1 / 8

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 +

galvin
Télécharger la présentation

Aqueous solutions & concepts of pH

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related