just in general im really confused on the concepts of acids and bases in terms of Ka Kb and Kw vs. pka and pkb so for this problem could someone explain how to do it conceptually?
"The percentage deprotonation of benzoic acid in a 0.110 M solution is 2.4%. What is the pH of the solution and the Ka of benzoic acid."
12.63 Concepts
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Re: 12.63 Concepts
Postby Kevin Neumann 1A » Sun Nov 29, 2015 9:23 pm
In questions 12.55 and 12.59, you had to find the % protonation of the solute by finding the equilibrium concentration of H3O+ (the value of x in the ICE box) and dividing it by the original concentration of the acid/base that was given in the problem. This time, the % deprotonation is given to you, so you can find the concentration of H3O+.
0.024 (the % deprotonation) = X/0.11 M, where X is the concentration of H3O+. (0.11)(0.024)=0.00264 M is the conc. of H3O+.
From here, you have all the information you need to find Ka by using an ICE box for C6H5COOH+H2O > H3O+C6H5COO-.
0.024 (the % deprotonation) = X/0.11 M, where X is the concentration of H3O+. (0.11)(0.024)=0.00264 M is the conc. of H3O+.
From here, you have all the information you need to find Ka by using an ICE box for C6H5COOH+H2O > H3O+C6H5COO-.
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