1. Chlorine compounds in the water of a swimming pool prevent the growth of bacteria. The concentration of hydronium ions in solution must be carefully controlled so that the right compounds of chlorine will be present. Sodium bicarbonate can be used to lower the concentration of hydronium ions in solution.

2. The pH Scale
How is pH used to describe the concentration of acids and bases?

3. The pH Scale
The pH of a solution is a measure of its hydronium ion concentration
The lower the pH value, the greater the H3O+ ion concentration in solution is.
The higher the pH value, the lower the H3O+ ion concentration is.

4. The pH Scale
Chemists use the pH scale–a number scale from 0 to 14–to describe the concentration of hydronium ions in a solution.
A pH of 7 indicates a neutral solution.
Acids have a pH less than 7.
Bases have a pH greater than 7.

5. The pH Scale
The pH scale classifies solutions as acids or bases.

6. The pH Scale
Pure water ionizes slightly according to the following reaction.
The arrow pointing to the left is longer than the arrow pointing to the right to show that water contains more molecules than ions.

7. The pH Scale
Water is neutral because it contains small but equal concentrations of hydronium ions and hydroxide ions.
At 25°C, the concentration of both H3O+ and OH– in water is 1.0 × 10–7 M.
Pure water has a pH of 7.

8. The pH Scale
Adding an acid to water increases the concentration of H3O+ and decreases the concentration of OH–.
A hydrochloric acid solution in which the concentration of H3O+ is 0.10 M (or 1.0 × 10–1 M) has a pH of 1.

9. The pH Scale
Adding a base to water increases the concentration of OH– and decreases the concentration of H3O+.
A sodium hydroxide solution in which the concentration of OH– is 0.10 M has a concentration of H3O+ of 1.0 × 10–13 M. This solution has a pH of 13.

10. Strong Acids and Bases
How do strong acids and bases differ from weak acids and bases?
When strong acids dissolve in water, they ionize almost completely.
Strong bases dissociate almost completely in water.

11. Strong Acids and Bases
Some reactions go to completion, while others reach equilibrium.
When certain acids and bases dissolve in water, the formation of ions from the solute almost goes to completion.
Such acids and bases are classified as strong.

12. Strong Acids and Bases
Strong Acids
When hydrogen chloride dissolves in water, there are about the same number of hydronium ions in solution as there were molecules of HCl to begin with.
HCl is an example of a strong acid. Other strong acids include sulfuric acid, H2SO4, and nitric acid, HNO3.

13. Strong Acids and Bases
Strong Bases
When dissolved in water, sodium hydroxide almost completely dissociates into sodium and hydroxide ions.
Sodium hydroxide is an example of a strong base. Other strong bases include calcium hydroxide, Ca(OH)2, and potassium hydroxide, KOH.

14. Weak Acids and Bases
How do strong acids and bases differ from weak acids and bases?
Weak acids and bases ionize or dissociate only slightly in water.

15. Weak Acids and Bases
Weak Acids
A solution of acetic acid, CH3COOH, and water can be described by the following equation.
The equilibrium favors the reactants over the products, so few ions form in solution.

16. Weak Acids and Bases
A weak acid forms fewer hydronium ions than a strong acid of the same concentration, so a weak acid has a higher pH than a strong acid of the same concentration.
Concentration is the amount of solute dissolved in a given amount of solution.
Strength refers to the solute’s tendency to form ions in water.
Concentration and strength both affect pH.

17. Weak Acids and Bases
Weak Bases
Ammonia, NH3, is a colorless gas with a distinctive smell. When it dissolves in water, very little of it ionizes.
Equilibrium favors the reactants, so few NH4+ and OH– ions are produced.

18. Weak Acids and Bases
Buffers
Weak acids and bases can be used to make buffers.
A buffer is a solution that is resistant to large changes in pH.
Buffers can be prepared by mixing a weak acid and its salt or a weak base and its salt.

19. Electrolytes
Why are strong acids and bases good electrolytes?
An electrolyte is a substance that ionizes or dissociates into ions when it dissolves in water.
Strong acids and bases are strong electrolytes because they dissociate or ionize almost completely in water.

20. Electrolytes
Sports drinks contain salts of elements such as sodium, potassium, and calcium. The electrolytes in sports drinks help restore the balance of ions in your body.

21. Electrolytes can be classified as strong or weak.
Sodium hydroxide is a strong electrolyte that produces many ions in water.
Salts are also strong electrolytes.
Acetic acid is a weak electrolyte because it only partially ionizes.

22. Assessment Questions
Which pH value indicates the solution with the lowest concentration of hydronium ions?
pH 1
pH 7
pH 10
pH 14

23. Assessment Questions
Which pH value indicates the solution with the lowest concentration of hydronium ions?
pH 1
pH 7
pH 10
pH 14 ANS: D

24. Assessment Questions
Which substance forms a strong base solution when it is dissolved in water?
NaCl
HCl
H2CO3
Ca(OH)2

25. Assessment Questions
Which substance forms a strong base solution when it is dissolved in water?
NaCl
HCl
H2CO3
Ca(OH)2
ANS: D

26. Assessment Questions
Which combination of solutes will form a solution that is resistant to pH changes?
weak acid and water
weak acid and strong base
weak acid and its salt
strong acid and its salt

27. Assessment Questions
Which combination of solutes will form a solution that is resistant to pH changes?
weak acid and water
weak acid and strong base
weak acid and its salt
strong acid and its salt ANS: C

28. Assessment Questions
Acetic acid and sodium carbonate are examples of strong electrolytes. True False

29. Assessment Questions
Acetic acid and sodium carbonate are examples of strong electrolytes. True False
ANS: F, weak