acids lesson 22 subtle items
DESCRIPTION
Acids Lesson 22 Subtle Items. 1. Weak bases neutralize a strong acid as well as a strong base would. Subtle Acid Items 1. Weak bases neutralize a strong acid as well as a strong base would. HCl +NaOH. Subtle Acid Items - PowerPoint PPT PresentationTRANSCRIPT
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AcidsLesson 22
Subtle Items
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1. Weak bases neutralize a strong acid as well as a strong
base would.
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Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would. HCl + NaOH
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Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH → NaCl + HOH
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Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH → NaCl + HOH
HCl + HCO3-
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Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH → NaCl + HOH
HCl + HCO3
- → H2CO3 + Cl-
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Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH → NaCl + HOH
HCl + HCO3
- → H2CO3 + Cl-
Both reactions go to completion because of the strong acid.
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2. H3BO3
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2. H3BO3 triprotic
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However,
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However,
H3BO3 + NaOH
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However, loses all three because of the strong base!
H3BO3 + 3NaOH → Na3BO3 + 3HOH
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However, loses all three because of the strong base!
H3BO3 + 3NaOH → Na3BO3 + 3HOH
HCl + NaOH →
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However, loses all three because of the strong base!
H3BO3 + 3NaOH → Na3BO3 + 3HOH
HCl + NaOH → NaCl + HOH
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However, loses all three because of the strong base!
H3BO3 + 3NaOH → Na3BO3 + 3HOH
HCl + NaOH → NaCl + HOH
Which neutralizes more NaOH, H3BO3 or HCl?
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2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However, loses all three because of the strong base!
H3BO3 + 3NaOH → Na3BO3 + 3HOH
HCl + 1NaOH→ NaCl + HOH
Which neutralizes more NaOH? H3BO3 or HCl?
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3. Which determines acid strength?
Molarity
pH =
Ka
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3. Which determines acid strength?
Molarity is concentration.
pH =
Ka
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3. Which determines acid strength?
Molarity is concentration.
pH = -Log[H+]
Ka
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3. Which determines acid strength?
Molarity is concentration.
pH = -Log[H+]
Ka is strength as indicated in the acid chart
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4. Which determines the pH.
Ka
Molarity
Temperature
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4. Which determines the pH = -Log[H+]
Ka
Molarity
Temperature
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4. Which determines the pH = -Log[H+]
Ka determines the [H+] and the pH
Molarity
Temperature
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4. Which determines the pH = -Log[H+]
Ka determines the [H+] and the pH
Molarity determines the [H+] and the pH
Temperature
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4. Which determines the pH = -Log[H+]
Ka determines the [H+] and the pH
Molarity determines the [H+] and the pH
Temperature determines the [H+] and the pH
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5. Pick the best conductor.
1 M NaOH 0.1 M HCl 0.01 M KOH
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5. Pick the best conductor.
1 M NaOH 0.1 M HCl 0.01 M KOH
All strong- highest Molarity!
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6. Pick the worst conductor.
NaOH HCl NaCN NH3
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6. Pick the worst conductor.
NaOH HCl NaCN NH3
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6. Pick the worst conductor.
NaOH HCl NaCN NH3
Good Conductors are…..
Strong acids
Strong Bases
Soluble Salts
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7. 1 mole H2CO3 and 1mole NaHCO3 are dissolved in 0.5 L of water.
What kind of solution results in the above mixture?
Buffer
Write an equation for the equilibrium.
H2CO3 ⇋ H+ + HCO3-
Label each chemical species with a concentration.
2 M Low 2 M
What limits the ability to buffer against acid?
[HCO3-]
What limits the ability to buffer against base?
[H2CO3]
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8. Acid Base
HF
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8. Acid Base
HF F-
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8. Acid Base
HF F-
H2BO3-
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8. Acid Base
HF F-
H3BO3 H2BO3-
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8. Acid Base
HF F-
H3BO3 H2BO3-
HCN
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8. Acid Base
HF F-
H3BO3 H2BO3-
HCN CN-
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8. Acid Base
HF F-
H3BO3 H2BO3-
HCN CN-
Put an asterisk next to the strongest acid and base
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8. Acid Base
* HF F-
H3BO3 H2BO3-
HCN CN-
Put an asterisk next to the strongest acid and base
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8. Acid Base
* HF F-
H3BO3 H2BO3-
HCN CN- *
Put an asterisk next to the strongest acid and base
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8. Acid Base
* HF F-
H3BO3 H2BO3-
HCN CN- *
Put an asterisk next to the strongest acid and base
What is the relationship between acid strength and strength of conjugate base?
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8. Acid Base
* HF F-
H3BO3 H2BO3-
HCN CN- *
Put an asterisk next to the strongest acid and base
What is the relationship between acid strength and strength of conjugate base? Inverse
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9. What ions are in H2SO4 solution?
H2SO4
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4-
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
[ OH-]
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
[ OH-]
because it is in water!
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9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
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10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH
H2SO4 + Ba(OH)2
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10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 →
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10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 →
High Solubility
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10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 → BaSO4 + 2HOH
High Solubility
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10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 → BaSO4 + 2HOH
High Solubility
Low Solubility
Lowest Conductivity
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11. What is the best acid for titrating 0.10 M NH3?
0.10 M NaOH 0.10 M HF6.0 M HCl 0.10 M HCl
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11. What is the best acid for titrating 0.10 M NH3?
0.10 M NaOH 0.10 M HF6.0 M HCl 0.10 M HCl
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11. What is the best acid for titrating 0.10 M NH3?
0.10 M NaOH 0.10 M HF6.0 M HCl 0.10 M HCl
Must be strong and about the same molarity!
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12. HCl Molarity pH
1 M
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12. HCl Molarity pH
1 M 0
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12. HCl Molarity pH
1 M 0
0.1M
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12. HCl Molarity pH
1 M 0
0.1M 1
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12. HCl Molarity pH
1 M 0
0.1M 1
0.01M
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12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
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12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M
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12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M 3
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12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M
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12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
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12. HCl Molarity pH
10 M
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
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12. HCl Molarity pH
10 M -1
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
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13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
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13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
Strong
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13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
Strong as pH = -Log[0.00010] = 4.0
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13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
Strong as pH = -Log[0.00010] = 4.0
The pH is not 0 because the acid is 0.00010 M!
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14. Describe the buffer present in human blood.
H2CO3 NaHCO3
15. What is stomach acid?
HCl
16. What is battery acid?
H2SO4