Question

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

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

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.