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Acids Lesson 14 Amphiprotic Ions Acids or Bases?. Amphiprotic Ions H 3 PO 4 Acid H 2 PO 4 - Amphiprotic HPO 4 2- Amphiprotic PO 4 3- Base Amphiprotic ions have a Ka and a Kb . If the Ka > Kb , then the ion is an acid . If the Kb > Ka , then the ion is a base. - PowerPoint PPT Presentation
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AcidsLesson 14
AmphiproticIons
Acids or Bases?
Kwantlen Science Challenge:
Kwantlen Science Challenge:
Kwantlen Science Challenge:
Amphiprotic Ions H3PO4 AcidH2PO4
- AmphiproticHPO4
2- AmphiproticPO4
3- Base Amphiprotic ions have a Ka and a Kb.
If the Ka > Kb, then the ion is an acid in water.
If the Kb > Ka, then the ion is a basein water.
Is H2PO4- acid or basic
acid
1. Is H2PO4- an acid or base when in water? Write the predominate hydrolysis
equation for this ion.
Ka (H2PO4-) = 6.2 x 10-8
Kb (H2PO4-) = Kw
Ka(H3PO4)
= 1 x 10-14
7.5 x 10-3
= 1.3 x 10-12
Ka > Kb Acid
H2PO4- + H2O ⇄
HPO42- + H3O+
Is HPO42- acid or basic
basic
2. Is HPO42- an acid or base when in water? Write the hydrolysis equation for this
ion.
Ka (HPO42-) = 2.2 x 10-13
Kb (HPO4
2-) = KwKa(H2PO4
-)
= 1 x 10-14
6.2 x 10-8
= 1.6 x 10-7
Kb > Ka base
HPO42- + H2O ⇄
H2PO4- + OH-
3. Show by calculation if NH4F is an acid or base when in water.
NH4F → NH4+ + F-
acid baseBoth have weak parents- neither will cross off!What will the salt be?
Ka(NH4+) = 5.6 x 10-10
Kb (F-) = = KwKa(HF)
= 1 x 10-14
3.5 x 10-4
= 2.9 x 10-11
Ka > Kb acid
4. Show by calculation if NH4CH3COO is an acid or base when in water.
NH4CH3COO → NH4+ + CH3COO-
acid base
Ka(NH4+) = 5.6 x 10-10
Kb (CH3COO-) = = KwKa(CH3COOH)
= 1 x 10-14
1.8 x 10-5
= 5.6 x 10-10
Ka = Kb neutral pH = 7.00
5. Calculate the volume of 0.100 M H2CO3 required to neutralize 25.0 mL of 0.200 M KOH.
1H2CO3 + 2KOH → K2CO3 + 2HOH? L 0.0250 L0.100 M 0.200 M
5. Calculate the volume of 0.100 M H2CO3 required to neutralize 25.0 mL of 0.200 M KOH.
1H2CO3 + 2KOH → K2CO3 + 2HOH? L 0.0250 L0.100 M 0.200 M
0.0250 L KOH
5. Calculate the volume of 0.100 M H2CO3 required to neutralize 25.0 mL of 0.200 M KOH.
1H2CO3 + 2KOH → K2CO3 + 2HOH? L 0.0250 L0.100 M 0.200 M
0.0250 L KOH x 0.200 mol L
5. Calculate the volume of 0.100 M H2CO3 required to neutralize 25.0 mL of 0.200 M KOH.
1H2CO3 + 2KOH → K2CO3 + 2HOH? L 0.0250 L0.100 M 0.200 M
0.0250 L KOH x 0.200 mol x 1 mole H2CO3 L 2 mole KOH
5. Calculate the volume of 0.100 M H2CO3 required to neutralize 25.0 mL of 0.200 M KOH.
1H2CO3 + 2KOH → K2CO3 + 2HOH? L 0.0250 L0.100 M 0.200 M
0.0250 L KOH x 0.200 mol x 1 mole H2CO3 x 1 L L 2 mole KOH 0.100 mol
5. Calculate the volume of 0.100 M H2CO3 required to neutralize 25.0 mL of 0.200 M KOH.
1H2CO3 + 2KOH → K2CO3 + 2HOH? L 0.0250 L0.100 M 0.200 M
0.0250 L KOH x 0.200 mol x 1 mole H2CO3 x 1 L = 0.0250 L L 2 mole KOH 0.100 mol
6. Label the equation that has a Ka, Kb, Ksp, Kw, or Keq.
Mg(OH)2(s) ⇌ Mg2+ + 2OH-
CN- + H2O ⇌ HCN + OH-
NH4+ + H2O ⇌ H3O+ + NH3
N2O4(g) ⇌ 2NO2(g)
2H2O ⇌ H3O+ + OH-
6. Label the equation that has a Ka, Kb, Ksp, Kw, or Keq.
Ksp Mg(OH)2(s) ⇌ Mg2+ + 2OH-
CN- + H2O ⇌ HCN + OH-
NH4+ + H2O ⇌ H3O+ + NH3
N2O4(g) ⇌ 2NO2(g)
2H2O ⇌ H3O+ + OH-
6. Label the equation that has a Ka, Kb, Ksp, Kw, or Keq.
Ksp Mg(OH)2(s) ⇌ Mg2+ + 2OH-
Kb CN- + H2O ⇌ HCN + OH-
NH4+ + H2O ⇌ H3O+ + NH3
N2O4(g) ⇌ 2NO2(g)
2H2O ⇌ H3O+ + OH-
6. Label the equation that has a Ka, Kb, Ksp, Kw, or Keq.
Ksp Mg(OH)2(s) ⇌ Mg2+ + 2OH-
Kb CN- + H2O ⇌ HCN + OH-
Ka NH4+ + H2O ⇌ H3O+ + NH3
N2O4(g) ⇌ 2NO2(g)
2H2O ⇌ H3O+ + OH-
6. Label the equation that has a Ka, Kb, Ksp, Kw, or Keq.
Ksp Mg(OH)2(s) ⇌ Mg2+ + 2OH-
Kb CN- + H2O ⇌ HCN + OH-
Ka NH4+ + H2O ⇌ H3O+ + NH3
Keq N2O4(g) ⇌ 2NO2(g)
2H2O ⇌ H3O+ + OH-
6. Label the equation that has a Ka, Kb, Ksp, Kw, or Keq.
Ksp Mg(OH)2(s) ⇌ Mg2+ + 2OH-
Kb CN- + H2O ⇌ HCN + OH-
Ka NH4+ + H2O ⇌ H3O+ + NH3
Keq N2O4(g) ⇌ 2NO2(g)
Kw 2H2O ⇌ H3O+ + OH-