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Explain why the ions Na' and $\mathrm{Cl}^{-}$ are strongly solvated in water but not in hexane, a solvent composed of nonpolar molecules.
Solvation is the physical process in which the homogenous mixture of molecules of solvent and solute molecules is formed. The solubility is dependent on the nature of the solute and the solvent. The rule of thumb for predicting solubility is "like dissolves like" that is polar solute will be more soluble in polar solvent and non-polar solute in non-polar solvent. The ions $\mathrm{Na}^{+}$ and $\mathrm{Cl}^{-}$ are polar in nature and hence by the general rule it will be solvated by the water, which is also polar in mature. On the other hand, hexane is non-polar in nature and hence will not solvate the ions.
01:15
Aadit S.
Chemistry 102
Chapter 11
Solutions and Colloids
Solutions
Drexel University
University of Maryland - University College
University of Kentucky
Lectures
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To answer this question, we first need to recognize that sodium chloride is an ionic compound, and if dissolved in a solvent, it will disassociate into a cat eye on sodium and an an ion chloride. In order for this to occur, we need to overcome the strong attractive force between the sodium cat eye on and the chloride. An eye on. The only way that this can be overcome is if we have a polar solvents such as water, that has a partial positive end, that can attract the chloride away from the sodium and a partial negative end, that can attract the sodium away from the chloride in a fashion such as this. This is not possible with a non polar solvents, such as heck saying there's nothing associated with the non polar solvent hexane that allows for the interaction between the sodium cat eye on and the chloride, and I am to be overcome. Thus it won't dissolve.
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