, NH4NO3 Acidic (Cation Hydrolysis) Weak Acid + Strong Base CH3COONa, Na2CO3 , Na3PO4Basic (Anion Hydrolysis) Weak Acid + Weak Base CH3COONH4, (NH4)3PO4pH depends on Ka and Kb Ka > Kb = acidic Kb > Ka = basic 44. Acidic SaltNeutralization bet Strong Acid + Weak Base Salts of Transition Metal ionsTransition metal ions: SIZE and CHARGE of cation Acidic Salt High charge density Ni2+, Cu2+,Fe3+, Al3+ Small size ion Ni2+, Cu2+,Fe3+, Al3+ Weak Strong Base Acid(NH4OH) (HCI) NH4OH + HCI NH4CI + H2O [Fe(H2O)6]3+CI3[AI(H2O)6]3+CI3 NH4+CI- Fe AI Weak base Strong acidNH4OH < HCI Acidic Salt NH4+ - Conjugate acid NH4+ - Cation hydrolysis NH4+ + H2O H3O+ + NH3 Acid (proton donor) 6 H2O attract to Fe3+ ion 6 H2O attract to AI3+ ion pH < 7 Lone pair on Oxygen act as a ligand Lone pair on Oxygen act as a ligand Ligand attract to Fe3+ Ligand attract to AI3+ Form dative bond Form dative bond Salt ExamplesNature of saltProducedStrong Acid + NH4CI, Acidic Weak base(NH4)2SO4, NH4NO3Polarise water/water hydrolysis to produce H+ ions Acidic saltNH4OH + HCI NH4CI + H2ONH4OH + H2SO4 NH4SO4+ H2ONH4OH + HNO3 NH4NO3 + H2O[Fe(H2O)6]3+ (H2O)5Fe3+ :OH+ [(H2O)5FeOH]2+ + H+ | Hydrogen ionWater hydrolysisproducedHhttp://fineartamerica.com/featured/transition-metal-ion-colours-martyn-f-chillmaid.html 45. Simulation and Animation on Buffer and TitrationsClick here titration animationClick here titration animationClick here for videos from Khan Academy Click here titration simulation Click here salt hydrolysis animationClick here acidic buffer animationClick here on acid base indicator Click here on universal indicator Click here on universal indicator 46. 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