chapters 13-14
DESCRIPTION
Chapters 13-14. Acids, Bases, Buffers. Common Acids. HCl HNO 3 H 2 SO 4 H 3 PO 4 H 4 SiO 4 HBr H I H 2 SO 3 Patterns?. Common Acids. HCl HNO 3 H 2 SO 4 H 3 PO 4 H 4 SiO 4 HBr H I H 2 SO 3 Patterns? All contain H. - PowerPoint PPT PresentationTRANSCRIPT
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Chapters 13-14
Acids, Bases, Buffers
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Common AcidsHClHNO3H2SO4H3PO4H4SiO4HBrHIH2SO3
Patterns?
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Common AcidsHClHNO3H2SO4H3PO4H4SiO4HBrHIH2SO3 Patterns? All contain H. H was written first.
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Common BasesNaOHLiOHKOHCa(OH)3Ba(OH)2Mg(OH)2Al(OH)3Si(OH)4 NH4OH Patterns?
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Common BasesNaOHLiOHKOHCa(OH)3Ba(OH)2Mg(OH)2Al(OH)3Si(OH)4 NH4OH Patterns? all contain OH, written second.
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DefinitionsArrhenius - (common)(specific) Acid - releases contained H+ ions Base - releases contained OH- ions
Bronsted - Lowry Acid - proton (H+) donor Base - proton (H+) acceptor
Lewis (general) Acid - accepts an electron pair Base - donates an electron pair
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Conjugate Acid-Base Pairs(B-L)
HB(aq) + A-(aq) HA (aq) + B -(aq)
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Conjugate Acid-Base Pairs(B-L)
HB(aq) + A-(aq) HA (aq) + B -(aq) D A D AWho donates, who acceptsconjugate acid base pairs
pair 1 D A Pair 2 D A
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Conjugate Acid-Base Pairs(B-L)
HB(aq) + A-(aq) HA (aq) + B -(aq) D A D AWho donates, who acceptsconjugate acid base pairs
pair 1 D A Pair 2 D A
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Conjugate Acid-Base Pairs(B-L)
HB(aq) + A-(aq) HA (aq) + B -(aq) D A D AWho donates, who acceptsconjugate acid base pairs
pair 1 D A Pair 2 A D
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Special CaseH2O(l) + H2O(l) H3O+(aq) + OH -(aq)
autoionization of waterOR
H2O(l) + H2O(l) H+(aq) + OH -(aq)
If the thought of naked protons running around in a pool does not bother you,
This is simpler!
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Special Case H2O(l) + H2O(l) H3O+(aq) + OH -(aq)
autoionization of waterOR
H2O(l) + H2O(l) H+(aq) + OH -(aq)
If the thought of naked protons running around in a pool does not bother you,
This is simpler!
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Special CaseH2O(l) + H2O(l) H3O+(aq) + OH -(aq)
autoionization of waterOR
H2O(l) + H2O(l) H+(aq) + OH -(aq)
If the thought of naked protons running around in a pool does not bother you,
This is simpler!
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Special CaseH2O(l) + H2O(l) H3O+(aq) + OH -(aq)
autoionization of waterOR
H2O(l) + H2O(l) H+(aq) + OH -(aq)
If the thought of naked protons running around in a pool does not bother you,
this is simpler!
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K #3H2O(l) + H2O(l) H+(aq) + OH -(aq)
Keq(water) = Kw = H+(aq)OH-(aq)1 x 10-14
Why is the water not included???H+(aq)OH-(aq)means water is neutral. H+(aq)OH-(aq)1 x 10-14
∴H+(aq)2 1 x 10-14 Why?
∴H+(aq) 1 x 10-7 neutralWhy?
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the power of Hydrogen ionsH+(aq) 1 x 10-7
neutralstronger weaker
H+(aq) 1 x 10-6 acid base? H+(aq) 1 x 10-5 acid base?H+(aq) 1 x 10-4 acid base?H+(aq) 1 x 10-3 acid base?H+(aq) 1 x 10-2 acid base?H+(aq) 1 x 10-1 acid base?H+(aq) 1 x 100 acid base?weaker stronger
? ?
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the power of Hydrogen ionsH+(aq) 1 x 10-7
neutralstronger weaker
H+(aq) 1 x 10-6 acid base? H+(aq) 1 x 10-5 acid base?H+(aq) 1 x 10-4 acid base?H+(aq) 1 x 10-3 acid base?H+(aq) 1 x 10-2 acid base?H+(aq) 1 x 10-1 acid base?H+(aq) 1 x 100 acid base?weaker stronger
? ?
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the power of Hydrogen ionsH+(aq) 1 x 10-7
= .0000001weaker
H+(aq) 1 x 10-6 = .000001 H+(aq) 1 x 10-5 = .00001 H+(aq) 1 x 10-4 = .0001 H+(aq) 1 x 10-3 = .001 H+(aq) 1 x 10-2 = .01 H+(aq) 1 x 10-1 = .1 H+(aq) 1 x 100 =1. we aker stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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the power of Hydrogen ionspHH+(aq) 1 x 10-7 = .00000017weaker
H+(aq) 1 x 10-6 = .000001 6H+(aq) 1 x 10-5 = .00001 5H+(aq) 1 x 10-4 = .0001 4H+(aq) 1 x 10-3 = .001 3H+(aq) 1 x 10-2 = .01 2H+(aq) 1 x 10-1 = .1 1H+(aq) 1 x 100 =1. 0 stronger
? ?
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Definitions and Other Stuff pH = - logH+pOH = - logOH-
As pH gets larger, acid content drops As pOH gets larger, base content drops
pH + pOH = 14 H+OH-= 1 x 10-14
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Acid-Base Differences Strong Acids Weak acids Strong Bases Weak bases
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Strong Acids (6 only)
HCl HBr HIHNO3 H2SO4 HClO4
HCl(aq) H+(aq)Cl-(aq)
So little product returns, reaction considered 100% ionized
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Weak acids
a) ionizable H+ HB(aq)H2O(l) B-(aq)H3O+(aq) OR HB(aq) B-(aq)H+(aq)
So little H+ ionizes, most of the acid molecule remains intact.
b) cations B+(aq)H2O(l) BOH(aq) H+(aq)Certain anions have the ability to promote H+ ionization.
So little product returns, reaction considered 100% ionized
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K #4 Weak acids
HB(aq)H2O(l) B-(aq)H3O+(aq)
HB(aq) B-(aq)H+(aq) weak acid ionization constant
Ka = H+B- = H3O+B- HB HB
pKa = -log Ka
So little product returns, reaction considered 100% ionized
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Polyprotic AcidsExample: H3PO4
H3PO4(aq) H2PO4-(aq) H+(aq)
H2PO4-(aq) HPO4-2(aq) H+(aq)
HPO4 -2(aq) PO4-3(aq) H+(aq)
K1 = H2PO4-H +K2 = HPO4 -2H +K3 = PO4 -
3H +H3PO4H2PO4-
HPO4 -2
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Polyprotic Acids Complex EquilibriaH3PO4(aq) H2PO4-(aq) HPO4-2(aq) PO4-3(aq) H+(aq) H+(aq) H+(aq)
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Strong Bases (6 only)
LiOH NaOH KOHCa(OH)2 Sr(OH)2 Ba(OH)2
LiOH(aq) Li+(aq)OH-(aq)
So little product returns, reaction considered 100% ionized
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Weak bases
a) molecules BH(aq)H2O(l) BH2+(aq)OH-(aq)Certain molecules have the ability to promote OH- ions
b) anions B-(aq)H2O(l) BH(aq) OH-(aq)
Certain anions have the ability to promote OH- ions
So little product returns, reaction considered 100% ionized
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K #5 Weak bases
BH(aq)H2O(l) BH2+(aq)OH-(aq)
B-(aq)H2O(l) BH(aq) OH-(aq)
Kb = BH+OH- =BHOH- BH B-
pKb = -log Kb
So little product returns, reaction considered 100% ionized
weak base ionization constant
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Relationships
(Ka)(Ka) = 1 x 10-14
pKa + pKa = 14
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Titration Possibilities
SASBSAWBWASBWAWB
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SASBStrong Acid
H+
Strong BaseOH-
Strong Acid-Strong BaseNet Ionic Equation
H+ + OH- H2O
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SAWBStrong Acid
H+ + OH- H2OWeak Base
BH + H2O BH2+ + OH-
B - + H2O BH + OH-
Net Ionic EquationBH + H+ BH2+
B - + H+ BH
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WASBStrong Base
H+ + OH- H2OWeak Acid
HB B - + H+
Net Ionic Equation HB + OH- B - + H2O
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WAWBWeak Base
BH + H2O BH2+ + OH-
D - + H2O DH + OH-
Weak Acid HB B - + H+
Net Ionic Equation BH + HB B - + BH2+
D - + HB B - + DH
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BuffersAbility to resist change
meter out change
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BuffersContain:weak acids conjugate bases example: HF H+ + F-
Ka = H+F- = 3.50 x 10-4 HF
H+= Ka HFF-
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Bufferssuppose: HF = .1,F-= .1 Ka = 3.50 x 10-4
H+= 3.50 x 10-4 .1.1
pH = - logH+ = 3.46
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Buffer Action HF H+ + F-
F- + H2O HF + OH-
Add .01 moles OH-
HF H+ + OH- + F-
.1-.01= .09 .1+.01= .11 H+ = 3.50 x 10-4(.09) (.11) pH = 3.50
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Buffer Action HF H+ + F-
F- + H2O HF + OH-
Add .01 moles H+
HF H+ + H+ + F-
.1+.01= .11 .1-.01= .09 H+ = 3.50 x 10-4(.11) (.09) pH = 3.37
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Buffer ActionpH ranged from 3.37 to 3.50 in this bufferCompare to: strong acid [H+] = 1.85 x 10-5 pH = 4.74 [H+] = 1.0 x 10-14 add .01 [OH-][OH-][H+] = 1.0 x 10-14 = 1.0 x 10-12
.01 pH = 12
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Summary of Buffer ActionBuffer / addition of .01 basepH ranged 3.46 to 3.50
No buffer / addition of .01 basepH range 4.74 to 12
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Titration:SASB50.00 ml of 1 M HCl titrate with 1 M NaOHbeginning pH = -log[1] = 0moles 1/1000 = x/50 = .05000
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Titration:SASBadd 25.00 ml OH-.05000 - .02500 = .02500 H+ in 75.00 ml [H+] = .3333 and pH = .4778
add 49.99 ml OH-.05000 - .04900 = .00001 H+ in 100.00 ml [H+] = .0001000 and pH = 4.000
add 50.00 ml OH-neutral so pH = 7.000
add 50.01 ml OH-.05000 - .05001 = .00001 OH- in 100.00 ml [OH-] = .0001000, pOH = 4.00, pH = 10.00
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Titration:SASBSummary:pH changed from 4 to 10 with the addition of .02 ml of OH-.
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Titration:WASBReview: acetic acid Hac H+ + ac-
Ka = H+ac-= H+2 = 1.8 x 10-5
HacH+ = 4.2 x 10-3 pH = 2.4
Titrate 50.00 ml of 1 M Hac with 1M NaOH
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Titration:WASBTitrate 50.00 ml of 1 M Hac with 1M NaOH* with 25.00 ml OH-
Hac H+ + OH- + ac-
.05000 - .02500 .02500 H+ = Ka HacThis is a bufferac-Hac=ac-∴H+ = Ka, pH = pKa pH = 4.700
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Titration:WASB*with 50.00 ml OH-, all Hac converted to ac- Hac H+
+ OH- + ac-.05000 - .05000 .05000equation is: ac- + H2O Hac + OH-
becomes a weak base in waterKb = [Hac][OH-] = [OH -]2
[ac-] [ac-][ac-] has same moles as original Hac, butin twice the water.Kb[ac-] = [OH-]2 5.6 x 10-10[.5000] = [OH-]2
[OH-]2 = 2.8 x 10-10 [OH-] = 1.7 x 10-5
pOH = 4.8 14 - 4.8 = 9.2 pH = 9.2
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Titration:WASBSUMMARY:pH range 2.4 to 9.2 full titrationhalf titration, pH = pKa
Remember this from SASB summary?pH changed from 4 to 10 with the addition of .02 ml of OH-