a. when 0.10 mol of the ionic sold NaX, where X is an unknownanion, is dissolved in enough water to make 1.0 L of solution, thepH of the solution is 9.12. When 0.10 mol of the ionic solid ACl,where A is an unknown cation, is dissolved in enough water to make1.0 L of solution, the pH of the solution is 7. What would be thepH of the 1.0 L of solution that contained 0.10 mol of AX? Be sureto document how you arrived ar your answer.
b. In the AX solution prepared above, is there any OH-present? If so, compare the [OH-] in the solution to the[H3O+].
c. From the information presented in part A, calculate Kb forthe X^- (aq) anion and Ka for the conjugate acid of X^- (aq).
d. To 1.0 L of solution that contains 0.10 mol of AX, you add0.025 mol of HCl. How will the pH of this solution compare to thatof the solution that contained only NaX? Use chemical reactions aspart of your explanantion; you do not need to solve for a numericalanswer.
e. Another 1.0 L sample of solution is prepared by mixing 0.10mol of AX a d 0.10 mol of HCl. The pH of the resulting solution isfound to be 3.12. Explain why the pH of this solution is3.12.
f. Finally, consider a different 1.0 L sample of solution thatcontains 0.10 mol of AX and 0.1 mol of NaOH. The pH of thissolution is found to be 13. Explain why the pH of this solution is13.
g. Some students mistakenly think that a solution thatcontains 0.10 mol of AX and 0.10 mol of HCl should have a pH of1.00. Can you come up with a reason why students have thismisconception? Write an approach that you would use to help thesestudents understand what they are doing wrong.
