A calorimeter contains 95 g of water at 25.0°C. A 5.0 g sample of ice (18.02 g/mol) at -5.0°C is added to the water in the calorimeter, and eventually all of the ice melts. Calculate the final temperature of the water. Assume no heat is lost to the calorimeter or the surroundings.

CH₂O(l) = 4.184 J/g °C
CH₂O(s) = 2.04 J/g °C
ΔH fusion = 6.01 kJ/mol

a. 21.5°C
b. 20.7°C
c. 23.5°C
d. 17.5°C