There are some FEW ionic liquids, and their deployment is limited to the past 20-30 years...... $"1-butyl-3-methylimidazolium"$$"hexafluorophosphate"$ is a common ionic liquid, with a melting point of $265$$K$. The solubility of ionic solids in this is the subject of experiment; I could not find much data on the web.
Some ionic crystals display considerable solubility in water. Water is a protic, dipolar , i.e. $stackrel(delta+)H-stackrel(delta-)O-stackrel(delta+)H$, that can very efficiently solvate many ions. That is the solvent allows charge separation...
The first step is that the ionic compound is broken down due to the polarity of the surrounding water molecules with oxygen being electronegative and hydrogen being electropositive. Hence, the...
Many are insoluble in most solvents. Ionic are soluble in a suitable , and this is an experimental phenomenon. Water, as a polar, diprotic solvent can dissolve MANY ionic solutes,...
Both dissolve in a similar way, but are different in the detail. They dissolve because they are able to form more stable bonds or associations with the molecules than they...
The length of time this question has been unanswered means that it is a tricky proposition to address...so let us make a ham-fisted attempt here. We specify the as water...
Ionic are non-molecular; they do not have molecular boundaries. In the solid-state, each particle, each ion, is bound electrostatically to every other counterion in the lattice, and repelled by every...
Ionic compounds are inherently non-molecular. Each cation is electrostatically ATTRACTED to EVERY other anion in the crystal. Of course, each cation is electrostatically REPELLED by EVERY other cation in the...
$"Solubility"$ $=$ $"Moles of solute"/"Volume of solution"$. For silver chloride we are given that: $2.5*g$ wil dissolve in over $1$ $m^3$ of water. And thus, $"Solubility"$ $=$ $(2.5*g)/(143.32*g*mol^-1)xx1/(1.3xx10^3*L)$ $=$ $1.34xx10^-5*mol*L^-1$....
