1 / 2

Calculating the pH of a 0.005 M Ammonia Solution

This example problem illustrates the step-by-step process of calculating the pH of a 0.005 M ammonia (NH3) solution. Given the base dissociation constant (Kb = 1.8 x 10^-5), we set up an ICE table to track the concentration changes. We assume that x, the change in concentration, is negligible compared to the initial concentration. By rearranging and solving the equation, we find that x equals 2.91 x 10^-4. From this value, we calculate the pH as -log(2.91 x 10^-4), resulting in a pH of approximately 3.53.

tanek
Télécharger la présentation

Calculating the pH of a 0.005 M Ammonia Solution

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. Example Problem: Weak Base Calculate the pH of a 0.005M solution of Ammonia 0.005 M ------- 0 M 0 M I C E -x ------- +x +x 0.005-x ------- +x +x Kb=1.8x10-5 = Assumption check:

  2. https://todaysmeet.com/1CBrindley Example Problem Cont.: Weak Base 0.005 M ------- 0 M 0 M I E Kb=1.8x10-5= 0.005-x ------- +x +x Rearranging => x=2.91x10-4 Solve for pH =-log(2.91x10-4)=3.53 10.5

More Related