Problem 8
Explain why NaBr cannot be a component in either an acidic or a basic buffer.
Problem 9
Identify each salt as neutral, acidic, or basic. a) \(\mathrm{NaBr}\) b) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\) c) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\)
Problem 9
Write the balanced chemical equation for the neutralization reaction between \(\mathrm{HCl}\) and \(\mathrm{Fe}(\mathrm{OH})_{3} .\) What is the salt?
Problem 9
What is the \(\mathrm{pH}\) of a solution when \(\left[\mathrm{H}^{+}\right]\) is \(3.44 \times 10^{-4} \mathrm{M}\) ?
Problem 9
For a given aqueous solution, if \(\left[\mathrm{H}^{+}\right]=7.92 \times 10^{-5} \mathrm{M},\) what is \(\left[\mathrm{OH}^{-}\right] ?\)
Problem 9
Can an amphiprotic substance be a strong acid and a strong base at the same time? Explain your answer.
Problem 9
Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. $$ \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}+\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N} \rightarrow ? $$
Problem 9
Two solutions are made containing the same concentrations of solutes. One solution is composed of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{Na}_{3} \mathrm{PO}_{4}\), while the other is composed of HCN and \(\mathrm{NaCN}\). Which solution should have the larger capacity as a buffer?
Problem 10
Two solutions are made containing the same concentrations of solutes. One solution is composed of \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{4} \mathrm{NO}_{3},\) while the other is composed of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{Na}_{2} \mathrm{SO}_{4}\). Which solution should have the larger capacity as a buffer?
Problem 10
Can an amphiprotic substance be a weak acid and a weak base at the same time? If so, explain why and give an example.
