Chapter 8: Q96E (page 298)
The common ion effect for ionic solids (salts) is to significantly decrease the solubility of the ionic compound in water. Explain the common ion effect.
The common ion effect can be explained.
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Question: What if all you know about two salts is that the value of Ksp for salt A is greater than that of salt B? Why can we not compare the relative solubilities of the salts? Use numbers to show how salt A could be more soluble than salt B, and how salt B can be more soluble than salt A.
Which of the indicators in Fig. 8.8 could be used for doing the titrations in Exercises 68 and 70?
The solubility of Ce(IO3)3 in a 0.20M KIO3 solution is 4.4 x 10-8 mol/L. Calculate Ksp forCe(IO3)3
A friend asks the following: “Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base such as NaOH is added, the HA reacts with the OH-to make A-. Thus, the amount of acid (HA) is decreased, and the amount of base (A-) is increased. Analogously, adding HCl to the buffered solution forms more of the acid (HA) by reacting with the base (A-). Thus how can we claim that a buffered solution resists changes in the pH of the solution?” How would you explain buffering to your friend?
Question:A 0.200-g sample of a triprotic acid (molar mass =165.0 g/mol) is dissolved in a 50.00-mL aqueous solutionand titrated with 0.0500 M NaOH. After 10.50 mL of thebase was added, the pH was observed to be 3.73. The pH
at the first stoichiometric point was 5.19 and at the second stoichiometric point was 8.00.
a. Calculate the three Ka values for the acid.
b. Make a reasonable estimate of the pH after 59.0 mLof 0.0500 M NaOH has been added. Explain youranswer.
c. Calculate the pH after 59.0 mL of 0.0500 M NaOHhas been added
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