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Chapter 16: Problem 8

Oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) has the following structure: An oxalic acid solution contains these species in varying concentrations: \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}, \mathrm{HC}_{2} \mathrm{O}_{4}^{-}, \mathrm{C}_{2} \mathrm{O}_{4}^{2-}\), and \(\mathrm{H}^{+}\). (a) Draw Lewis structures of \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) and \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\). (b) Which of the four species listed here can act only as acids, which can act only as bases, and which can act as both acids and bases?

Short Answer

Expert verified
\(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) can act as both an acid and a base, \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\) acts as a base, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) works as an acid and \(\mathrm{H}^{+}\) acts only as an acid.

Step by step solution

01

Lewis Structure of \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\)

The Lewis structure of \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) can be drawn by understanding that oxalic acid loses one of its acidic protons (H) to form the \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) ion. Thus the Lewis structure would look similar to the Lewis structure of Oxalic acid but with one less H.
02

Lewis Structure of \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\)

The Lewis structure of \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\) can be drawn by understanding that oxalic acid loses two of its acidic protons (H) to form the \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\) ion. Thus the Lewis structure would look similar to the Lewis structure of Oxalic acid but with two less H.
03

Identify Acidic and Basic Species

A substance is an acid if it donates a proton (H+) and a base if it accepts a proton. \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) can donate two H+ ions, so it acts as an acid. \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) can donate an H+ ion and can also accept an H+ ion, so it can act as both an acid and a base. \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\) can only accept H+ ions, so it acts only as a base. \(\mathrm{H}^{+}\) is a proton donor and serves only as an acid.

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Most popular questions from this chapter

Which of the following is a stronger base: \(\mathrm{NH}_{3}\) or \(\mathrm{PH}_{3}\) ? (Hint: The \(\mathrm{N}-\mathrm{H}\) bond is stronger than the \(\mathrm{P}-\mathrm{H}\) bond. \()\)

Specify which of these salts will undergo hydrol\(\begin{array}{llll}\text { ysis: } \mathrm{KF}, & \mathrm{NaNO}_{3}, & \mathrm{NH}_{4} \mathrm{NO}_{2}, & \mathrm{MgSO}_{4}, & \mathrm{KCN},\end{array}\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}, \mathrm{RbI}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{CaCl}_{2}, \mathrm{HCOOK}\).

The disagreeable odor of fish is mainly due to organic compounds \(\left(\mathrm{RNH}_{2}\right)\) containing an amino group, \(-\mathrm{NH}_{2}\), in which \(\mathrm{R}\) is the rest of the molecule. Amines are bases just like ammonia. Explain why putting some lemon juice on fish can greatly reduce the odor.

Classify each of these following species as a Lewis acid or a Lewis base: \((\mathrm{a}) \mathrm{CO}_{2},(\mathrm{~b}) \mathrm{H}_{2} \mathrm{O},(\mathrm{c}) \mathrm{I}^{-},(\mathrm{d}) \mathrm{SO}_{2}\) (e) \(\mathrm{NH}_{3},\) (f) \(\mathrm{OH}^{-}\) \((\mathrm{g}) \mathrm{H}^{+},(\mathrm{h}) \mathrm{BCl}_{3}\).

Compare the strengths of the following pairs of acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SeO}_{4},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{3} \mathrm{AsO}_{4}\).
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