91Ó°ÊÓ

Which solute combinations can make a buffer? Assume all are aqueous solutions. 1\. \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) 2\. \(\mathrm{NaHCO}_{3}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) 3\. \(\mathrm{NaNO}_{3}\) and \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) 4\. \(\mathrm{HN}_{3}\) and \(\mathrm{NH}_{3}\)

Is each compound a strong acid or a weak acid? Assume all are in aqueous solution. 1\. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) 2\. \(\mathrm{HSO}_{4}\) 3\. \(\mathrm{HPO}_{4}^{2-}\) 4\. \(\mathrm{HNO}_{3}\)

List the general properties of bases.

Explain why a Brønsted-Lowry base can be called a proton acceptor.

A friend brings you a small sample of an unknown chemical. Assuming that the chemical is soluble in water, how would you determine if the chemical is an acid or a base?

Is each compound a strong base or a weak base? Assume all are in aqueous solution. 1\. \(\mathrm{NH}_{3}\) 2\. \(\mathrm{NaOH}\) 3\. \(\mathrm{Mg}(\mathrm{OH})_{2}\) 4\. \(\mathrm{Cu}(\mathrm{OH})_{2}\)

Write the chemical equation of the reaction of ammonia in water and label the Brønsted-Lowry acid and base.

Why is pure water considered neutral?

Is each compound a strong base or a weak base? Assume all are in aqueous solution. 1\. KOH 2\. \(\mathrm{H}_{2} \mathrm{O}\) 3\. \(\mathrm{Fe}(\mathrm{OH})_{2}\) 4\. \(\mathrm{Fe}(\mathrm{OH})_{3}\)

Write the chemical equation of the reaction of methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)\) in water and label the Brønsted-Lowry acid and base.