Acids Lesson 1 Acid and Base Properties. Taste sour Change litmus paper red React with metals such as Mg and Zn to make H 2 Are electrolytes that conduct.

AcidsLesson 1

Acid and Base Properties

Taste sour

Change litmus paper red

React with metals such as Mg and Zn to make H2

Are electrolytes that conduct electricity

Neutralize bases

Properties of Acids

Taste bitter

Change litmus paper blue

Feel slippery

Are electrolytes that conduct electricity

Neutralize acids

Properties of Bases

Arrhenius acid

HCl

Arrhenius base

NaOH Na+ + OH-

H+ + Cl-

produces H+ in solutionChemistry 11

produces OH- in solutionChemistry 11

H+

Bronsted Acid

H+

HCl + H2O

Bronsted Base

NH3 + H2O ⇄

A proton donor

A proton acceptor

Chemistry 12

Chemistry 12

H3O+ + Cl-

NH4+ + OH-

weak

strong

H+H+

Write a Bronsted reaction for the base HCO3-

base acid acid base

HCO3- ⇄ H2CO3 + OH- + H2O

weak

Conjugate acid base pairs differ by one proton H+

HCO3- and H2CO3 H2O and OH-

5. H+ is the same as H3O+

4. Bronsted acids donate a proton to water to form H3O+

3. Arrhenius acids dissociate in water to form H+

2. Bronsted bases accept a proton from water to produce OH-

1. Arrhenius bases dissociate in water to produce OH-

Note

H+ is another way to show H3O+.

Hydronium ion

H3O+H+ + H2O ⇋

+

H+

H2O

NH4+ NH3

Fe(H2O)63+

OH-

HCO3-

HPO42-

PO43- HPO4

2-

H2PO4-

H2CO3

H2O

One more H+ 1 less H+

Conjugate BaseConjugate Acid

C6H5COOH C6H5COO-

C6H5OH C6H5O-

Fe(H2O)5(OH)2+ Look on page 6

Strong Acids

Weak Acids

HCl + H2O H3O+ + Cl-

Use a “” and not “⇄”

Have very large Ka’s.

Produce large amounts of H3O+.

Are good conductors.

Completely ionize in water

Left side Acid Chart top six

Strong Acids

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 H⇄ 3O+ + 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]

HF + OH- F- + H2O(l)

HF + K+ + OH- K+ + F- + H2O(l)

HF + KOH KF + H2O(l)

Do not break up weak acids or bases!

H+ + OH- H2O(l)

H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O(l)

HCl + NaOH NaCl + H2O(l)

Writing Ionic Equations: Formula, Complete, and Net.

HF is a weak acid