91Ó°ÊÓ

Define a Brønsted-Lowry acid and a Brønsted-Lowry base.

Explain in your own words what \(100 \%\) ionization means.

Write the chemical equation for the autoionization of water. Write the equilibrium constant expression for this reaction. What is the value of the equilibrium constant at \(25^{\circ} \mathrm{C} ?\) What is this constant called?

When \(\mathrm{OH}^{-}\) is the base in a conjugate acid-base pair, the acid is ________ ; when \(\mathrm{OH}^{-}\) is the acid, the base is __________.

Designate the acid and the base on the left side of these equations, and designate the conjugate partner of each on the right side. (a) \(\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})\) (b) \(\mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{CN}^{-}(\mathrm{aq}) \longrightarrow \mathrm{NH}_{3}(\mathrm{aq})+\mathrm{HCN}(\mathrm{aq})\)

Dissolving ammonium bromide in water gives an acidic solution. Write a balanced equation showing how that can occur.

Solution A has a pH of 8 and solution \(\mathrm{B}\) a p \(\mathrm{H}\) of 10 Which has the greater hydronium ion concentration? How many times greater is its concentration?

Contrast the main ideas of the Brønsted-Lowry and Lewis acid-base definitions. Name and write the formula for a substance that behaves as a Lewis acid but not as a Brønsted-Lowry acid.

Write a chemical equation to describe the proton transfer that occurs when each of these acids is added to water. (a) \(\mathrm{HCO}_{3}^{-}\) (b) HCl (c) \(\mathrm{CH}_{3} \mathrm{COOH}\) (d) HCN

Write a chemical equation to describe the proton transfer that occurs when each of these acids is added to water. (a) HIO (b) \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH}\) (c) HOOCCOOH (d) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\)