Acids Lesson 2 Acid and Base Properties.

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Presentation transcript:

Acids Lesson 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 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 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 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 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 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- PO43-

Conjugate Acid Conjugate Base One more H+ 1 less H+ NH4+ NH3 H3O+ H2O H2O OH- H2CO3 HCO3- H2PO4- HPO42- HPO42- 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- CO32- HPO42-

Conjugate Acid Conjugate Base CH3COOH CH3COO- C6H5COOH C6H5COO- C6H5OH C6H5O- HCO3- CO32- HPO42- PO43- HO2-

Conjugate Acid Conjugate Base CH3COOH CH3COO- C6H5COOH C6H5COO- C6H5OH C6H5O- HCO3- CO32- HPO42- 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)