...And if this step is endothermic, then is it true that the substance will be soluble in water? Is it true that its solubulity will increase as the temperature decreases? Or, will the substance be insoluble in water (or even insoluble in all solvents)?
2007-03-13 12:52:05 · 3 answers · asked by Random G 3 in Science & Mathematics ➔ Chemistry
Breaking ionic bonds is always an endothermic process. However, when solvation occurs (water molecules surrounding the ions), this is an energy favorable process.
Entropy plays a role in forming an aqueous solution, too...you're going from a system of low entropy (the solid) to high entopy and disorder (the solution).
So I don't think you can determine an ionic compounds solubility just by looking at whether dissociation is endothermic.
Finally, the general rule is that the solubility of solids INCREASES as you increase the temperature of the solvent.
2007-03-13 13:03:51 · answer #1 · answered by ihatedecaf 3 · 0⤊ 0⤋
It is true that the substance will be soluble in water if water can hydrate the cations and anions with the net liberation of energy (exothermic). This is the Haber-Born cycle. If the overall process is exothermic, then solubility will increase with temperature. The substance will be insoluble in water or in any solvent if these conditions are not met. For example, silver chloride and barium sulfate are famously insoluble in water.
2007-03-13 13:08:24 · answer #2 · answered by steve_geo1 7 · 0⤊ 0⤋
hi while Nacl (salt) dissolves thoroughly in water, there could be no ionic bonds left! so as meaning that it could not be an ionic compound. and Hcl (aq) capacity Hcl + Water, so back this is not an ionic bond.... and sry i don't be responsive to approximately CH3COOH
2016-12-19 04:50:40 · answer #3 · answered by ? 3 · 0⤊ 0⤋