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Chapter 18: Q89E (page 1047)

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.

Short Answer

Expert verified

Therefore, this will result in the easier release of hydrogen in\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\), making it a stronger acid.

Step by step solution

01

To find the stronger acid.

If we compare two acids, such as\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\)and\({{\rm{H}}_2}{\rm{Se}}{{\rm{O}}_4}\)where\({\rm{S}}\)and\(Se\)have the same oxidation number, stronger is the one with a higher electro negativity of a central atom.

Electro negativity of\({\rm{S}}\)is\(2.5\), while the electro negativity of\(Se\)is\(2.4\).

Since sulfur is more electronegative than selenium, the shared electron pair between the central atom and\(O\)will be more attracted by sulfur in\({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\)than selenium in\({{\rm{H}}_2}{\rm{Se}}{{\rm{O}}_4}\).

This will result in the easier release of hydrogen in \({{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\), making it a stronger acid.

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Most popular questions from this chapter

Assign an oxidation state to phosphorus in each of the following:

(a) \({\rm{Na}}{{\rm{H}}_2}{\rm{P}}{{\rm{O}}_3}\)

(b) \({\rm{P}}{{\rm{F}}_5}\)

(c) \({{\rm{P}}_4}{{\rm{O}}_6}\)

(d) \({{\rm{K}}_3}{\rm{P}}{{\rm{O}}_4}\)

(e) \({\rm{N}}{{\rm{a}}_3}{\rm{P}}\)

(f) \({\rm{N}}{{\rm{a}}_4}{{\rm{P}}_2}{{\rm{O}}_7}\)

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

(b) \(O{F_2}\)

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