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Chapter 18: Q94 E (page 1047)

Which is a stronger acid, sulfurous acid or sulfuric acid? Why?

Short Answer

Expert verified


\({\rm{SO}}_4^ - \) is the stronger acid because of stability\({\rm{SO}}_4^ - \)of ion.

Step by step solution

01

To find the stronger acid.

\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\)is much stronger acid then the\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_3}\)because there is an extra double bonded oxygen atom on the sulfur atom in sulfuric acid.

The unprotonated \(O\)helps with delocalization of electron in deprotonated ion making the\(SO_4^{2 - }\)ion more stable than the\(SO_3^{2 - }\)ion.

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Most popular questions from this chapter

Which is the stronger acid,\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\)or \({{\rm{H}}_2}{\rm{Se}}{{\rm{O}}_4}\)? Why? You may wish to review the chapter on acid-base equilibrium.

How many tons of \(C{a_3}{\left( {P{O_4}} \right)_2}\)are necessary to prepare 5.0 tons of phosphorus if the yield is 90 % ?

Give the hybridization and oxidation state for sulfur in\({\rm{S}}{{\rm{O}}_2}\), in\({\rm{S}}{{\rm{O}}_3}\), and in\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\).

Determine the oxidation number of each element in each of the following compounds:

(a) \({\bf{HCN}}\)

(b) \(O{F_2}\)

(c) \(AsC{l_3}\)

Name each of the following compounds:

\(\begin{array}{l}(a){\rm{Br}}{{\rm{F}}_3}\\(b){\rm{NaBr}}{{\rm{O}}_3}\\(c){\rm{PB}}{{\rm{r}}_5}\\(d){\rm{NaCl}}{{\rm{O}}_4}\\(e){\rm{KClO}}\end{array}\)
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