Some uncharged organic compounds have so many polar functional groups that they are somewhat soluble in...

Some uncharged organic compounds have so many polar functional groups that they are somewhat soluble in water. During an extraction such compounds reside partially in the water layer and partially in the water-immiscible organic layer. Why does the addition of a salt (like NaCl) to the aqueous phase often diminish the solubility of the polar organic (uncharged) compounds in the aqueous phase (the process is referred to as “salting out”)? Please explain.

Solutions

Expert Solution

NaCl will increase ions in solution

Na+ and Cl-

Note that these ions will increase IONIC STRENGHT of solution

Recall that ionic strength considers all ions in solution, and its charges. It is typically used to calculate the ionic activity of other ions. The stronger the electrolytes, the more ionic strength they will have.

The formula:

I.S. = 1/2*sum( Ci * Zi^2)

Where

I.S. = ionic strength, M (also miu / μ ) used

Ci = concentration of ion “i”

Zi = Charge of ion “i”

Therefore, solubility is actually based on ACTIVITY

which depend directly on activity coefficients

which all depend directly to the ionic strenght

therefore

more ionic strneght, more activity coeff. more activity overall, more solubility

queen_honey_blossom answered 1 year ago

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