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Aqueous solutions & concepts of pH Chapter 19-3. I. Ion Product constant - water A.  Acids→ hydronium ions (H 3 O+)  Bases → hydroxide ions (OH-) B.Self.

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Presentation on theme: "Aqueous solutions & concepts of pH Chapter 19-3. I. Ion Product constant - water A.  Acids→ hydronium ions (H 3 O+)  Bases → hydroxide ions (OH-) B.Self."— Presentation transcript:

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 M [OH - ] = 1.0 x M Kw = [H 3 O + ] [OH - ] = 1.0 x M 2

3 C. Neutral, Acidic, Basic [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 M Calculate [OH - ] when have a 1.0 x M NaOH solution NaOH → 2. Calculate [H 3 O + ] of a 1.0 x 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 M HCl

5 Calculate hydronium and hydroxide ion concentrations 1.In a solution that is 1 x M HCl 2.In a solutuion that is 1.0 x M HNO 3 3.In a solution that is 1.0 x 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: x M HCl x M KOH x 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


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