1. Chapter 16 pH and Titration

2. I. Concentration Units for Acids and Bases
A. Chemical Equivalents
1. Definition: quantities of solutes that have equivalent combining capacity
a. Acid: mass of one equivalent is numerically equal to the mass of one mole of the acid divided by the number of protons( H3O+ ) that one mole of the acid can provide
Example:
HCl 36 g/mol; 1 eq = 1 H3O+; 36 g/mol H3O+
H2SO4 98g/mol; 2 eq = 2 H3O+; 49 g/mol H3O+

3. b. Base: mass of one equivalent is numerically equal to the mass of one mole of the base divided by the number of protons(OH-) that one mole of the base can provide
Example:
NaOH 40 g/mol; 1 eq = 1 OH-; g/mol OH-
Ca(OH)2 74 g/mol; 2 eq = 2 OH-; g/mol OH-

4. B. Normality
Definition: number of equivalents of solute per liter of solution
N = eq of solute
L of solution

5. C. Relationship Between Normality and Molarity
N = nM
N: Normality
n: number of equivalents (# of H+= or OH-)
M: Molarity
Example:
1M HCl = 1N HCl M NaOH = 1N NaOH
1M H2SO4 = 2N H2SO M Ca(OH)2 = 2N Ca(OH)2

6. II. Aqueous Solutions and the Concept of pH
A. Self-Ionization of Water
1. Definition: Two water molecules interact to produce a hydronium ion and a hydroxide ion by proton transfer - forms a weak electrolyte
2. [ ] is symbol used to indicate concentration in moles per liter (Molarity)

7. 3. H2O + H2O <---> H3O+ + OH- ;
in pure water [H3O+ ] = [OH- ]
4. [H3O+ ][OH- ] = 1 x 10-14
5. If the [H3O+ ] increases then the [OH- ] decreases or
If the [H3O+ ] decreases then the [OH- ] increases

8. Example
What is the hydronium and hydroxide concentration of a 3 x 10-4 M Ca(OH)2 solution?

9. B. The pH scale
1. pH -- the negative of the common logarithm of the hydronium ion concentration
pH = -log[H3O+ ]
2. Acid: pH < 7
3. Base: pH > 7
4. Neutral: pH = 7

10. C. Calculations involving pH
pH = -log[H3O+ ]
0.001 M HCl = [H3O+ ] =1 x 10 -3
pH = -log[1 x 10-3]
pH = 3 (acid)
{Remember that [H3O+ ][OH- ] = 1 x ; so if [H3O+ ] = 1 x 10-3; then [OH- ] = 1 x 10-11
FYI: there is also pOH = - log[OH- ] and
pH + pOH = 14

11. Example:
1. Determine the hydronium concentration, hydroxide concentration of a solution that has a pH of 7.52.

12. III. Acid-Base Titrations
A. Indicators
1. Definitions:
a. indicators - weak acid or base dyes whose colors are sensitive to pH, or hydronium, concentration
b. transition interval - the pH range over which an indicator changes color

13. 2. Types of indicators
a. Change color at about pH 7
b. Change color below pH 7
c. Change color above pH 7

14. B. The Principle of Titration
Definitions:
1. Titration - the controlled addition and measurement of the amount of a solution of known concentration that is required to react completely with a measured amount of a solution of unknown concentration
2.Standard solution - a solution that contains a precisely known concentration of a solute

15. 3. Equivalence point - in a neutralization reaction, the point at which there are equivalent quantities of hydronium and hydroxide ions
4. End point - the point in a titration where an indicator changes color
5. Primary standard - a highly purified compound, when used in solution to check the concentration of the known solution in a titration

16. C. Molarity and Titration
1. Determine the moles of acid (or base) from the standard solution used during titration
2. From a balanced chemical equation, determine the ratio of moles of acid (base) to base (acid)
3. Determine the moles of solute of the unknown solution used during the titration
4. Determine the molarity of the unknown solution

17. D. Examples
1. In a titration of vinegar, you find that it requires mL of 0.748M NaOH to neutralize a 10.0 mL sample of vinegar. What is the concentration of acetic acid in this sample of vinegar?
NaOH + HC2H3O2 →

18. 2. What is the molarity of a magnesium hydroxide solution if 45
2. What is the molarity of a magnesium hydroxide solution if mL of a 0.50M HCl solution is used to titrate 25 mL of magnesium hydroxide?

19. D. Normality and Titrations
Va x Na = Vb x Nb
Va : volume of the acid
Na : normality of the acid
Vb: volume of the base
Nb: normality of the base