Acids Lesson 22 Subtle Items

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



HCl + HCO3-

Subtle Acid Items



HCl + HCO3

- → H2CO3 + Cl-

Subtle Acid Items



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-


H2CO3


H2CO3 diprotic


H2CO3 diprotic H2CO3 ⇌ H+ + HCO3

-



-

HCl



-

HCl monoprotic



-

HCl monoprotic HCl → H+ + Cl-



-


Only lose one proton when in water!However,



-


Only lose one proton when in water!However,

H3BO3 + NaOH



-


Only lose one proton when in water!However, loses all three because of the strong base!

H3BO3 + 3NaOH → Na3BO3 + 3HOH



-




HCl + NaOH →



-







-





Which neutralizes more NaOH, H3BO3 or HCl?



-




HCl + 1NaOH→ NaCl + HOH

Which neutralizes more NaOH? H3BO3 or HCl?

3. Which determines acid strength?

Molarity

pH =

Ka


Molarity is concentration.

pH =

Ka



pH = -Log[H+]

Ka



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


Ka determines the [H+] and the pH

Molarity

Temperature



Molarity determines the [H+] and the pH

Temperature



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

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-


8. Acid Base

* HF F-

H3BO3 H2BO3-

HCN CN- *


8. Acid Base

* HF F-

H3BO3 H2BO3-

HCN CN- *


What is the relationship between acid strength and strength of conjugate base?

8. Acid Base

* HF F-

H3BO3 H2BO3-

HCN CN- *


What is the relationship between acid strength and strength of conjugate base? Inverse

9. What ions are in H2SO4 solution?

H2SO4


H2SO4 → H+ + HSO4

-


H2SO4 → H+ + HSO4

-

HSO4-


H2SO4 → H+ + HSO4

-

HSO4- ⇌ H+ + SO4

2-


H2SO4 → H+ + HSO4

-

HSO4- ⇌ H+ + SO4

2-

[ OH-]


H2SO4 → H+ + HSO4

-

HSO4- ⇌ H+ + SO4

2-

[ OH-]

because it is in water!


H2SO4 → H+ + HSO4

-

HSO4- ⇌ H+ + SO4

2-

10. Which titration will have the equivalence point with lowest conductivity?

HCl + NaOH

H2SO4 + Ba(OH)2



H2SO4 + Ba(OH)2 →



H2SO4 + Ba(OH)2 →

High Solubility



H2SO4 + Ba(OH)2 → BaSO4 + 2HOH

High Solubility



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

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?


Strong


Strong as pH = -Log[0.00010] = 4.0


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

Acids Lesson 22 Subtle Items

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