I understand how $\ce{NaCl}$ and $\ce{AlCl3}$ dissolves in water but I'm wondering why one is more conductive than the other. Is it their extra ions to conduct the electricity?

I know that in $\ce{NaCl}$ the water molecules 'steals' the Sodium or the Chloride depending on which end becomes closest to the material due to the Dipole-Dipole attraction. However, this reaction alone cannot break down the ionic lattice alone so there is a separate endothermic reaction. But I still can't understand the science behind why one conducts more than the other.

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    $\begingroup$ Your question might really benefit from adding more details, e.g. what do they conduct and in what conditions. Also, welcome to Chem.SE. $\endgroup$ – Ivan Neretin Mar 9 '16 at 10:13
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    $\begingroup$ This is a homework question. We have a policy which states that ‎you should show your thoughts and/or efforts into solving the problem. It'll make us certain that ‎we aren't doing your homework for you. Otherwise, this question may get closed.‎ $\endgroup$ – It's Over Mar 9 '16 at 10:51
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    $\begingroup$ @Kelsey ; clarify molar concentration of the solutions at the very least and if any other compounds are dissolved in the solutions $\endgroup$ – permeakra Mar 9 '16 at 11:13
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    $\begingroup$ @KlausWarzecha I don't think a high school student is going to be familiar with the Grotthuss diffusion mechanism. Heck, the people who wrote OP's textbook may not even know of it.... $\endgroup$ – hBy2Py Mar 9 '16 at 11:42
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    $\begingroup$ @Brian You're probably right and I was just overdoing the problem. Counting ions might be good enough here :) $\endgroup$ – Klaus-Dieter Warzecha Mar 9 '16 at 11:47

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