1 / 8

20.1

20.1. Hydrogen Ions and Acidity. Section 20.2. Self-ionization - the reaction in which two water molecules produce ions. H 2 O  H + + OH - Water Hydrogen ion hydroxide ion. H 2 O + H 2 O  H 3 0 + + OH -

cameron-graham
Download Presentation

20.1

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. 20.1 Hydrogen Ions and Acidity Section 20.2

  2. Self-ionization - the reaction in which two water molecules produce ions H2O  H+ + OH- Water Hydrogen ion hydroxide ion H2O + H2O  H30+ + OH- Water Water Hydronium ion hydroxide ion Pure Water: neutral solution [H30+] = 1.0 x 10-7 M [OH-] = 1.0 x 10-7 M Kw = ion-product constant for water Kw = [H30+] [OH-] = 1.0 x 10-14 M

  3. Remember LeChatelier?? What happens to the H+ concentration when the OH- concentration increases? H2O  H+ + OH- Acidic: when [H+] is greater than [OH-] Basic: when [OH-] is greater than [H+] AKA: Alkaline solution

  4. Use the Kw expression to solve the following: Kw = [H30+] [OH-] = 1.0 x 10-14 M 1. What is [H30+] equal to if [OH-] is 1.9 x10-2 M? 2. What is the hydroxide concentration if the hydronium concentration is 5.1 x10-9 M?

  5. pH: scale used to measure how acidic or basic a solution is pH = - log [H30+] Acid: pH < 7.0 [H30+] > 1 x 10-7 Neutral: pH = 7.0 [H30+] = 1 x 10-7 Base: pH > 7.0 [H30+] < 1 x 10-7

  6. Equations for all pH and related problems... pH = - log [H30+] pOH = - log [OH-] [H30+] = inv log (-pH) [OH-] = inv log (-pOH) pH + pOH = 14 [H30+] [OH-] = 1.0 x 10-14 M

  7. Complete the following table using the equations on the previous slide:

  8. Acid / Base Indicators HIn  H+ + In- acid form base form Use LeChatelier to determine which direction the reaction will shift... More [H+]…reaction shifts __________ Less [H+]…reaction shifts __________

More Related