acids lesson 20 subtle items
DESCRIPTION
Acids Lesson 20 Subtle Items. Subtle Acid Items 1. Weak bases neutralize a strong acid as well as a strong base would. HCl + NaOH HCl +HCO 3 -. →NaCl +HOH. →H 2 CO 3 +Cl -. Both reactions go to completion because of the strong acid. 2. H 3 BO 3 H 2 CO 3 HCl . - PowerPoint PPT PresentationTRANSCRIPT
AcidsLesson 20
Subtle Items
Subtle Acid Items
1. Weak bases neutralize a strong acid as well as a strong base would.
HCl + NaOH
HCl + HCO3
-
→ NaCl + HOH
→ H2CO3 + Cl-
Both reactions go to completion because of the strong acid.
2. H3BO3
H2CO3
HCl
triprotic H3BO3 ⇌ H+ + H2BO3-
diprotic H2CO3 ⇌ H+ + HCO3-
monoprotic HCl → H+ + Cl-
Only lose one proton when in water!
Which neutralizes more NaOH? H3BO3 or HCl?
H3BO3 + 3NaOH → Na3BO3 + 3HOH
HCl + 1NaOH → NaCl + HOH
3. Which determines acid strength?
Molarity
Ka is strength as indicated in the acid chart
is concentration
4. Which determines the pH
= -Log[H+]
determines the [H+]
determines the [H+]
affects the Ka
Ka
Molarity
Temperature
5. Pick the best conductor.
1 M NaCN 0.1 M HCl 0.1 M KOH
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?BufferWrite an equation for the equilibrium.H2CO3 ⇋ H+ + HCO3
-
Label each chemical species with a concentration. 2 M Low 2 MWhat limits the ability to buffer against acid?[HCO3
-]What limits the ability to buffer against base?[H2CO3]
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 → H+ + HSO4
-
HSO4- ⇌ H+ + SO4
2-
[ OH-]
because it is in water!
BaSO4(s) + 2HOH
10. Which titration will have the equivalence point with lowest conductivity?
HCl + NaOH →
H2SO4 + Ba(OH)2 →
NaCl(aq) + HOH
High Solubility
Low Solubility
Lowest Conductivity
11. What is the best acid for titrating 0.10 M NH3?
0.00010 M HCl 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 0
0.1M 1
0.01M 2
0.001M 3
0.0001M 4
10 M -1
13.A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak?
Strong pH = -Log[0.00010] = 4.0
The pH is only at 1.0 M!
14.A 0.0010 M acid has a pH of 4.0. Is the acid strong or weak?
Weak pH = -Log[0.0010] = 3.0
The pH is only at 1.0 M!
15. HInd ⇌ H+ + Ind-
It’s yellow in HCl and red in HCN
Assign each colour
Which is the stronger acid; HInd or HCN?
HCN + Ind- ⇌ HInd + CN-
What is favoured?
Reactants
yellow red
16. Describe the buffer present in human blood.
H2CO3 NaHCO3
17. What is stomach acid?
HCl
18 . What is battery acid?
H2SO4
pH
Volume 1.0 M NH3 added
14
7
00 30 60
19. Match the Curve with the Reaction
A. 3HCl + Al(OH)3 → AlCl3 + 3HOHB. HCl + KOH → KCl + HOHC. HCN + KOH → KCN + HOH
pH
Volume 1.0 M NH3 added
14
7
00 30 60
A. 3HCl + Al(OH)3 → AlCl3 + 3HOHB. HCl + KOH → KCl + HOHC. HCN + KOH → KCN + HOH
20. Match the Curve with the Reaction
21. Write a reaction between NaHCO3 and NaHC2O4
HCO3- + HC2O4
- H2CO3 + C2O42- ⇌
Are the reactants or products favoured?
products
0.10 M Weak Acid
x2
Ka0.10
0.10 M Weak Base
x2
Kb0.10
Kw
Ka== =