Chemistry (Enthalpy) Problem

Since they already tell you the ice will be melt at then end, all you have to do is calculate how much energy you need to go from:
-9,3ºC to 0ºC as ice (ice heat capacity 37.5 J/K.mol times the temperature difference and total ammount of ice in mols)
Energy1 = (0 - (-9.3)) * (37.5) * (mols of ice)

-0ºC ice to 0ºC water (entalpy of fusion, 6.01*10³ J/mol times the ammount of ice in mols).
Energy2 = (mols of ice) * (6.01*10³)

Then you take these two ammounts of energy you used to heat the ice and you use it to calculate how much the water has cooled:
(Energy1 + Energy2) = (water heat capacity) * (Nº of mols of water) * (95.3º - NewTemperature)

After that, to the final temperature you just need to do a weighted average of the two bodies of water, the one at 0ºC and the one at the temperature you just calculated.
(mass of water at ºC) * (0ºC) + (mass of water at NewTemperature) * (NewTemperature) = (total mass of water) * (Final Temperature)

Also, take care for when the values of entalpy/heat capacity are in kJ or J. And be sure to use mols when the aforementioned are per mol.