Electrical conductivity decreases as an acid becomes more concentrated because more ions form pairs. However, does that affect the speed of reaction of the acid as there is a smaller concentration of Hydrogen ions?
More ions form pairs when concentration of acid increases, does that decrease the speed of reaction?
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1$\begingroup$ Considering H3O+ activity coefficient steeply raises for high acid concentrations, it is the opposite. $\endgroup$– PoutnikCommented Apr 18, 2021 at 7:27
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In general, the conductivity of any liquid increases with the concentrations of its ions, and decreases with their dimensions. In pure sulfuric acid, the only ions existing are $\ce{H3SO4+}$ and $\ce{HSO4-}$. They are big and their concentration is low. So the conductivity of pure sulfuric acid is low. But when you add some water, the $\ce{H2O}$ molecules are totally transformed into $\ce{H3O+}$ and $\ce{HSO4-}$ ions which are numerous and sometimes small (for $\ce{H3O+}$). The conductivity must increase.
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$\begingroup$ Does this affect the number/concentration of H3O+ ions available for acid reactions? $\endgroup$ Commented Apr 18, 2021 at 11:33