According to Wikipedia:
The atmospheric pressure on the Martian surface averages 600 pascals (0.087 psi; 6.0 mbar), about 0.6% of Earth's mean sea level pressure of 101.3 kilopascals (14.69 psi; 1.013 bar).
This chart seems to indicate that the 77°F (25°C) water would be above its boiling point by more than 75°F (the granularity of the chart does not give more info).
This would result in a (perhaps explosive) boiling of the pool until it had released enough energy to be below its boiling point in the 6°F to -24°F (-14°C to -31°C) range. At this point the remaining water may freeze and sublimate in the future.
But, according to Wikipedia, the surface of Mars is between -226°F (-143°C) and 95F (35°C), so depending on conditions the pool may never cool below its boiling point, and all of it simply evaporates.
@Dean MacGregor correctly points out that at 600Pa water will never be a stable liquid, so the final result (after 'explosive' boiling) will eventually be that all the water evaporates, or a portion boils off, allowing the remainder to cool to ice, which may or may not sublimate. All depending largely on the temperature of this particular part of Mars.
As a demonstration, this is a video of water being subjected to a vacuum at room temperature. On those conditions the water boils, until it cools to freezing.