Acids Lesson 1 Acid and Base Properties

Properties of Acids Neutralize bases Are electrolytes that conduct electricity Change litmus paper red Taste sour React with metals such as Mg and Zn to make H2

Properties of Bases Are electrolytes that conduct electricity Neutralize acids Change litmus paper blue Feel slippery Taste bitter

Arrhenius acid Chemistry 11 produces H+ in solution HCl  H+ + Cl- Arrhenius base Chemistry 11 produces OH- in solution NaOH  Na+ + OH-

Bronsted Acid Chemistry 12 A proton donor H+ HCl + H2O  H3O+ + Cl- strong Bronsted Base Chemistry 12 A proton acceptor NH3 + H2O ⇄ NH4+ + OH- H+ weak

Write a Bronsted reaction for the base HCO3- weak H+ H+ HCO3- + H2O ⇄ H2CO3 + OH- base acid acid base HCO3- and H2CO3 H2O and OH- Conjugate acid base pairs differ by one proton H+

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. H+ is the same as H3O+

H+ is another way to show H3O+. H+ + H2O ⇋ H3O+ Hydronium ion + H+ H2O

Conjugate Acid Conjugate Base One more H+ 1 less H+ C6H5OH C6H5O- H2CO3 HCO3- H2O OH- HPO42- PO43- H2PO4- HPO42- C6H5COOH C6H5COO- NH4+ NH3 Fe(H2O)63+ Fe(H2O)5(OH)2+ Look on page 6

Strong Acids Weak Acids

Strong Acids Left side Acid Chart top six Completely ionize in water Are good conductors. Produce large amounts of H3O+. Have very large Ka’s. Use a “” and not “⇄” HCl + H2O  H3O+ + Cl-

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 is a weak acid HF + KOH  KF + H2O(l) HF + K+ + OH-  K+ + F- + H2O(l) HF + OH-  F- + H2O(l)