A calorimeter contains $365g$ of water at $30\mathrm{.}0C.$ A $11\mathrm{.}3-$g sample of ice at $-11\mathrm{.}0C)$ 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. $($The heat of fusion of ice is $334\frac{J}{g}$; the specific heat capacity of ice is $2\mathrm{.}108\frac{J}{g}*C$; the specific heat capacity of water is $4\mathrm{.}184\frac{J}{?}g$