1. Figure: 04-02
Title:
Measuring conductivity.
Caption:
The ability of a solution to conduct electricity depends on the number of ions it contains. (Left) A nonelectrolyte solution does not contain ions, and the bulb does not light. (Middle and right) An electrolyte solution contains ions to serve as charge carriers, causing the bulb to light. If the solution contains a small number of ions, the bulb will be only dimly lit, as in the figure in the middle. If the solution contains a large number of ions, the bulb will be brightly lit, as in the figure on the right.

2. Figure: 04-03
Title:
Dissolution in water.
Caption:
(a) When an ionic compound dissolves in water, H2O molecules separate, surround, and disperse the ions into the liquid. (b) Methanol, CH3OH, a molecular compound, dissolves without forming ions. The methanol molecules can be found by looking for the black spheres, which represent carbon atoms. In both parts (a) and (b), the water molecules have been moved apart so the solute particles can be seen more clearly.

3. Figure: UN
Title:
Sample Exercise 4.1
Caption:
Relating Relative Numbers of Anions and Cations to Chemical Formulas

4. Figure: 04-04
Title:
A precipitation reaction.
Caption:
The addition of a colorless solution of potassium iodide (KI) to a colorless solution of lead nitrate [Pb(NO3) 2] produces a yellow precipitate of lead iodide (PbI2) that slowly settles to the bottom of the beaker.

5. Figure: UN
Title:
Molecular models of three common acids.
Caption:
Hydrochloric acid, nitric acid, and acetic acid.

6. Figure: 04-06
Title:
Hydrogen ion transfer.
Caption:
An H2O molecule acts as a proton donor (acid), and NH3 as a proton acceptor (base). Only a fraction of the NH3 reacts with H2O; NH3 is a weak electrolyte.

7. Figure: UNEX4.5
Title:
Sample Exercise 4.5
Caption:
Comparing Acid Strengths

8. Figure: 04-07
Title:
The acid–base indicator bromthymol blue.
Caption:
The indicator is blue in basic solution and yellow in acidic solution. The left flask shows the indicator in the presence of a base, aqueous ammonia (labeled as ammonium hydroxide). The right flask shows the indicator in the presence of hydrochloric acid, HCl.

9. Figure: 04-08
Title:
Reaction of Mg(OH)2(s) with acid.
Caption:
(a) Milk of magnesia is a suspension of magnesium hydroxide, Mg(OH)2(s), in water. (b) The magnesium hydroxide dissolves upon the addition of hydrochloric acid, HCl(aq). (c) The final clear solution contains soluble MgCl2(aq), shown in Equation 4.15.

10. Figure: 04-09
Title:
Carbonates react with acids to form carbon dioxide gas.
Caption:
Here NaHCO3 (white solid) reacts with hydrochloric acid; the bubbles contain CO2.

11. Figure: 04-12
Title:
Oxidation of calcium metal by molecular oxygen.
Caption:
The oxidation involves transfer of electrons from the metal to O2, eventually leading to formation of CaO.

12. Figure: UN
Title:
Oxidation and reduction.
Caption:
Oxidation is the loss of electrons by a substance; reduction is the gain of electrons by a substance. Oxidation of one substance is always accompanied by reduction of another.

13. Figure: 04-13
Title:
Reaction of magnesium with acid.
Caption:
The bubbles are due to hydrogen gas.

14. Figure: C
Title:
Reaction of copper with silver ion.
Caption:
When copper metal is placed in a solution of silver nitrate, a redox reaction occurs, forming silver metal and a blue solution of copper(II) nitrate.

15. Figure: 04-16
Title:
Procedure for preparation of L of 1.00 M solution of CuSO4.
Caption:
(a) Weigh out mol (39.9 g) of CuSO4 (formula weight = amu). (b) Put the CuSO4 (solute) into a 250-mL volumetric flask, and add a small quantity of water. (c) dissolve the solute by swirling the flask. (d) Add more water until the solution just reaches the calibration mark etched on the neck of the flask. Shake the stoppered flask to ensure complete mixing.

16. Figure: 04-16a
Title:
Procedure for preparation of L of 1.00 M solution of CuSO4.
Caption:
Weigh out mol (39.9 g) of CuSO4 (formula weight = amu).

17. Figure: 04-16b
Title:
Procedure for preparation of L of 1.00 M solution of CuSO4.
Caption:
Put the CuSO4 (solute) into a 250-mL volumetric flask, and add a small quantity of water.

18. Figure: 04-16c
Title:
Procedure for preparation of L of 1.00 M solution of CuSO4.
Caption:
Dissolve the solute by swirling the flask.

19. Figure: 04-16d
Title:
Procedure for preparation of L of 1.00 M solution of CuSO4.
Caption:
Add more water until the solution just reaches the calibration mark etched on the neck of the flask. Shake the stoppered flask to ensure complete mixing.

20. Figure: 04-18
Title:
Procedure for preparing 250 mL of M CuSO4 by dilution of 1.00 M CuSO4.
Caption:
(a) Draw 25.0 mL of the 1.00 M solution into a pipet. (b) Add this to a 250-mL volumetric flask. (c) Add water to dilute the solution to a total volume of 250 mL.

21. Figure: 04-19
Title:
Problem-solving procedure.
Caption:
Outline of the procedure used to solve stoichiometry problems that involve measured (laboratory) units of mass, solution concentration (molarity), or volume.

22. Figure: 04-20
Title:
Change in appearance of a solution containing phenolphthalein indicator as base is added.
Caption:
Before the end point, the solution is colorless (a). As the end point is approached, a pale pink color forms where the base is added (b). At the end point, this pale pink color extends throughout the solution after mixing. As even more base is added, the intensity of the pink color increases (c).

23. Figure: 04-21
Title:
Procedure for titrating an acid against a standardized solution of NaOH.
Caption:
(a) A known quantity of acid is added to a flask. (b) An acid-base indicator is added, and standardized NaOH is added from a buret. (c) The equivalence point is signaled by a color change in the indicator.

24. Figure: UNE04.01
Title:
Exercise 4.1
Caption:
Schematic diagrams of ions in aqueous solution.

25. Figure: UNE04.03
Title:
Exercise 4.3
Caption:
Schematic diagrams of substances in aqueous solution.

26. Figure: UNE04.09
Title:
Exercise 4.9
Caption:
Schematic diagram of a precipitation reaction.

27. Figure: UNE04.10
Title:
Exercise 4.10
Caption:
Three solutions represented schematically.

28. Figure: UNE04.47
Title:
Exercise 4.47
Caption:
Regions of the periodic table.

29. Figure: 04-T01
Title:
Table 4.1
Caption:
Solubility Guidelines for Common Ionic Compounds in Water

30. Figure: 04-T02
Title:
Table 4.2
Caption:
Common Strong Acids and Bases

31. Figure: 04-T03
Title:
Table 4.3
Caption:
Summary of the Electrolytic Behavior of Common Soluble Ionic and Molecular Compounds

32. Figure: 04-T04
Title:
Table 4.4
Caption:
Some Common Antacids

33. Figure: 04-T05
Title:
Table 4.5
Caption:
Activity Series of Metals in Aqueous Solution