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Chemistry 12 Acid-Base Equilibrium VII Name: Date: Block: 1. Titrations 2. Indicators Titrations Titration is a form of volumetric analysis where the number of moles of solute in a solution is determined by adding a sufficient volume of another solution of known concentration to just produce a complete reaction. • The reaction is completed when the number of moles of H3O + equals the total number of moles of OH- - this is called the equivalence point or stoichiometric point of the titration. • An indicator is used that will indicate when the equivalence point has been reached by changing colour at or very near the pH associated with the equivalence point. We will be dealing with 3 scenarios: 1. 2. 3. (Chemistry 11) Example 1: A student standardizing a solution of NaOH finds that 28.15 mL of that solution is required to neutralize 25.00 mL of a 0.1072 M standard solution of HCl. Calculate the [NaOH]. • Write the balanced equation. • What is the concentration of NaOH?

Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

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Page 1: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

Chemistry12Acid-BaseEquilibriumVII

Name:Date:Block:

1. Titrations2. Indicators

TitrationsTitrationisaformofvolumetricanalysiswherethenumberofmolesofsoluteinasolutionisdeterminedbyaddingasufficientvolumeofanothersolutionofknownconcentrationtojustproduceacompletereaction.

• ThereactioniscompletedwhenthenumberofmolesofH3O+equalsthetotalnumberofmolesofOH--thisiscalledtheequivalencepointorstoichiometricpointofthetitration.

• AnindicatorisusedthatwillindicatewhentheequivalencepointhasbeenreachedbychangingcolouratorverynearthepHassociatedwiththeequivalencepoint.

Wewillbedealingwith3scenarios:1.2.3.

(Chemistry11)Example1:AstudentstandardizingasolutionofNaOHfindsthat28.15mLofthatsolutionisrequiredtoneutralize25.00mLofa0.1072MstandardsolutionofHCl.Calculatethe[NaOH].

• Writethebalancedequation.

• WhatistheconcentrationofNaOH?

Page 2: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

Example2:A20.0mLsampleof0.450MHNO2istitratedwitha0.500MNaOHsolution.Whatvolumeofbaseisaddedatexactlyhalfwaytotheequivalencepoint?

• Drawasketchoftheset-up:

• Whatisthebalancedreaction?

• WhatvolumeofNaOHwasneededatequivalencepoint?

• Whatishalfwaytoequivalencepoint?

TITRATIONCURVES:• AgraphthatplotsthepHofthesolutionvs.thevolumeofthetitrantadded.

Asthetitrantisadded,thepHisgradually(increasing/decreasing)whichmeansthat(acid/base)isthetitrant.HowmanymLoftitrantwasrequiredtoattainequivalencepoint?___________LookingattheequivalencepointpH,doyouthinkthereactionproducedanacidicorbasicsalt?

Whatdoyouthinkthegraphwouldlooklikeifanacidwasthetitrant?Explainyouranswer.

Page 3: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

1.StrongAcid&StrongBase

HCl(aq)+NaOH(aq)àNaCl(aq)+H2O(l)

• Typicalstrongacid+strongbaseneutralizationtypeofquestion.(1)Dilution(2)Neutralization(3)Acidicorbasic?

2.WeakAcid&StrongBase

CH3COOH(aq)+NaOH(aq)àNaCH3COO(aq)+H2O(l)

50.0mLof0.100Maceticacidistitratedwith0.150MNaOH.WhatdoyouthinkthepHcurvewilllooklike?

BecausethepHmeterismeasuringfromthebeaker,wealwayshavetothinkabout__________________!

Wewillbecalculating(andcomparing)thepHat4pointsonthecurve:1. 2. 3. 4.

CalculatethepHofthesolutionproducedinthereactionflaskatthefollowingpoints:1) ThepHofthesolutionofaceticacidwhennoNaOHisyetadded.

• Thisisaweakacidcalculation.

Page 4: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

2) When10.0mLof0.150MNaOHhasbeenadded.

• Actsverysimilarlytoabufferastheaddedhydroxideionsreactswithaceticacidtoproduceacetateions.

• Whatarethedilutedconcentrationsofreactantacidandbasebeforethereaction(initialconcentrations)?

• CreateanICEtable.

• CH3COOHandCH3COO-createsanacidbuffer.

• CalculatethepH.

Page 5: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

3) Attheequivalencepointwhen______mLofNaOHhasbeenadded.

• WhatvolumeofNaOHisneededatequivalencepoint?

• Whatarethedilutedconcentrationsofreactantacidandbasebeforethereaction(initialconcentrations)?

• CreateanICEtable.

• Theanionofthedissociatedsalt,NaCH3COO,istheconjugatebaseofaweakacidandisthuscapableofacceptingprotonsfromwaterinahydrolysisreaction.

• Whatisthehydrolysisreaction?

• CreateanICEtable.

• CalculatepHofthesolutionresultingfromtheanionichydrolysisoftheacetateion.

Page 6: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

4) Beyondtheequivalencepointwhen60.0mLofNaOHadded

Page 7: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

Practice:A20.0mLsampleof0.450MHNO2istitratedwitha0.500MNaOHsolution.WhatwillthepHbeinthereactionflaskatthefollowingpoints:

a) 2.0mLbeforeexactlyhalfwaytotheequivalencepoint?

Page 8: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

b) Atequivalencepoint?

Page 9: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

3.StrongAcid&WeakBase

NH3(aq)+HCl(aq)àNH4+(aq)+Cl-(aq)100.0mLof0.050MNH3istitratedwith0.10MHCl.CalculatethepHofthesolutionproducedinthereactionflaskatthefollowingpoints:

1) BeforeanyHClisadded.2) Atthemidpointofthetitration.

Page 10: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

3) Attheequivalencepointwhen_______mLofHClhasbeenadded.

Page 11: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

4) When60.0mLofHClhasbeenadded.

Page 12: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

Practice:CalculatethepHofthesolutionproducedinthereactionflaskwhen13.00mLof0.100MHClO4hasbeenaddedto25.00mLof0.100MNaNO2.(Thisisjustbeyondhalfwaytotheequivalencepoint.)

Page 13: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

IndicatorsWemeasurepHusingeitheranacid-baseindicatororapHmeter.Acid-baseindicatorsareweakorganicacidswhoseconjugatepairsdisplaydifferentandnormallyintensecolours.Acid-baseindicatorsarecomplexorganicmoleculesandrefertothemassimply“HIn.”

HIn+H2O⇋In-+H3O+

Ka=Example:Considermethylredindicator.

pH:Colour:

• ThepHvalueatwhichtheindicatorexhibitsacolourchangeshouldbeclosetothepHatequivalencepoint.(____________à____________ß____________).

• Whenthecolourchanges,(reached_______________________point)itisanindicationthatthetitrationhasreachedequivalencepoint.

pHatequivalence

point[H3O+] Indicator Colourexhibited

Alizarinyellow

6.8

Lightpink

Thymolblue Green

2.0

Page 14: Chemistry 12 Acid-Base Equilibrium VII• A graph that plots the pH of the solution vs. the volume of the titrant added. ... • Calculate pH of the solution resulting from the anionic

When1.0MNH3istitratedwith1.0MHCl,themostsuitableindicatoris:

A.methylviolet. C.phenolphthalein. B.indigocarmine. D.bromcresolgreen.

Themostappropriateindicatorforthetitrationof0.50MCH3COOHwith0.50MNaOHis

A.methylviolet. C.phenolphthalein. B.indigocarmine. D.bromcresolgreen.

HebdenWorkbookPg.162#108-116


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