91Ó°ÊÓ

It takes \(9.77 \mathrm{~mL}\) of \(0.883 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) to titrate \(15.00 \mathrm{~mL}\) of KOH to its equivalence point. What is the original concentration of the KOH solution?

Can an amphiprotic substance be a strong acid and a strong base at the same time? Explain your answer.

For a given aqueous solution, if \(\left[\mathrm{H}^{+}\right]=7.92 \times 10^{-5} \mathrm{M},\) what is \(\left[\mathrm{OH}^{-}\right] ?\)

What is the \(\mathrm{pH}\) of a solution when \(\left[\mathrm{H}^{+}\right]\) is \(3.44 \times 10^{-4} \mathrm{M}\) ?

Identify each salt as neutral, acidic, or basic. a) \(\mathrm{NaBr}\) b) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\) c) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\)

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. $$ \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}+\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N} \rightarrow ? $$

Write the balanced chemical equation for the neutralization reaction between \(\mathrm{HCl}\) and \(\mathrm{Fe}(\mathrm{OH})_{3} .\) What is the salt?

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?

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?

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. $$ \left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{3} \mathrm{~N}+\mathrm{H}_{2} \mathrm{O} \rightarrow ? $$