figure 4.1 the electrical conductivity of ionic solutions · figure 4.1 the electrical conductivity...

Figure 4.1 The electrical conductivity of ionic solutions

Figure 4.2 Electron distribution in molecules of H2 and H2O

Figure 4.3 The dissolution of an ionic compound

Table 4.1 Solubility Rules For Ionic Compounds in Water

1. All common compounds of Group 1A(1) ions (Li+, Na+, K+, etc.) and ammonium

ion (NH4+) are soluble.

2. All common nitrates (NO3-), acetates (CH3COO- or C2H3O2

-) and most

perchlorates (ClO4-) are soluble.

3. All common chlorides (Cl-), bromides (Br-) and iodides (I-) are soluble, except

those of Ag+, Pb2+, Cu+, and Hg22+.

1. All common metal hydroxides are insoluble, except those of Group 1A(1)

and the larger members of Group 2A(2)(beginning with Ca2+).

2. All common carbonates (CO32-) and phosphates (PO4

3-) are insoluble,

except those of Group 1A(1) and NH4+.

3. All common sulfides are insoluble except those of Group 1A(1), Group

2A(2) and NH4+.

Soluble Ionic Compounds

Insoluble Ionic Compounds

4. All common sulfates (SO42-)are soluble, except those of Ca2+, Sr2+, Ba2+, Ag+ and

Pb2+

Copper(II) Bromide and Potassium Hydroxide

CuBr2 + KOH Cu(OH)2 + KBr

2+ 1- 1+ 1-

2 2 Molecular Equation

(aq) (aq) (aq) (s)

Complete Ionic Equation

Cu2+ + 2Br- + 2K+ + 2OH- Cu(OH)2 + 2K+ + 2Br-

(aq) (aq) (aq) (aq)

(aq) (aq) (s)

Net Ionic Equation

Cu2+ + 2OH- Cu(OH)2

(aq) (aq) (s)

• Acids and Corresponding Anions

• Oxoacids contain hydrogen, oxygen, and a third central atom.

• To name an acid from its anion name:

1. Change an –ate suffix to –ic.

2. Change an –ite suffix to –ous.

3. Add the word “acid.””

• For example:

HNO3 nitric acid

H2SO4 sulfuric acid

sulfuric

acid

H2SO4 sulfate ion SO4

2-

sulfurous

acid

H2SO3 sulfite ion SO3

2-

phosphoric

acid H3PO4

phosphate ion PO43-

nitric acid HNO3 nitrate ion NO3

-

nitrous

acid

HNO2 nitrite ion NO2-

carbonic

acid

H2CO3 carbonate

ion

CO32-

Oxoacid Oxoanion

Table 4.2 Selected Acids and Bases

Acids

Strong

hydrochloric acid, HCl

hydrobromic acid, HBr

hydroiodic acid, HI

nitric acid, HNO3

sulfuric acid, H2SO4

perchloric acid, HClO4

Weak

hydrofluoric acid, HF

phosphoric acid, H3PO4

acetic acid, CH3COOH (or

HC2H3O2)

Bases

Strong

Weak

sodium hydroxide, NaOH

calcium hydroxide, Ca(OH)2

potassium hydroxide, KOH

strontium hydroxide, Sr(OH)2

barium hydroxide, Ba(OH)2

ammonia, NH3

Figure 4.4 The hydrated proton

Figure 18.3

Strong acid: HA(g or l) + H2O(l) H3O+(aq) + A-(aq)

The extent of dissociation for strong and weak acids

Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Figure 18.3 The extent of dissociation for strong and weak acids

Weak acid: HA(aq) + H2O(l) H2O+(aq) + A-(aq)

(continued)

Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Polyprotic Acids

H3PO4(aq) + NaOH(aq) NaH2PO4(aq) + H2O(l)

NaH2PO4(aq) + NaOH(aq) Na2HPO4(aq) + H2O(l)

Na2HPO4(aq) + NaOH(aq) Na3PO4(aq) + H2O(l)

H3PO4 = triprotic

H3PO4(aq) + Na+(aq) + OH-

(aq) Na+

(aq) + H2PO4-(aq) + H2O(l)

Complete Ionic Equation

Weak acid Strong Base

2 More Protons from Phosphoric Acid:

H3PO4(aq) + 3NaOH(aq) Na3PO4(aq) + 3H2O(l)

Citric Acid: C6H8O7 or H3C6H5O7

Sodium Bicarbonate: NaHCO3

H3C6H5O7 (s) + 3NaHCO3(s) H2O

Na3C6H5O7(aq) + 3CO2(g) + H2O(l)