acids lesson 2 acid and base properties. properties of acids neutralize bases are electrolytes that...
TRANSCRIPT
AcidsLesson 2
Acid and Base Properties
Properties of Acids
Neutralize bases
Are electrolytes that conduct electricity
React with metals such as Mg and Zn to make H2
Change litmus paper red
Taste sour
Properties of Bases
Neutralize acids
Are electrolytes that conduct electricity
Feel slippery
Change litmus paper blue
Taste bitter
Arrhenius acid (Chemistry 11):
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution.
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11):
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution.
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12):
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor HCl + H2O
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor HCl + H2O H+
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor HCl + H2O H3O
+ + Cl-
H+
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor HCl + H2O H3O
+ + Cl-
Bronsted Base (Chemistry 12): A proton acceptor
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor HCl + H2O H3O
+ + Cl-
Bronsted Base (Chemistry 12): A proton acceptor NH3 + H2O ⇄ H+
Arrhenius acid (Chemistry 11): A substance that produces H+ when in solution. HCl H+ + Cl-
Arrhenius base (Chemistry 11): A substance that produces OH- when in solution. NaOH Na+ + OH-
Bronsted Acid (Chemistry 12): A proton donor HCl + H2O H3O
+ + Cl-
Bronsted Base (Chemistry 12): A proton acceptor NH3 + H2O ⇄ NH4
+ + OH- H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄
base acid
H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
base acid
H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
Base acid
H+ H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
Base acid acid base
H+ H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
Base acid acid base
Conjugate acid base pairs differ by one proton H+
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
Base acid acid base
Conjugate acid base pairs differ by one proton
HCO3- and H2CO3
Complete the Bronsted reaction assuming HCO3- is
a base.
HCO3- + H2O ⇄ H2CO3 + OH-
Base acid acid base
Conjugate acid base pairs differ by one proton
HCO3- and H2CO3 H2O and OH-
Note 1. Arrhenius bases dissociate in water to produce OH-. 2. Bronsted bases accept a proton from water to produce OH-. 3. Arrhenius acids dissociate in water to form H+. 4. Bronsted acids donate a proton to water to form H3O
+. 5. This leads us to the conclusion that H+ is the same as H3O
+.
H+ is another way to show H3O+. We can treat them as
the same. H+ is really just a proton.
H+ + H2O
+
H+ is another way to show H3O+. We can treat them as
the same. H+ is really just a proton.
H+ + H2O
proton water
+
H+ is another way to show H3O+. We can treat them as
the same. H+ is really just a proton.
H3O+
+
H+ is another way to show H3O+. We can treat them as
the same. H+ is really just a proton.
H3O+
This is called the hydronium ion
+
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+ NH3
H2O
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+ NH3
H3O+ H2O H2O
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+ NH3
H3O+ H2O H2O OH-
HCO3
-
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+ NH3
H3O+ H2O H2O OH-
H2CO3 HCO3
-
H2PO4
-
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+ NH3
H3O+ H2O H2O OH-
H2CO3 HCO3
-
H2PO4
- HPO42-
PO4
3-
Conjugate Acid Conjugate Base One more H+ 1 less H+
NH4+ NH3
H3O+ H2O H2O OH-
H2CO3 HCO3
-
H2PO4
- HPO42-
HPO4
2- PO43-
Conjugate Acid Conjugate Base
CH3COOH
Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COO-
Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH
Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O
-
CO32-
Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O
-
HCO3- CO3
2-
HPO4
2-
Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O
-
HCO3- CO3
2-
HPO4
2- PO43-
HO2-
Conjugate Acid Conjugate Base
CH3COOH CH3COO-
C6H5COOH C6H5COO-
C6H5OH C6H5O
-
HCO3- CO3
2-
HPO4
2- PO43-
H2O2 HO2-
Strong Acids There are six on the top of the Acid Chart- p6.All completely ionize in water.All are very good conductors.All produce lots of H3O
+.All have very large Ka. Use a “” and not “⇄” HCl + H2O
Strong Acids There are six on the top of the Acid Chart- p6.All completely ionize in water.All are very good conductors.All produce lots of H3O
+.All have very large Ka. Use a “” and not “⇄” HCl + H2O H3O
+ + Cl-
Weak Acids Left side of the Acid Chart below the top six. Partially ionize in water.Are poor conductors.Produce small amounts of H3O
+.Have small Ka’s. Use a “⇄” and not “”
HF + H2O
Weak Acids Left side of the Acid Chart below the top six. Do not completely ionize in water.Are poor conductors.Produce small amounts of H3O
+.Have small Ka’s. Use a “⇄” and not “”
HF + H2O ⇄ H3O+ + F-
Weak Acids Left side of the Acid Chart below the top six. Do not completely ionize in water.Are poor conductors.Produce small amounts of H3O
+.Have small Ka’s. Use a “⇄” and not “”
HF + H2O ⇄ H3O+ + F-
Ka = [H3O
+][F-]= 3.5 x 10-4 from
page 6 [HF]
Water is not included because it is a pure liquid!Its concentration is constant!
You can also write: HF ⇌ H+ + F-
Ka = [H+][F-]
= 3.5 x 10-4
[HF]
Writing Ionic Equations: Formula, Complete, and Net.
HCl + NaOH NaCl + H2O(l)
H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O(l)
H+ + OH- H2O(l)
Do not break up weak acids or bases!
HF + KOH KF + H2O(l)
HF + K+ + OH- K+ + F- + H2O(l)
HF + OH- F- + H2O(l)