Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid.
a. Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions?
b. One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak?
c. Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer?
d. What is the concentration of A(aq) in the HA solution described in part c?
e. If HB(aq) is a strong acid, what is the hydronium-ion concentration?
f. In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide?
g. In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A(aq), HA(aq), or OH(aq)? How did you decide?
h. Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer.
i. You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA (aq)? Be sure to support your answer.