5 posts • Page 1 of 1
In the Lecture 6 example of partial dissociation, we used 1.3x10^-3 as the concentration for CH3COO-, is this because there are the same molar ratio of CH3COO- in the reaction as there is H3O+? If not, how did we figure out that the concentration of CH3COO- was this value?
If you meant that CH3COO and H30 had the same stoichiometric coefficients, then yes you are correct. We get the value by setting the Ka value equal to [CH3COO][H3O]/[CH3COOH] and plugging in the values from the ICE box to get 1.8 x 10-5 = x2/0.1-x. Then solving for x you get 1.3 x 10-3.
Who is online
Users browsing this forum: No registered users and 1 guest