name: regents chemistry: dr. shanzer practice...

Name:

Regents Chemistry: Dr. Shanzer

PracticePacket

Chapter13:Acids&Bases

1

Characteristics of

Acids & BasesChemistry 200

Video Lesson 13.1

Objective:How can we recognize characteristics of acids and bases?

How can we determine the difference between Arrhenius and Bronsted/Lowry acids and bases?

Acids&BasesAcids&Basescanberecognizedbytheirproperties.

• Dilutesolutionshaveasourtastelemons-->citricacid

vinegar-->aceticacidcarbonateddrinks-->carbonicacidtomato-->ascorbicacid

• Haveabittertaste&slippery,soapyfeel.soap,milkofmagnesia

ex:

ex:

Acids

Bases

AcidsTwotheoriesusedtoexplainthebehaviorofacids:

• asubstancethatreleaseshydrogenions[H+]inanaqueoussolutionex:HCl,H2SO4

• notallsubstancesthatcontainhydrogenareacids.CH4(methane)isnotanacidbecausethehydrogenatomsdonotionize.

ArrheniusAcid(SvanteArrhenius)

• A Hydrogen Ion is produced when a hydrogen atom

loses an electron to become a positive ion • AHydroniumIon[H3O]+isformedwhenahydrogenionreactsw/H2O

TableE

2

ex:HCl(g)-------->H3O+(aq)+Cl-(aq)H2O

Arrheniusacidscanbedividedinto2maincategoriesInorganicAcid• anacidthatstartsw/hydrogen&doesnothavecarbon

ex:HCl,H2SO4

OrganicAcid• anacidthathascarbon&endsw/COOH

(CarboxylGroup)

ex:CH3COOH(ethanoicacid)HCOOH(methanoicacid)

AnArrheniusacidcansometimesyieldmorethanone

hydrogenioninaqueoussolution

MonoproticAcid

• acidsthatproduceasinglehydrogenion(ionizesin1step) ex:HCl+H2O-->H3O++Cl-

DiproticAcid

• acidsthatproduce2hydrogenions(ionizesin2steps)

ex:H2SO4-->H++HSO4-(step1)HSO4--->H++SO4-2(step2)Triproticacids:3hydrogenionsex:H3PO4

TheBrønsted-Lowrytheoryfocusessolelyonthehydrogenionasaproton&canbeusedtofurtherexplainacidbehavior:

Brønsted-LowryAcid• anyspecies(anyparticle:atom,moleculeorion)thatcandonateaproton[H+]toanotherspecies(aprotondonor)

• allArrheniusacidsarealsoBrønsted-Lowryacids

ex:HCl(g)+H2O(l)-->H3O+(aq)+Cl-(aq)

• accordingtoBrønsted-Lowry,HClisanacidbecauseitdonatesaproton(H+)

Bases

Theoriesusedtoexplainacidbehaviorcanalsobeusedtoexplainbasesaswell

ArrheniusBase

• asubstancethatreleaseshydroxideions[OH-]inanaqueoussolution

ex:NaOH------>Na+(aq)+OH-(aq)H2O

AnAlcoholshouldnotbeconfusedw/anArrheniusBaseasitdoesnotformahydroxideion[OH-]inan(aq)solution,thereforeitisNOTabase!!!

CH3OHC2H5OH

Brønsted-LowryBase• anyspeciesthatcanacceptaproton[H+]fromanotherspecies-->aprotonacceptor

• accordingtoArrhenius,onlymetallichydroxidesarebases

• Brønsted-LowrydeUinitionsexplainwhyasubstancethathasno[OH-],likeNH3,behaveslikeabaseinH2O

ex:NH3+H2O-->NH4++OH-

3

Amphiprotic(Amphoteric)

• asubstancethatcanactasanacidorabase

ex:H2O

NH3+H2O-->NH4++OH-

HCl+H2O-->H3O++Cl-Base

Acid

Electrolytes

Chemistry 200 Video Lesson 13.2

Objective:How do we determine which acids and bases are strong or weak electrolytes?

Electrolytes

Ex: Acids Bases Salts

• are substances that have mobile ions when put intosolution (aq). This allows it to conduct electricity.

AWeakAcidisaweakelectrolytebecauseitpartiallyionizesinwatertoproduceasmallnumberofH+ionsinsolution.

AStrongAcidisastrongelectrolytebecauseitcompletelyionizesinwatertoproducealargenumberofH+ionsinsolution.

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AStrongBaseisastrongelectrolytebecauseitcompletelyionizesinwatertoproducealargenumberofOH-ionsinsolution

AWeakBaseisaweakelectrolytebecauseitpartiallyionizesinwatertoproduceasmallnumberofOH-ionsinsolution.

ex:

HCl(aq) + NaOH(aq) --> NaCl(aq) + HOH(l)

Acid/Base Reactions

• Acid react with a base to produce a salt and water

Acid/Metal Reactions

• Acids react with a metal to producea salt and hydrogen gas (H2(g))

2HNO3(aq) + Ca(s) --> Ca(NO3)2(aq) + H2(g)

ex:

2HCl(aq) + Cu(s) --> CuCl2(aq) + H2(g)

NO REACTION!!

Conjugate Acid-Base pairs

Video Lesson 13.3

Objectives• Compare and contrast acids and bases as

defined by the theories of Arrhenius andBronsted-Lowry (alternate acid/basetheory).

• QUESTION: Why is ammonia (NH3) a base?

5

• Explains the behavior of WEAK acids and BASES (Na2CO3& NH3)

• Bronsted-Lowry Acids are PROTON DONORS o The prefer to give away a proton (H+)

Alternate Acid-Base Theory AKA Bronsted-Lowry Theory

• Bronsted-Lowry Bases are PROTON ACCEPTORS

Alternate Acid Base Theory

• An acid is a H+ donor while a base is a H+ acceptor. • The substance produced when an acid

has donated its proton is called theconjugate base.

• The substance produced when thebase accepts a H+ is called theconjugate acid

Conjugate Acid/Base Pairs Label the acids and bases according to Bronsted-Lowry:

Acid

Conjugate Base

Base Conjugate Acid

Conjugate Acid-Base Pairs

Practice

Label conjugate acid base pairs in the following equation

Acid

Base

c. base

c. acid

Practice

pH & Acid-Base Indicators

Video Lesson 13.4

6

Objectives• Describe how [H+] and [OH-] are related in

an aqueous solution.• Classify a solution as neutral, acidic or basic.• Describe the purpose of an acid-base

indicator.

The pH Scale• pH = direct measurement of H+ ion concentration in

a solution • “power of hydrogen”

H+H+H+H+ H+

OH-OH-OH-OH-

O 7 14

Acidic Neutral Basic

• The pH scale is logarithmic o Based on exponents of the number 10

• The pH of a solution is the negative log of the [H+] or [OH-] ions

Logarithmic• Each change in a single pH unit signifies a tenfold

change in [H+] concentration

A Tenfold Change

• Indicator o A substance that changes color as a result of a

pH change • Table M• Example: Phenolphthalein à colorless up until a pH

of 8, light pink from 8 to 9 and pink from pH of 9 up

Acid-Base Indicators

7

pH = 5 pH = 11

Acid-Base Titration

Video Lesson 13.5

Objectives• Define products of an acid-base reaction.• Explain how acid-base titration is used to

calculate the concentration of an acid orbase.

• Explain the concept of equivalence inneutralization reactions.

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Neutralization Reactions• Neutral

o Neither acidic nor basic o Equal concentrations of H+ and OH-

o Occurs when Arrhenius acid and an Arrhenius base react to form water and salt

Acid + Base à Salt + Water

HCl + KOH à KCl + HOH

Double Replacement!

+1 -1 -1+1 +1 -1

SaltOr

Ionic Substance

Water

Acid Base

+1 -1

Neutralization Reactions

• Stomach acido pH between 2-3

• Heart burn o Happens when pH

level drops in the stomach

• Milk of Magnesia bringsthe pH up

• Mg(OH)2

Magnesium hydroxide

Acid-Base Titration• Titrations are used to calculate the concentration

(Molarity) of an unknown solution. • Lab process in which an unknown solution is

systematically reacted with a solution of known concentration by adding measured volumes of an acid or a base to the unknown until neutralization occurs.

• In all neutralizationreactions there mustbe a 1:1 ratio of molesof H+ ions and moles ofOH- ions.

• Equivalence Pointo [H+] = [OH-]

9

Example #1• What is the concentration of a solution of HI if 0.3 L is

neutralized by 0.6 L of 0.2 M solution of KOH?

Example #2• You have 50 mL of 1.0 M H2SO4 (aq). What volume of

0.5 M NaOH would be required to neutralize the acid? (Diprotic Acids yield 2 H+ ions in solution!)

10

PracticePacket:AcidsandBases

http://drshanzerchemistry.weebly.com

Video13.1:CharacteristicsofAcidsandBasesAcid/Base/SaltCharacteristics:Onthelinetotheleft,writeAifthestatementisapropertyofanacid,writeBifthepropertyisthatofabase,andwriteX,ifitisapropertyofbothacidicandbasicsolutions.Completethechart.

Answerthefollowingquestions1. _____Whichspeciescanconductanelectriccurrent?

1. H2O(s) 2. CH3OH(aq)

3. NaOH(s)4. HCl(aq)

2. _____AccordingtoArrheniustheory,whichspeciesdoesanacidproduceinaqueous

solution?1. hydroxideions 2. sodiumions

3. hydrogenions4. chlorideions

3. _____WhichsubstanceisanArrheniusacid?

1. Mg(OH)2(aq) 2. LiF(aq)

3. CH3CHO(aq)4. HBr(aq)

4. _____AccordingtotheArrheniustheory,whenabaseisdissolvedinwater,itproducesa

solutioncontainingonlyonekindofnegativeion.Whatisthenameofthisnegativeion?

1. hydrogensulfateion2. hydrogencarbonateion

3. hydrideion4. hydroxideion

5. IntermsofH+ions,explainthedifferencebetweenmonoprotic,diproticandtriprotic

acids.

Substance Acid,BaseorSalt?

Howdoyouknow?

1. NaOH 2. HCl 3. NaCl 4. HF 5. K2SO4 6. Fe(OH)3 7. H3PO4

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Arrhenius Acids and Bases

A)B)C)D)

1. Which compounds are classified as Arrhenius acids?

A) the behavior of many acids and basesB) the effect of stress on a phase equilibriumC) the operation of an electrochemical cellD) the spontaneous decay of some nuclei

2. What can be explained by the Arrhenius theory?

A) OH– ions B) O2– ionsC) K+ ions D) H+ ions

3. Potassium hydroxide is classified as an Arrheniusbase because KOH contains

A) a salt B) a hydrocarbonC) an Arrhenius acid D) an Arrhenius base

4. When one compound dissolves in water, the onlypositive ion produced in the solution isH3O+ (aq). This compound is classified as

A) hydroxide B) hydroniumC) hypochlorite D) perchlorate

5. Given the equation:

HCl(g) + H2O( ) X(aq) + Cl–(aq)Which ion is represented by X?

A) ammonium ion B) hydronium ionC) hydroxide ion D) sulfate ion

6. The only positive ion found in H2SO4(aq) is the

A) Ba(OH)2 B) CH3COOCH3

C) H3PO4 D) NaCl

7. Which substance is an Arrhenius acid?

A) CH3COOH and CH3CH2OHB) HC2H3O2 and H3PO4

C) KHCO3 and KHSO4

D) NaSCN and Na2S2O

8. Which two formulas represent Arrhenius acids?

A) HC2H3O2(aq) + NaOH(aq) NaC2H3O2(aq) +H2O( )

B) C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O( )C) Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g)D) BaCl2(aq) + Na2SO4(aq) BaSO4(s) + 2

NaCl(aq)

9. Which chemical equation represents the reaction of anArrhenius acid and an Arrhenius base?

A) CO32– as the only negative ion in solutionB) OH– as the only negative ion in solutionC) NH4+ as the only positive ion in solutionD) H+ as the only positive ion in solution

10. According to the Arrhenius theory, when a basedissolves in water it produces

A) Mg(OH)2 B) C2H4(OH)2

C) MgCl2 D) CH3Cl

11. Which substance yields hydroxide ion as the onlynegative ion in aqueous solution?

A) KOH, Ca(OH)2, and CH3OHB) KOH, NaOH, and LiOHC) LiOH, Ca(OH)2, and C2H4(OH)2

D) NaOH, Ca(OH)2, and CH3COOH

12. According to the Arrhenius theory, which list ofcompounds includes only bases?

12



6. Identifyeachofthefollowingacidsasmonoprotic,diproticortriproticandstatehowmanyH+ionsarereleasedinsolution.

1. H2CO32. H3PO43. HNO34. CH3COOH

5. H2SO46. HCl7. C2H5COOH8. H2S

Video13.2:ElectrolytesAnswerthequestionsbelowbasedontheinformationaboveandonyourknowledgeofchemistry.1. Usingthediagrambelow,drawadiagramofthemoleculeformedwhenonehydrogen

(proton)ispulledoffonewatermoleculeandattachedtoanother.

2. Whataretheformulasoftheionsformed?

3. Writeanequationshowingtheformationoftheionsfromtwomoleculesofwater.

4. Thehydroniumion(H3O+)andthehydroxideion(OH-)areformedbythereaction

betweenwatermolecules.Whatwouldformfromthereactionbetweenhydroniumandhydroxideions?Writeanequationshowingthereaction.

5. Howdoesthereactionbetweenwatermoleculescomparetothereactionbetweenhydroniumandhydroxideions?

6. Purewaterisactuallyamixtureofwatermolecules,hydroniumions,andhydroxideions:

a. Howdoestheconcentrationofhydroxideionscomparetotheconcentrationofhydroniumionsinpurewater?Explain

b. Howdoestheconcentrationofionscomparetotheconcentrationofmoleculesinpurewater?

13

Electrolytes

A)B)C)D)

1. Which two compounds are electrolytes?

A) saturated hydrocarbons B) alcoholsC) alkynes D) organic acids

2. Which compounds can be classified as electrolytes?

A) electrical conductivity of KCl(aq)B) pH of KCl(s)C) electrical conductivity of KCl(s)D) pH of KCl(aq)

3. Which laboratory test result can be used to determine if KCl(s) isan electrolyte?

A) 1.0 L of 2.0 M HCI(aq)B) 2.0 L of 2.0 M HCI(aq)C) 3.0 L of 0.50 M HCI(aq)D) 4.0 L of 0.50 M HCI(aq)

4. Which sample of HCI(aq) contains the greatest number of molesof solute particles?

A) increases because the concentration of ions decreasesB) decreases, but the concentration of ions remains the sameC) increases, but the concentration of ions remains the sameD) decreases because the concentration of ions decreases

5. As water is added to a 0.10 M NaCl aqueous solution, theconductivity of the resulting solution

A) C2H5OH B) CC14

C) CH3COOH D) CH4

6. Which compound dissolves in water to form an aqueous solutionthat can conduct an electric current?

A) LiOH B) LiBr C) CH3OH D) HBr

7. A student tested a 0.1 M aqueous solution and made thefollowing observations:• conducts electricity• turns blue litmus to red• reacts with Zn(s) to produce gas bubbles

Which compound could be the solute in this solution?

A) 1.0 M NaOH B) 0.10 M NaOHC) 0.10 M CH3OH D) 1.0 M CH3OH

8. Which of the following aqueous solutions is the best conductor ofelectricity?

A) barium sulfate B) sodium nitrateC) silver chloride D) magnesium carbonate

9. Based on Reference Table F, which of these salts is the bestelectrolyte?

A) K2SO4(aq) B) NaCl(aq)C) HCl(aq) D) C6H12O6(aq)

10. An example of a nonelectrolyte is

A) C12H22O11(aq) B) LiOH(aq)C) C6Hl2O6(aq) D) CH3OH(aq)

11. The diagram below shows an apparatus used to test theconductivity of various materials.

Which aqueous solution will cause the bulb to light?

A) A and D B) C and DC) B and C D) A and B

12. Beakers A, B, C, and D shown below each contain a differentsolution.

The bulb will glow when the conductivity apparatus is placedinto which beakers?

14



Completethefollowingreactions,balanceandindicatephaseoftheproducts

1. ____HNO3(aq)+____Mg(s)à

2. ____H2SO4(aq)+____Li(s)à

3. ____HBr(aq)+____Zn(s)à

4. Aluminummetalreactsw/phosphoricacid.

5. Calciummetalreactsw/hydrochloricacidUsingTableJanswerthefollowingquestions.

1. Whydoesgoldoccuruncombinedwhereaszincdoesnot?_________________________________________________________________________________________________

2. Whywassilverusedtomakecoinsinthepast?_________________________________________________________________________________________________

3. Whyiscopperusedtomakeelectricalwiresandcables?_________________________________________________________________________________________________

4. WhydoweknowlittleaboutthelifestylesofthepeopleoftheIronAge?_________________________________________________________________________________________________

Video13.3:ConjugateAcid-BasePairsOperationalDefinition:Acidsandbasesarechemicalspeciesthatexhibitdistinctivesetsofobservableproperties.Acidstastesour,basesarebitter.ConceptualDefinitions:Acidsandbasesaredefinedconceptuallytohelpaccountforwhatishappeningonthemicroscopiclevel. ArrheniusConcept:Anacidisasubstancethatwhendissolvedinwaterformshydrogenions(H+).Abaseisasubstancethatwhendissolvedinwaterproduceshydroxideions(OH-).ThisconceptislimitedbecauseotherchemicalshaveoperationalacidorbasepropertiesbutdonotformH+orOH-.Anexamplewouldbeammonia(NH3)hasbasicpropertiesbutdoesn’tcontainhydroxideions. AlternateAcidBaseConcept(Bronsted-Lowry):Anacidisaproton(H+)donorandabaseisaproton(H+)acceptor.

15



HF+H2O⇔H3O++F- AcidBaseC.AcidC.Base

Fillinthefollowingtable.Identifytheacid,base,conjugateacidandconjugatebaseineachoftheequations.

6. Writetheequationthatshowsammonia,NH3reactingwithhydrobromicacid,HBr.Labeltheacid,thebase,theconjugateacidandtheconjugatebase.

7. Writetheequationthatshowsthereactionofhydrogensulfide,HS-withhydroxideion,OH-.Labeltheacid,thebase,theconjugateacidandtheconjugatebase.

Video13.4:pH&Acid-BaseIndicatorsIndicators:GiventhepHofthefollowingsubstances,usetableMofyourreferencetodeterminewhatcolortheindicatorwillturnwhenplacedineachsubstance.

Equation Acid Base ConjugateAcid

ConjugateBase

1. HCl+NH3àNH4+Cl-

2. PO43-+HNO3àNO3-+HPO42-

3. HCO3-+OH-àH2O+CO32-

4. NH4++H2OàNH3+H3O+

5. HPO42-+H2OàOH-H2PO4-

Solution pHRange

MethylOrange

Bromthymolblue

Phenolphthalein Litmus Bromcresolgreen

Thymolblue

Acid/Base

Vinegar 1.3Soap 8.4Cola 3.2Ammonia 12Coffee 5.2

16

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Foreachquestion,thetwopHvaluesarebeingcompared.HowmanytimesstrongerorweakeristhepHofthesolution?

1. pH5àpH3 ___________________________________

2. pH8àpH4 ___________________________________

3. pH10àpH7 ___________________________________

4. pH14àpH7 ___________________________________

5. pH3àpH6 ___________________________________

Video13.5:Neutralization&TitrationsCompleteandbalanceeachoftheacidbaseneutralizationreactionsbelow. 1. _____H2SO4+_____Mg(OH)2à

2. _____HNO3+_____Al(OH)3à

3. _____H3PO4+_____Ca(OH)2à

4. _____HI+_____KOHà

5. _____HBr+_____Ba(OH)2à

6. _____HCl+_____KOHà

7. _____H3PO4+_____LiOHà

8. _____HF+_____Ca(OH)2à

9. InatitrationofHClO4withNaOH,100.0mLofthebasewasrequiredtoneutralize20.0mLof5.0MHClO4.WhatisthemolarityoftheNaOH?(Besuretowritetheneutralizationreaction.)

10. InatitrationofHNO3withNaOH,60.0mLof0.020MNaOHwasneededtoneutralize15.0mLofHNO3.Whatisthemolarityoftheacid?(Writetheneutralizationreaction.)

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11. If10.0mLof0.300MKOHarerequiredtoneutralize30.0mLofstomachacid(HCl),whatisthemolarityofthestomachacid?(Writetheneutralizationreaction.)

12. Ifittakes50mLof0.5MKOHsolutiontocompletelyneutralize125mLofsulfuricacidsolution(H2SO4),whatistheconcentrationoftheH2SO4solution?

TitrationPractice:AtitrationwassetupandusedtodeterminetheunknownmolarconcentrationofasolutionofNaOH.A1.2MHClsolutionwasusedasthetitrationstandard.Thefollowingdatawerecollected.

Trial1 Trial2 Trial3 Trial4Volumeof1.2M

HCl10.0mL 10.0mL 10.0mL 10.0mL

IntialburetreadingofNaOH

0.0mL 12.2mL 23.2mL 35.2mL

FinalburetreadingofNaOH

12.2mL 23.2mL 35.2mL 47.7mL

VolumeofNaOHused(mL)

MolarityofNaOH(M)

1. CalculatethevolumeofNaOHusedtoneutralizetheacidforeachtrial.Recordinthedatatableabove.Showonesamplecalculationbelow.

2. UsingtheMAVA=MBVBformula,calculatethemolarityofthebaseforeachtrial.Recordinthedatatableabove.Showonesamplecalculationbelow.

3. CalculatetheaveragemolarityoftheNaOHusingyourresultsfromquestion2.Youranswermustincludethecorrectnumberofsignificantfiguresandthecorrectunitsofmeasure.

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name: regents chemistry: dr. shanzer practice...

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