Karli S.

Write the Lewis structure for each molecule.
$\begin{array}{ll}{\text { a. } S F_{2}} & {\text { b. } \operatorname{SiH}_{4}} \\ {\text { c. HCOOH (both O bonded to } C )} & {\text { d. } C H_{3} S H(C \text { and } S \text { central) }}\end{array}$

What two components make up a buffered solution? Give an example of a combination that would serve as a buffered solution.

The concepts of acid–base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted–Lowry acid–base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia, $\mathrm{NH}_{3}$ .
a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia.
b. Write a chemical equation indicating how $\mathrm{OH}^{-}$ behaves as a base in liquid ammonia.

Is it possible for a solution to have $\left[\mathrm{H}^{+}\right]=0.002 \mathrm{M}$ and $\left[\mathrm{OH}^{-}\right]=5.2 \times 10^{-6} \mathrm{M}$ at $25^{\circ} \mathrm{C}$ ? Explain.

According to Arrhenius, bases are species that produce _______ ion in aqueous solution.

According to the Bronsted–Lowry model, a base is a species that _______ protons.