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Chapter 13: Problem 161

Students are often surprised to learn that organic acids, such as acetic acid, contain - OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as \(\mathrm{H}_{2} \mathrm{SO}_{4}\) has the structural formula \(\mathrm{SO}_{2}(\mathrm{OH})_{2},\) where \(\mathrm{S}\) is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. \(\mathrm{SO}(\mathrm{OH})_{2}\) b. \(\mathrm{ClO}_{2}(\mathrm{OH})\) c. \(\mathrm{HPO}(\mathrm{OH})_{2}\)

Short Answer

Expert verified
The given structural formulas represent the following acids: a. \(H_{2}SO_{3}\) (Sulfurous acid), b. \(HClO_{2}\) (Chlorous Acid), and c. \(H_{3}PO_{4}\) (Phosphoric Acid). These compounds act as acids due to their ability to donate protons (H+) as a result of the electronegativity difference between the central atom and the O-H bond. On the other hand, NaOH and KOH act as bases because they contain OH- ions, which are capable of accepting protons (H+).

Step by step solution

01

Identifying the Acids

From the structural formulas given, we can rewrite them as: a. \(\mathrm{SO}(\mathrm{OH})_{2}: H_{2}SO_{3}\) (Sulfurous acid) b. \(\mathrm{ClO}_{2}(\mathrm{OH}): HClO_{2}\) (Chlorous Acid) c. \(\mathrm{HPO}(\mathrm{OH})_{2}: H_{3}PO_{4}\) (Phosphoric Acid)
02

Acidic Behavior

Acids are substances that can donate a proton (H+) to other substances. In the case of oxyacids, the -OH group is connected to a central atom that is more electronegative. This electronegativity difference causes the central atom in the oxyacid to attract the electron pair in the O-H bond and makes the H atom in -OH group to loose electron to become ionized H+ atom which can be donated to the other substances.
03

Bases Behavior

Bases are substances that can accept a proton (H+). In the case of NaOH and KOH, they each have an OH- ion present in their structure. The presence of the electron pair in the O-H bond makes the OH- anion a strong nucleophile which is capable of accepting the ionic H+ from other substances. This behavior of being able to accept a proton makes NaOH and KOH behave as bases. So, in conclusion, the given structural formulas represent acids due to their ability to donate protons (H+). NaOH and KOH, on the other hand, behave as bases because they have an ion that is capable of accepting protons.

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Most popular questions from this chapter

Zinc hydroxide is an amphoteric substance. Write equations that describe \(\mathrm{Zn}(\mathrm{OH})_{2}\) acting as a Brönsted-Lowry base toward \(\mathrm{H}^{+}\) and as a Lewis acid toward \(\mathrm{OH}^{-}\).

A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and \(20.0 \mathrm{mL}\) concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate \(\left[\mathrm{H}^{+}\right],\left[\mathrm{OH}^{-}\right],\) and the \(\mathrm{pH}\) for this solution. [Hint: Concentrated HCl is \(38 \%\) HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO_ is 70.\% HNO_3 (by mass) and has a density of \(1.42 \mathrm{g} / \mathrm{mL} .]\)

Consider 0.10 \(M\) solutions of the following compounds: \(\mathrm{AlCl}_{3}, \mathrm{NaCN}, \mathrm{KOH}, \mathrm{CsClO}_{4},\) and NaF. Place these solutions in order of increasing \(\mathrm{pH}\).

What are the major species present in 0.015 \(M\) solutions of each of the following bases? a. KOH b. \(\mathrm{Ba}(\mathrm{OH})_{2}\) What is \(\left[\mathrm{OH}^{-}\right]\) and the \(\mathrm{pH}\) of each of these solutions?

A codeine-containing cough syrup lists codeine sulfate as a major ingredient instead of codeine. The Merck Index gives \(\mathrm{C}_{36} \mathrm{H}_{44} \mathrm{N}_{2} \mathrm{O}_{10} \mathrm{S}\) as the formula for codeine sulfate. Describe the composition of codeine sulfate. (See Exercise \(155 .\) ) Why is codeine sulfate used instead of codeine?
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