please refer to images and answer bi bii and biii b.) Starting with a 0.55 M solution of H2A, you want to know the pH and the final concentrations of allions present. You find the Ka values for the two dissociation steps:Ka1= 1.5 x 10-4Ka2 = 2.0 x 10-7i.) The first step for this problem is to consider the first dissociation reaction on its own. Below, solve forthe concentrations of the ions involved at the end of the first dissociation and the percent ionization.You should end up with 3 total concentrations. ii.) Now you've accounted for the ionization of the first proton. But what about the second step? You'llneed to make another RICE chart to figure out what the final concentrations of all the ions will be. Thinkcarefully about what your initial values should be. (Hint: instead of x, you might want to use y this timeto make your work less confusing). Solve for all the final concentrations and the pH. You should end upwith 4 total concentrations.iii.) If all went well, you should have found that y is approximately equal to Ka2. Why is this the case?(Look at your Ka2 expression and consider the size of y).

conc. = 0.55 M Acid = H2A Ka1 = 1.5 ×10-4 Ka2 =2.0 × 10 -7

b.) Starting with a 0.55 M solution of H2A, you want to know the pH and the final concentrations of all ions present. You find the Ka values for the two dissociation steps: Ka1 = 1.5 x 10-4 Ka2 = 2.0 x 10-7 i.) The first step for this problem is to consider the first dissociation reaction on its own. Below, solve for the concentrations of the ions involved at the end of the first dissociation and the percent ionization. You should end up with 3 total concentrations.

b.) Starting with a 0.55 M solution of H2A, you want to know the pH and the final concentrations of all ions present. You find the Ka values for the two dissociation steps: Ka1 = 1.5 x 10-4 Ka2 = 2.0 x 10-7 i.) The first step for this problem is to consider the first dissociation reaction on its own. Below, solve for the concentrations of the ions involved at the end of the first dissociation and the percent ionization. You should end up with 3 total concentrations.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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