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Chapter 16: Problem 98

Phosphorous acid is listed in Appendix D as a diprotic acid. Propose a Lewis structure for phosphorous acid that is consistent with this fact.

Short Answer

Expert verified
Phosphorus is the central atom bonded with three oxygen atoms. Two of these oxygen atoms are further bonded with one hydrogen atom each. The two protons donated originate from these hydrogen atoms, indicating that phosphorus acid is a diprotic acid.

Step by step solution

01

Identify the central atom.

Phosphorus is the central atom because it is the least electronegative element in phosphorus acid.
02

Determine the total number of valence electrons

Phosphorous has 5 valence electrons, each oxygen has 6 and each hydrogen has 1. In total there are: \(5+(3 \times 6)+(3 \times 1)= 23\) valence electrons.
03

Draw the structure

Place Phosphorus in the center and arrange oxygen and hydrogen atoms around it. For a start, connect them with single bonds. Then fill the octets of other atoms starting with the most electronegative atom (Oxygen) before returning to the central atom.
04

Check the formal charges

Considering Formal charges: Phosphorus has +1, each oxygen bonded with hydrogen has 0, and the oxygen bonded only with phosphorus has -1. This implies that the structure satisfies the Formal Charge criterion, having charges as close as possible to zero.

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Most popular questions from this chapter

Briefly describe each of the following ideas or phenomena: (a) conjugate base; (b) percent ionization of an acid or base; (c) self-ionization; (d) amphiprotic behavior.

What is the (a) degree of ionization and (b) percent ionization of propionic acid in a solution that is \(0.45 \mathrm{M}\) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H} ?\) $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}\\\ &&\mathrm{p} K_{\mathrm{a}}=4.89 \end{aligned}$$

Codeine, \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{O}_{3} \mathrm{N},\) is an opiate, has analgesic and antidiarrheal properties, and is widely used. In water, codeine is a weak base. A handbook gives \(\mathrm{p} K_{\mathrm{a}}=6.05\) for protonated codeine, \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{O}_{3} \mathrm{NH}^{+} .\) Write the reaction for \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{O}_{3} \mathrm{NH}^{+}\) and calculate \(\mathrm{p} K_{\mathrm{b}}\) for codeine.

Adipic acid, \(\mathrm{HOOC}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH},\) is among the top 50 manufactured chemicals in the United States (nearly 1 million metric tons annually). Its chief use is in the manufacture of nylon. It is a diprotic acid having \(K_{\mathrm{a}_{1}}=3.9 \times 10^{-5}\) and \(K_{\mathrm{a}_{2}}=3.9 \times 10^{-6} .\) A saturated solution of adipic acid is about \(0.10 \mathrm{M}\) \(\mathrm{HOOC}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH} .\) Calculate the concentration of each ionic species in this solution.

The antimalarial drug quinine, \(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{O}_{2} \mathrm{N}_{2},\) is a diprotic base with a water solubility of \(1.00 \mathrm{g} / 1900 \mathrm{mL}\) of solution. (a) Write equations for the ionization equilibria corresponding to \(\mathrm{p} K_{\mathrm{b}_{1}}=6.0\) and \(\mathrm{p} K_{\mathrm{b}_{2}}=9.8\) (b) What is the \(\mathrm{pH}\) of saturated aqueous quinine?
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