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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 Presentation
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AcidsLesson 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
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH → NaCl + HOH
Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH → NaCl + HOH
HCl + HCO3-
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-
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.
2. H3BO3
2. H3BO3 triprotic
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
2. H3BO3 triprotic H3BO3 ⇌ H+ + H2BO3-
H2CO3 diprotic H2CO3 ⇌ H+ + HCO3
-
HCl monoprotic HCl → H+ + Cl-
Only lose one proton when in water!However,
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
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
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 →
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
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?
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?
3. Which determines acid strength?
Molarity
pH =
Ka
3. Which determines acid strength?
Molarity is concentration.
pH =
Ka
3. Which determines acid strength?
Molarity is concentration.
pH = -Log[H+]
Ka
3. Which determines acid strength?
Molarity is concentration.
pH = -Log[H+]
Ka is strength as indicated in the acid chart
4. Which determines the pH.
Ka
Molarity
Temperature
4. Which determines the pH = -Log[H+]
Ka
Molarity
Temperature
4. Which determines the pH = -Log[H+]
Ka determines the [H+] and the pH
Molarity
Temperature
4. Which determines the pH = -Log[H+]
Ka determines the [H+] and the pH
Molarity determines the [H+] and the pH
Temperature
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
5. Pick the best conductor.
1 M NaOH 0.1 M HCl 0.01 M KOH
5. Pick the best conductor.
1 M NaOH 0.1 M HCl 0.01 M KOH
All strong- highest Molarity!
6. Pick the worst conductor.
NaOH HCl NaCN NH3
6. Pick the worst conductor.
NaOH HCl NaCN NH3
6. Pick the worst conductor.
NaOH HCl NaCN NH3
Good Conductors are…..
Strong acids
Strong Bases
Soluble Salts
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]
8. Acid Base
HF
8. Acid Base
HF F-
8. Acid Base
HF F-
H2BO3-
8. Acid Base
HF F-
H3BO3 H2BO3-
8. Acid Base
HF F-
H3BO3 H2BO3-
HCN
8. Acid Base
HF F-
H3BO3 H2BO3-
HCN CN-
8. Acid Base
HF F-
H3BO3 H2BO3-
HCN CN-
Put an asterisk next to the strongest acid and base
8. Acid Base
* HF F-
H3BO3 H2BO3-
HCN CN-
Put an asterisk next to the strongest acid and base
8. Acid Base
* HF F-
H3BO3 H2BO3-
HCN CN- *
Put an asterisk next to the strongest acid and base
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?
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
9. What ions are in H2SO4 solution?
H2SO4
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4-
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
[ OH-]
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
[ OH-]
because it is in water!
9. What ions are in H2SO4 solution?
H2SO4 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH
H2SO4 + Ba(OH)2
10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 →
10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 →
High Solubility
10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH → NaCl + HOH
H2SO4 + Ba(OH)2 → BaSO4 + 2HOH
High Solubility
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
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
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
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!
12. HCl Molarity pH
1 M
12. HCl Molarity pH
1 M 0
12. HCl Molarity pH
1 M 0
0.1M
12. HCl Molarity pH
1 M 0
0.1M 1
12. HCl Molarity pH
1 M 0
0.1M 1
0.01M
12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M
12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M 3
12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M
12. HCl Molarity pH
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
12. HCl Molarity pH
10 M
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
12. HCl Molarity pH
10 M -1
1 M 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
Strong
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
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!
14. Describe the buffer present in human blood.
H2CO3 NaHCO3
15. What is stomach acid?
HCl
16. What is battery acid?
H2SO4