IB Chemistry on Acid Base, pH Scale and Ionic Product Water, Kw
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Transcript of IB Chemistry on Acid Base, pH Scale and Ionic Product Water, Kw
Brønsted-Lowry Acid - substance that donate proton/proton donor Bronsted-Lowry Base – substance that accept proton/proton acceptor One species donate proton – one species accept proton
Arrhenius acid - substance dissociate in water produce H+ ion. Arrhenius base – substance dissociate in water produce OH- ion. All Arrhenius acid are Bronsted Lowry acid and water must be present
HCI → H+ + CI-
HCI + H2O ↔ H3O+ + CI-
NaOH → Na+ + OH-
NH3 + H2O ↔ NH4+ + OH-
CO32- + H2O ↔ HCO3
- + OH-
Water/aqueous medium
Water/aqueous medium Other solvent medium possible
Definition of Acid and Bases
Arrhenius acid Arrhenius base H+ OH-
2
1
gain H+
Acid + Base ↔ Conjugate Base + Conjugate Acid
lose H+
HCI (acid) - CI- (conjugate base)
lose H+
H2O (base) - H3O+ (conjugate acid)
HCI + H2O ↔ CI- + H3O+
gain H+
Lewis Acid - substance that accept electron/electron acceptor, empty orbital/electron deficient Lewis Base – substance that donate electron/electron donor, lone pair electron Lewis Base - donate electron pair forming dative/coordinate bond with Lewis acid
3
HCI + H2O → CI- + H3O+
H2O donate e- HCI accept e-
Lewis acid Lewis base
Conjugate acid base pair differ by one proton
Physical properties of Acid
• Substance dissolves in water produce hydrogen ion/H+ or hydronium /H3O+
• HCI → H+ + CI- • Conduct electricity – free moving ions • Sour, pH < 7 • Turn blue litmus red
• Turn phenolphthalein colourless
• Turns methyl orange to red
Properties of Acids and Bases
Acid + Metal (above H) → Salt + H2 gas 2HCI + Mg → MgCI2 + H2
Acid + Base → Salt + Water + product. Bases are - Metal Hydroxide, Metal Oxide, Metal Carbonates Acid + Metal Hydroxide → Salt + Water Acid + Metal Oxide → Salt + Water Acid + Metal Carbonate → Salt + Water + Carbon Dioxide
Acid + Ammoniaaq and Amines → Salt + water HCI + NH4OH → NH4CI + H2O
HCI + CH3NH2 → CH3NH3 + CI-
Chemical properties of Acids / Bases
Physical properties of Acid
Physical properties of Bases • Substance dissolves in water produce hydroxide/OH- ion
• NaOH → Na+ + OH- • Conduct electricity – free moving ions • Bitter, pH > 7 • Turns red litmus blue
• Turns phenolphthalein pink
• Turns methyl orange to yellow
Physical properties of Base
Physical Properties Chemical Properties Physical Properties
Chemical Properties
Hydronium/Hydroxonium/Oxonium
Physical properties of Acid
• Electrolytes, produce H3O+, hydronium ion
• Conduct electricity • Sour, pH < 7 • Turn litmus red • Turn phenolphthalein colourless • Turn methyl orange to red
Physical properties of Base
• Bitter, pH > 7
• Turn litmus blue • Turn phenolphthalein pink • Turn methyl orange to yellow
Physical/Chemical Properties of Acids and Bases
Chemical properties of Acid / Base Physical properties of Acid/Base
Bases
Acid + Metal Hydroxide (Alkali) → Salt + Water LiOH + HCI → LiCI + H2O
NaOH + HNO3 → NaNO3 + H2O KOH + H2SO4 → K2SO4 + H2O
Acid + Metal Hydroxide (Insoluble) → Salt + Water Ca(OH)2 + 2HCI → CaCI2 + 2H2O
Fe(OH)2 + 2HNO3 → Fe(NO3)2 + 2H2O
Mg(OH)2 + H2SO4 → MgSO4 + 2H2O
Acid + Metal Oxide → Salt + Water CaO + 2HCI → CaCI2 + H2O
CuO + 2HCI → CuCI2 + H2O
Acid + Alkali
Acids + Metal Oxide
Acid + Metal Hydroxide
Acid + Metal Carbonate
Acid + Metal Carbonate → Salt, Water + CO2
CaCO3 + 2HCI → CaCI2 + H2O + CO2
CuCO3 + 2HCI → CuCI2 + H2O + CO2
Acid + Metal (above H) → Salt + H2 gas 2HCI + Mg → MgCI2 + H2
Acid + Base → Salt + Water + product. Bases are - Metal Hydroxide, Metal Oxide, Metal Carbonate Acid + Metal Hydroxide → Salt + Water Acid + Metal Oxide → Salt + Water Acid + Metal Carbonate → Salt + Water + Carbon Dioxide Acid + Ammoniaaq and Amines → Salt + water HCI + NH4OH → NH4CI + H2O
HCI + CH3NH2 → CH3NH3 + CI-
CH3COOH ↔ H+ + CH3COO-
(1 mole) (0.01 mole)
Strong Acid / Base Weak Acid / Base
Strong acid – ionise/dissociate completely producing H+ ion Strong base – ionise/dissociate completely producing OH- ion All are in ions state, NO molecule left Strong electrolyte with high conductivity ↑
Weak acid – ionise/dissociate partially producing H+ ion Weak base – ionise/dissociate partially producing OH- ion Most in undissociated molecule form Poor electrolyte with low conductivity ↓
HCI → H+ + CI- HBr → H+ + Br−
Monoprotic acid - 1 mole H+ ion
Diprotic acid - 2 mole H+ ion
H2SO4 → 2H+ + SO42-
(1 mole) (2 mole)
Strong Acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4
Strong Base - LiOH, KOH, NaOH, CsOH, Ca(OH)2, Ba(OH)2 Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, HNO2, H3PO4
Weak Base - NH3, C2H5NH2 , CH3NH2, (CH3)2NH, C3H5O2NH2
Weak acid dissociate partially produce few H+ ion
NH3 + H2O ↔ NH4+ + OH-
C2H5NH2 + H2O ↔ C2H5NH3+ + OH-
CO32- + H2O ↔ HCO3
- + OH-
Weak base dissociate partially produce few OH- ion
Vs
Example of Strong Acid/Base Example of Weak Acid/Base
Ba(OH)2 → Ba2+ + 2OH−
(1 mole) (2 mole)
(1 mole) (1 mole) Dissociate completely No molecules left
All ion form Few ions form
Dissociate partially Molecules left
Monoprotic base - Accept 1 mole H+ ions by 1mole OH-
Na(OH) → Na+ + OH−
(1 mole) (1 mole)
All ion form Dissociate completely No molecules left
Few ions form
Dissociate partially Molecules left
H3PO4 ↔ H+ + H2PO4
-
H2PO4- ↔ H+ + HPO4
2-
HPO42- ↔ H+ + PO4
3- H3PO4
↔ 3H+ + PO43-
Diprotic base - Accept 2 mole H+ ions by 2 mole OH-
Weak triprotic acid dissociate partially produce few H+ ion
One way reversible
reversible
One way
One way
reversible
CH3COOH ↔ H+ + CH3COO-
(1 mole) (0.01 mole)
Strong Acid / Base Weak Acid / Base
Strong acid – ionise/dissociate completely producing H+ ion Strong base – ionise/dissociate completely producing OH- ion All are in ionic ions state Strong electrolyte with high conductivity ↑
Weak acid – ionise/dissociate partially producing H+ ion Weak base – ionise/dissociate partially producing OH- ion Most in undissociated molecule form Poor electrolyte with low conductivity ↓
HCI → H+ + CI- HBr → H+ + Br−
Monoprotic acid - produce 1 mole H+ ions
Diprotic acid - 2 mole H+
H2SO4 → 2H+ + SO42-
Strong acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4
Strong base - LiOH, KOH, NaOH, CsOH, Ca(OH)2, Ba(OH)2
(1 mole) (2 mole)
Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, H3PO4
Weak Base - NH3, C2H5NH2 , (CH3)2NH, C3H5O2NH2
Weak acid dissociate partially produce few H+ ion
NH3 + H2O ↔ NH4+ + OH-
C2H5NH2 + H2O ↔ C2H5NH3+ + OH-
CO32- + H2O ↔ HCO3
- + OH-
Weak bases dissociate partially produce few OH- ion
Vs
Example Strong Acid/Base Example Weak Acid/Base
Concentrated Acid / Base Diluted Acid / Base
Concentrated Acid – High number of mole/amt of solute per dm3
1 M HCI – 1 mole of HCI molecules in 1 dm3
10 M HCI – 10 mole of HCI molecules in 1 dm3
Diluted Acid – Low number of mole/amt of solute per dm3
0.1M HCI – 0.1 mole of HCI molecule in 1 dm3
0.01M HCI – 0.01 mole of HCI molecule in 1 dm3
Concentrated Acid may NOT be a Strong Acid 10M CH3COOH – Concentrated Acid ↑ but Weak Acid ↓
Diluted Acid may be a Strong Acid 0.01M HCI – Diluted Acid ↓ but Strong Acid ↑
10M CH3COOH - CONCENTRATED WEAK acid because 10M acid molecule will dissociate partially forming few H+ ions
0.01M HCI - DILUTED STRONG acid because all 0.01M acid molecule dissociate fully forming H+ ions
Vs
Diprotic base - 2 mole OH-
Ba(OH)2 → Ba2+ + 2OH−
(1 mole) (2 mole)
(1 mole) (1 mole)
Strong/Weak Acid and Base
Strong Acid/Weak Acid
Strong acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4
Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, H3PO4
Strong Base/ Weak Base
Strong base - LiOH, KOH, NaOH, CsOH, Ca(OH)2
Weak Base - NH3, C2H5NH2, (CH3)2NH, C3H5O2NH2
Distinguish bet strong and weak acid
Electrical conductivity Rate of rxn pH
Strong acid
Strong acid → High ionization → High conc H+ → High conductivity → High rate rxn → Lower pH
Strong acid
Oxoacid O atom > number ionizable proton HNO3, H2SO4, HCIO3, HCIO4
Hydrohalic acid HI, HBr, HCI
Weak acid
Hydrohalic acid HF
Oxoacid O atom ≥ number ionizable proton by 1 HCIO, HNO2, H3PO4
Carboxylic acid COOH
Strong base – contain OH- or O2-
LiOH, NaOH, CaO, K2O Ca(OH)2, Ba(OH)2
Weak base – contain electron rich nitrogen, N NH3, C2H5NH2, (CH3)2NH, C3H5O2NH2
Strong base Weak base
1 2 3
Weak acid
0.1 M HCI 0.1 M CH3COOH
H+ 0.1 mole 0.0013 mole
pH 1 (Low) 2.87 (High)
Electrical conductivity High (Ionize completely) Low (Ionize partially)
Rate with magnesium Fast Slow
Rate with calcium carbonate
Fast Slow
Weaker acid → Low ionization → Low conc H+ → Low conductivity → Low rate rxn → High pH
Strong acid
HA A- H+
H+ H+
H+
H+ H+
H+
H+ A-
A-
A-
A- A-
A-
Ionizes completely
Weak acid
HA HA
H+ A- H+
H+
A-
A- HA
HA
HA
HA
HA
HA
Ionizes partially
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+]
Conc OH- increase ↑ by 10x
pH increase ↑ by 1 unit
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)
pH with Conc H+
pH = -log [H+] [H+] = 0.0000001M pH = -log [0.0000001] pH = -log1010-7
pH = 7 (Neutral)
Conc H+ increase ↑ by 10x
pH decrease ↓ by 1 unit
pH measurement of Acidity of solution
• pH is the measure of acidity of solution in logarithmic scale • pH = power of hydrogen or minus logarithm to base ten of hydrogen ion concentration
← Acidic – pH < 7 Alkaline – pH > 7 →
pOH with Conc OH-
pOH = -log [OH-] [OH-] = 0.1M pOH = -log[0.1] pOH = 1 pH + pOH = 14 pH + 1 = 14
pH = 13 (Alkaline)
pH with Conc H+
pH = -log [H+] [H+] = 0.01M pH = -log [0.01] pH = -log1010-2
pH = 2 (Acidic)
Easier pH scale Conc H+
Conc [H+] = 1 x 10-12 pH = -lg[H+] pH = -lg[10-12] pH = 12
Conc [OH-]= 1 x 10-2 pOH = -log10[OH-]
pOH = -log1010-2 = pOH = 2 pH + pOH = 14 pH + 2 = 14 pH = 12
Conc [H+] = 1 x 10-2 pH = -lg[H+] pH = -lg[10-2] pH = 2
Alkaline
Alkaline
Acidic
Acidic
Kw - Ionic product constant water
Using conc [H+] pH = -log10[H+]
pH = -log10[H+] pOH = -log10[OH-] pH + pOH = 14 Kw = [H+][OH-]
Using conc [OH-] pOH = -log10[OH-]
Conc[OH-]= 1 x 10-12 pOH = -log10[OH-]
pOH= -log1010-12 =pOH = 12 pH + pOH = 14 pH + 12 = 14 pH = 2
Formula for acid/base calculation
22
3
OH
OHOHKc
OHOHOHKc 3
22
OHOHKw 3
OHOH3
14100.1
7714 101101100.1
7101 OH
OHOHOHOH 322
H2O dissociate forming H3O+ and OH- (equilibrium exist)
14100.1 wK
Dissociation water small [H2O] is constant
Kw = 1.0 x 10-14 Ionic Product constant water at -25C
Kc - Dissociation constant water
7
3 101 OH
0.2
01.0log
log
10
10
pH
pH
HpH
22
3
OH
OHOHKc
OHOHKOHK wc 3
22
OHOH3
14100.1 7714 101101100.1
OHOHOHOH 322
H2O dissociate forming H3O+ and OH- (equilibrium exist)
14100.1 wK
Dissociation water small [H2O] is constant
Kw - Ionic product constant water Kw = 1.0 x 10-14 Ionic Product constant water at -25C
Kc - Dissociation constant water
Cal conc of H+ ,OH- and pH of water Cal conc of H+ ,OH- and pH of 0.01M HCI
OHHOH2
OHHKw
OHH14100.1
7714 101101100.1
7101 H
H2O H2O
HCI
OHHOH2
H2O
OHHKw
OHH14100.1
Assuming H+ all from HCI = 0.01
)()( 2OHHHCIHH
H+ = 0.01 + 1.0x10-12
= 0.01 + 0.000000000001 ≈ 0.01
OHHOH2
H+ = 1x10-12 OH- = 1x10-12
CIHHCI0.01 mol 0.01 mol 0.01
1 mol ↔ 1 mol 1mol
0.000000000001
0.000000000001
H+ OH-
= 0.01 = 0.000000000001
or
0.7
101log 7
10
pH
pH
0.21214
12
100.101.0
100.1
01.0100.1
1214
14
pH
pOH
OH
OH
22
3
OH
OHOHKc
OHOHKOHK wc 3
22
OHOH3
14100.1 7714 101101100.1
OHOHOHOH 322
H2O dissociate forming H3O+ and OH- (equilibrium exist)
14100.1 wK
Dissociation water small [H2O] is constant
Kw - Ionic product constant water Kw = 1.0 x 10-14 Ionic Product constant water at -25C
Kc - Dissociation constant water
Cal conc of H+ ,OH- and pH of 0.01M KOH Cal conc of H+ ,OH- and pH of 0.1M H2SO4
7.0
2.0log
log
10
10
pH
pH
HpH
H2O
KOH
H2SO4
OHHOH2
H2O
OHHKw
OHH14100.1
Assuming H+ all from H2SO4 = 0.2
7.03.1314
3.13
100.52.0
100.1
2.0100.1
1414
14
pH
pOH
OH
OH
)()( 242 OHHSOHHH
H+ = 0.2 + 5 x 10-14
= 0.2 + 0.000000000000005 ≈ 0.2
OHHOH2
H+ = 5x10-14 OH- = 5x10-14
2
442 2 SOHSOH
0.1 mol 0.2 mol
0.2
1 mol ↔ 1 mol 1 mol
0.00000000000005
0.0000000000005
H+ OH-
= 0.2 = 0.00000000000005
OHHOH2
1 mol ↔ 1 mol 1 mol
OHHOH2
OHHKw
OHKKOH0.01 mol 0.01 mol
0.01
Assuming OH- all from KOH = 0.01
)()( 2OHOHKOHOHOH
= 0.01 = 0.000000000001
12
10log
log
10101.0
100.1
01.0100.1
12
10
10
1214
14
pH
pH
HpH
H
H
or
H+ = 1x10-12 OH- = 1x10-12
Number sig fig in log calculation Significant number in log calculation
log10(3575)=3.55327 = 3.5532
log10(3.000x104) = 4.477121 = 4.4771 log10(3.3 x 104) = 4.5185 = 4.51 Calculation involve pH = -log10[H+]
Conc H+ = 1.9 x 10-4
pH= -log10[1.9 x 10-4] = 3.721 = 3.72
Measurement scale not linear • Simple average CANNOT be used • Average of pH 7, pH 8, pH 9 pH scale is logarithmic, pH = -log[H+] Correct average = convert to H+ conc pH 7 = -log10[H+] → H+ = 10-7
pH 8 = -log10[H+] → H+ = 10-8
pH 9 = -log10[H+] → H+ = 10-9
pH pH= -lg10H+ Conc H+
0 0 = -lg10100 1.0
1 1 = -lg1010-1 0.1
2 2 = -lg1010-2 0.01
3 3 = -lg1010-3 0.001
4 4 = -lg1010-4 0.0001
5 5 = -lg1010-5 0.00001
6 6 = -lg1010-6 0.000001
7 7 = -lg1010-7 0.0000001
8 8 = -lg1010-8 0.00000001
9 9 = -lg1010-9 0.000000001
10 10= -lg1010-10 0.0000000001
11 11= -lg1010-11 0.00000000001
12 12= -lg1010-12 0.000000000001
13 13= -lg1010-13 0.0000000000001
14 14= -lg1010-14 0.00000000000001
Easier using pH scale than Conc [H+] • Low pH – High H+ conc – More acidic • High pH – Low H+ conc – Less acidic • pH 3 (10x) more acidic > than pH 4 • 1 unit change in pH is 10 fold change in Conc [H+]
Relationship between pH and Conc H+
Uncertainty involving pH
83
987
Average
Uncertainty involving pH
4 sig fig 5 sig fig/4 decimal place
4 sig fig 5 sig fig/4 decimal place
Conc H+ = 3.2 x 10-5 M
pH = - log10[3.2 x 10-5]= 4.4948 = 4.49
2 sig fig 3 sig fig/2 decimal place
2 sig fig 3sig fig/2 decimal place
2 sig fig 3sig fig/2 decimal place
2 sig fig 3sig fig
2 sig fig 3 sig fig
2 sig fig 3 sig fig
pH solution = 7.40. Cal conc of H+ ions
7.40 = -log10 [H+] [H+] = 10-7.40
= 4.0 x 10-8
3 sig fig 2 sig fig
2 sig fig
4.7
]107.3lg[
107.3
3
101010
8
8
987
pH
pH
Average
Average
What is pH for [H+] = 1 x 10-12 M pH = -lg [10-12]
pH = 12
What is conc of H+ of pH 3.20?
3.20 = -lg [H+] [H+] = 10 –2.20
[H+] = 6.3 x 10-4
pH = -log10[H+] pOH = -log10[OH-] pH + pOH = 14 Kw = [H+][OH-]
Formula acid/base calculation
2 sig fig 1 sig fig 3 sig fig 2 sig fig
What is pH for [OH-] = 0.15M pOH = -lg [0.15] pOH = 0.823 pH + pOH = 14 pH = 14 – 0.823 = 13.2
pOH = -log[OH-]
3 sig fig 2 sig fig
Calculate conc of H+, OH- and pH for 0.0010M HCI.
1 2 3
4
CIHHCI0.001 ↔ 0.001 0.001
OHHOH2
HCI H2O
OHHKwAssuming H+ all from HCI = 0.0010
)()( 2OHHHCIHH
= 0.001 Negligible / too little
OHH14100.1
0.3
001.0log
log
10
10
pH
pH
HpH
0.31114
11
101001.0
100.1
001.0100.1
1114
14
pH
pOH
OH
OH
or
Cal conc OH-/pH when 3.o x 10-4 H+ add water
HCI H2O
CIHHCI OHHOH2
OHHKw
OHH14100.1
11
4
14
414
103.3100.3
100.1
100.3100.1
OH
OH
3x10-4 ↔ 3x10-4
52.3
100.3log
log
4
10
10
pH
pH
HpH
pH weak acid at various concentration
HCOOCHOHCOOHCH 2323
Extend of dissociation depend on initial concentration acid
Conc of acid Observed pH CH3COOH Calculated pH HCI
0.10 2.7 1.0
0.010 3.0 2.0
0.0010 3.5 3.0
0.00010 4.2 4.0
CIHHCI
Weak acid Strong acid
Dissociate partially Dissociate completely
At same acid concentration • HCI has HIGHER [H+] > CH3COOH
• HCI has LOWER pH < CH3COOH • HCI dissociate completely - Strong acid • CH3COOH dissociate partially - Weak acid
At decreasing acid concentration • Extend of dissociation for CH3COOH increase • pH weak acid closer to strong acid • Dilution increase the extend of dissociation
Conc decrease
HCOOCHOHCOOHCH 2323
Trends
Addition Water
Dilution shift equilibrium to right
Decrease conc of CH3COOH, CH3COO- and H+
Conc on left side is more effected due to CH3COO- and H+
Equilibrium shift to right to increase conc of CH3COO- and H+ again
Extend of dissociation for acid increase (shift to right)
О
О
Concept Map
[H+] [OH-]
pH pOH
Kw = [H+] x [OH-] = 1 x 10-14
pH + pOH = 14
pH = -lg [H+] [H+] = 10-pH pOH = -lg [OH-] [OH-] = 10-pOH
Question on Acid and Base
Which list contains only strong acids ? A. CH3COOH, H2CO3, H3PO4
B. HCI, HNO3, H2CO3
C. CH3COOH, HNO3, H2SO4
D. HCI, HNO3, H2SO4
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 < KOH B. HNO3 < CH3COOH < CH3CH2NH2 < KOH C. CH3CH2NH2 < HNO3 < CH3COOH < KOH D. KOH < CH3CH2NH2 < CH3COOH < HNO3
pH 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 100
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 B B. [A] > [B] C. Concentration of H+ ions in A is higher than B D. Concentration of H+ ions in B is twice the concentration of H+ in A
100ml of NaOH solution of pH 12 is mixed with 900ml of water. What is the pH of resulting solution? A. 1 B. 3 C. 11 D. 13
1
2
3
4
5
О
О
О
О
О
List two ways to distinguish between strong and weak acid/base 6
By Conductivity measurement
1M Strong Acid – Ionise completely – More H+ ion – pH lower ↓ 1M Weak Acid – Ionise partially – Less H+ ion – pH higher ↑
1M Strong Acid – Ionise completely – More H+ ion – Conductivity higher ↑ 1M Weak Acid – Ionise partially – Less H+ ion – Conductivity lower ↓
By pH measurement
Which method will distinguish bet equimolar strong base and strong acid? i) Add magnesium to each solution and observe formation bubbles ii) Add aqueous sodium hydroxide to each solution and measure temp change iii) Use each solution in circuit with battery/lamp to see brightness lamp
7
О О
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