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Aqueous solutions & concepts of pH

Aqueous solutions & concepts of pH. Chapter 19-3. I. Ion Product constant - water. A. Acids → hydronium ions (H 3 O+) Bases → hydroxide ions (OH-) Self ionization of water H 2 O + H 2 O  OH - + H 3 O +

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Aqueous solutions & concepts of pH

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

  2. I. Ion Product constant - water A. • Acids→ hydronium ions (H3O+) • Bases → hydroxide ions (OH-) • Self ionization of water • H2O + H2O OH- + H3O+ • Since every ionized water produces one hydronium ion and one hydroxide, the concentration of hydronium and hydroxide in, otherwise, pure water is the same. [H3O+] = 1.0 x 10-7M [OH-] = 1.0 x 10-7M • Kw = [H3O+] [OH-] = 1.0 x 10-14M2

  3. C. Neutral, Acidic, Basic 1. [H3O+] = [OH-] neutral 2. [H3O+] >[OH-] acidic 3. [H3O+] <[OH-] basic Solve practice problem 18, pg. 609

  4. D. Calculating [H3O+] &[OH-] • Kw = [H3O+] [OH-] = 1.0 x 10-14M2 • Calculate [OH-] when have a 1.0 x 10-2M NaOH solution NaOH→ 2. Calculate [H3O+] of a 1.0 x 10-4M H2SO4 solution • H2SO4 → • Determine hydronium and hydroxide ion concentrations in solution that is 1.0 x 10-4M HCl

  5. Calculate hydronium and hydroxide ion concentrations • In a solution that is 1 x 10-4M HCl • In a solutuion that is 1.0 x 10-3 M HNO3 • In a solution that is 1.0 x 10-4M Ca(OH)2

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

  7. A. Calculations with pH Determine the pH of: • 1.0 x 10-3M HCl • 1.0 x 10-2M KOH • 2.0 x 10-2M Sr(OH)2 solution

  8. B. Calculating [H3O+] & [OH-] from pH [H3O+] = 10-pH [OH-] = 10-pOH • pH = 5.0 What is[H3O+] ? • pH = 1.50 Calculate [H3O+] &[OH-] Practice problems pg. 611 19-22

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