According to Wikipedia $\pu{100 mL}$ of water dissolve at $\pu{25 ^\circ{}C}$ about $\pu{35 g}$ of $\ce{NaCl}$ (1), but about $\pu{79 g}$ of $\ce{NaClO3}$ (2), and around $\pu{210 g}$ for $\ce{NaClO4}$ (3).

This looks to me roughly like its doubling solubility for every single higher level of oxidation.

Earlier I was under the impression that the % of $\ce{Cl}$ or % of $\ce{Na}$ in the water would still be the same, and the amount of additional oxygen is what could be causing the increase in solubility.... ie. now each molecule has 3 oxygen atoms as opposed to none in case of $\ce{NaCl}$. But this doesn't hold true.

I would also like to know what is the effect of multiple solutes sharing same atoms on each other. For example does dissolving some chlorate cause the solvent to hold more chloride ?

As you may have guess Chemistry isn't my strong suite, I know basic chemistry, but now when I am looking at it again.. the whole thing has changed atleast w.r.t what I was taught during my school days. (right from how we determine the number of electrons)

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    $\begingroup$ There's no simple numerical dependence for solubility of different salts. That's why solubility tables are useful. $\endgroup$
    – Mithoron
    Commented Jun 9, 2017 at 21:45

2 Answers 2


Science is all about discovering hidden regularities, patterns, and laws. In that sense your bold generalization is good, but will it hold if we check just one more data point? Let's see: $\ce{KCl}$ has solubility of 25g/100ml, $\ce{KClO3}$ has 8, and $\ce{KClO4}$ has 1.5. Er, well...

What we have here is an interplay between solvatation energy and lattice energy, the latter being determined by the crystal structure, which is a tricky thing, and hence so is solubility. Don't expect it to be predictable from qualitative considerations. You don't know it until you measure it. Chemistry is an experimental science, after all.


The solubility of a salt depends on 2 factors:

  1. Force of attraction between H2O molecules and the ions of the solid. This force tends to bring ions into solution. If this is the predominant factor, then the compound may be highly soluble in water.

  2. Force of attraction between oppositely charged ions.This force tends to keep the ions in the solid state. When it is a major factor, then water solubility may be very low.

According to point 2, if the force of attraction between the oppositely charged ions is more, more energy is needed to break them and hence lattice enthalpy of that salt is more.

First, we compare sodium chloride and sodium chlorate. Force between sodium cation and chloride ion is way stronger than that with chlorate ion. So lattice enthalpy of sodium chlorate is less than sodium chloride. So, sodium chlorate is more soluble in water.

Force between sodium cation and perchlorate anion is way less than that with chlorate ion. So lattice enthalpy of sodium perchlorate is less than sodium chlorate. So, sodium perchlorate is way more soluble in water than sodium chlorate.

Arranging the above points, we get solubility order:

Sodium perchlorate > sodium chlorate > sodium chloride.


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