1. Aqueous solutions & concepts of pH Chapter 19-3

2. I. Ion Product constant - water A.  Acids→ hydronium ions (H 3 O+)  Bases → hydroxide ions (OH-) B.Self ionization of water H 2 O + H 2 O  OH - + H 3 O +   Since every ionized water produces one hydronium ion and one hydroxide, the concentration of hydronium and hydroxide in, otherwise, pure water is the same. [H 3 O + ] = 1.0 x 10 -7 M [OH - ] = 1.0 x 10 -7 M Kw = [H 3 O + ] [OH - ] = 1.0 x 10 -14 M 2

3. C. Neutral, Acidic, Basic 1. 1. [H 3 O + ] = [OH - ] neutral 2. [H 3 O + ] >[OH - ] acidic 3. [H 3 O + ] <[OH - ] basic Solve practice problem 18, pg. 609

4. D. Calculating D. Calculating [H 3 O + ] &[OH - ] Kw = [H 3 O + ] [OH - ] = 1.0 x 10 -14 M 2 1. 1.Calculate [OH - ] when have a 1.0 x 10 -2 M NaOH solution NaOH → 2. Calculate [H 3 O + ] of a 1.0 x 10 -4 M H 2 SO 4 solution H 2 SO 4 → 3. 3.Determine hydronium and hydroxide ion concentrations in solution that is 1.0 x 10 -4 M HCl

5. Calculate hydronium and hydroxide ion concentrations 1.In a solution that is 1 x 10 -4 M HCl 2.In a solutuion that is 1.0 x 10 -3 M HNO 3 3.In a solution that is 1.0 x 10 -4 M Ca(OH) 2

6. II. pH Scale  pH = -log  pH = -log [H + ]   pOH = -log [OH - ]   pH + pOH = 14

7. A. Calculations with pH Determine the pH of: 1.1.0 x 10 -3 M HCl 2.1.0 x 10 -2 M KOH 3.2.0 x 10 -2 M Sr(OH) 2 solution

8. B. Calculating B. Calculating [H 3 O + ] & [OH-] from pH [H 3 O + ] = 10 -pH [OH-] = 10 -pOH 4. 4.pH = 5.0 What is [H 3 O + ] ? 5. 5.pH = 1.50 Calculate [H 3 O + ] &[OH-] Practice problems pg. 611 19-22