1 / 8

Appendix III

Appendix III. pH and pOH. October 21, 2011 Equilibrium Unit. pH. A measure of the concentration of [H 3 O + ] in solution pH = - log [H 3 O + ] Conversely, [H 3 O + ] may be determined if pH of a solution is known. [H 3 O + ] = 10 -pH. pOH.

len-schroeder
Download Presentation

Appendix III

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. Appendix III

  2. pH and pOH October 21, 2011 Equilibrium Unit

  3. pH • A measure of the concentration of [H3O+] in solution pH = - log [H3O+] • Conversely, [H3O+] may be determined if pH of a solution is known. [H3O+] = 10-pH

  4. pOH • Similar to pH, pOH is a measure of the concentration of [OH-] in solution. pOH = - log [OH-] [OH-] = 10-pOH

  5. How are pH and pOH related? H2O(l) <===> H3O+(aq) + OH-(aq) Is the Kw value large or small? How do you know? Kw = [OH-][H3O+] = 1.0 x 10-14 @ 25°C It is mostly water and does not conduct electricity well.

  6. [H3O+] and [OH-] Acids and bases are determined by the relative [H3O+] and [OH-]. • neutral [H3O+] = [OH-] • acid [H3O+] > [OH-] • base [H3O+] < [OH-]

  7. Water Kw = [OH-][H3O+] = 1.0 x 10-14 What are the concentrations of [H+] and [OH-] of pure water? What happens when NaOH is added to water? HCl?

  8. Acids and Bases Interestingly, even in acidic and basic solutions. Kw = 1.0 x 10-14 Therefore, • if [H+] increases, [OH-] decreases • if [H+] decreases, [OH-] increases

More Related