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Chapter 13: Problem 3

According to the Bronsted-Lowry theory, which of the following would you expect to act as an acid? Which as a base? (a) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}\) (b) \(\mathrm{HClO}\) (c) \(\mathrm{CN}^{-}\)

Short Answer

Expert verified
Question: Identify the role of each substance as an acid or a base according to the Bronsted-Lowry theory: a) \(\mathrm{C}_{2}\mathrm{H}_{5}\mathrm{NH}_{3}{ }^{+}\) b) \(\mathrm{HClO}\) c) \(\mathrm{CN}^{-}\) Answer: a) \(\mathrm{C}_{2}\mathrm{H}_{5}\mathrm{NH}_{3}{ }^{+}\) acts as an acid. b) \(\mathrm{HClO}\) acts as an acid. c) \(\mathrm{CN}^{-}\) acts as a base.

Step by step solution

01

(Identifying Acid or Base for \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}\))

To analyze whether \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}\) is an acid or a base, take note of the positive charge on the nitrogen atom. This means that it has an extra proton (H+), which it can potentially donate. Therefore, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}\) will act as an acid.
02

(Identifying Acid or Base for \(\mathrm{HClO}\))

In the case of \(\mathrm{HClO}\), notice that it contains an acidic hydrogen (H+) bonded to an oxygen atom (O), which is known to be electronegative. This feature makes it easy to dissociate and donate a proton. As a result, \(\mathrm{HClO}\) will act as an acid.
03

(Identifying Acid or Base for \(\mathrm{CN}^{-}\))

Considering the negatively charged \(\mathrm{CN}^{-}\), it has an electron pair on the carbon atom, making it capable of accepting a proton (H+). Consequently, \(\mathrm{CN}^{-}\) will act as a base according to the Bronsted-Lowry theory.

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Most popular questions from this chapter

Milk of Magnesia has a pH of \(10.5\). (a) Calculate \(\left[\mathrm{H}^{+}\right]\). (b) Calculate the ratio of the \(\mathrm{H}^{+}\) concentration of gastric juice, \(\mathrm{pH} 1.5\), to that of Milk of Magnesia.

Calculate \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in solutions with the following \(\mathrm{pH}\). (a) \(4.0\) (b) \(8.52\) (c) \(0.00\) (d) \(12.60\)

There are \(324 \mathrm{mg}\) of acetylsalicylic acid \((\mathrm{MM}=180.15 \mathrm{~g} / \mathrm{mol})\) per aspirin tablet. If two tablets are dissolved in water to give two ounces \(\left(\frac{1}{16}\right.\) quart) of solution, estimate the \(\mathrm{pH} . K_{\mathrm{a}}\) of acetylsalicylic acid is \(3.6 \times 10^{-4}\).

\(\mathrm{m}\) Find \(\left[\mathrm{OH}^{-}\right]\) and the \(\mathrm{pH}\) of the following solutions. (a) \(0.25 \mathrm{~g}\) of \(\mathrm{Ba}(\mathrm{OH})_{2}\) dissolved in enough water to make \(0.655 \mathrm{~L}\) of solution. (b) A 3.00-L solution of KOH is prepared by diluting \(300.0 \mathrm{~mL}\) of \(0.149 \mathrm{MKOH}\) with water. What is the molarity of the diluted solution? What is the effect of a tenfold dilution on the \(\mathrm{pH}\) ?

WEB The pH of a \(2.642 M\) solution of a weak acid, \(\mathrm{HB}\), is \(5.32\). What is \(K_{\mathrm{a}}\) for the weak acid?
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