Why is salt so hard to remove from water? Water molecules and various salt molecules are very different.  However, it seems very difficult to separate the two.  Once a salt is dissolved in water, an energy or chemical intensive method (like boiling) is required to separate the salt back out again.  Why is this? 
 A: From The Feynman Lectures on Physics, Vol. I [1]:

If we put a crystal of salt in the water, what will happen? Salt is a solid, a crystal, an organized arrangement of “salt atoms.” [...] Strictly speaking, the crystal is not made of atoms, but of what we call ions. An ion is an atom which either has a few extra electrons or has lost a few electrons. In a salt crystal we find chlorine ions (chlorine atoms with an extra electron) and sodium ions (sodium atoms with one electron missing). The ions all stick together by electrical attraction in the solid salt, but when we put them in the water we find, because of the attractions of the negative oxygen and positive hydrogen for the ions, that some of the ions jiggle loose. 

Figure 1-6 
In Fig. 1–6 we see a chlorine ion getting loose, and other atoms floating in the water in the form of ions. This picture was made with some care. Notice, for example, that the hydrogen ends of the water molecules are more likely to be near the chlorine ion, while near the sodium ion we are more likely to find the oxygen end, because the sodium is positive and the oxygen end of the water is negative, and they attract electrically.

Feynman has done well in explaining you the process in atomic point of view. Now comes your complexity of separating salt from water in a salt solution. During the process of boiling, the intermolecular forces will be broken between water molecules, and also between ions and water molecules.
Water molecules ($\mathrm{H_2O}$) being less massive ($18.01528(33)$) than the other two individual ions ($\mathrm{Na}$, $22.98976928(2)$ – $\mathrm{Cl}$, $35.45(1)$), flies off easily leaving sodium and chlorine ions. These ions once again attract each other to form crystals. In other words, energy is required to break the intermolecular forces and release ions from prison to join their partners.   
Reference


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*Feynman Lectures on Physics. Vol. 1, pp. 1–6 (numbers may vary depending on edition). 

A: In short, they are hard to separate, because even though the molecules are very different, they have properties that attract them to each other.
Water is a polar molecule. The oxygen molecule oxidizes the two hydrogen molecules, creating a positive charge on the hydrogen side, and a negative charge on the oxygen side.
Meanwhile, salt is composed of sodium, a positive ion, and chlorine, a negative ion. The charges on the water molecule attract the oppositely charged ions and pull them off of the salt crystal, effectively breaking the salt apart at the molecular level.
Then energy that it takes to separate the particles back again is essentially what is needed to counteract these attractive forces.
A: You can see that the enthalpy of hydration is a two step proccess of solvation and reverse crystallization. The $\Delta H_\mathrm{hydr}$ is actually positive, so you have to give energy just to dissolve the $\mathrm{NaCl}$ in water. In order to separate the water from the $\mathrm{NaCl}$, you need to account for the enthalpy of evaporation of water and the enthalpy of reverse hydration:

The temperature is in Kelvins, so going at around the $300\,\rm K$ mark you can see the $\Delta H_\mathrm{evap}$ is $44\,\rm KJ/mol$. Substracting the $\Delta H_\mathrm{hydr}$, you get a lower $\Delta H$, meaning that the salt actually lowered the energy required to boil off the water.
