A calorimeter contains 365 g of water at 30.0 °C. A 29.3-g sample of ice (at -11.0 °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.

Step 3: Calculate the heat lost by the water as it cools down from 30.0 °C to the final temperature \( T_f \) using the formula \( q = m \cdot c \cdot \Delta T \), where \( m \) is the mass of the water, \( c \) is the specific heat capacity of water (4.18 J/g°C), and \( \Delta T \) is the change in temperature (30.0 °C - \( T_f \)).

Step 4: Set up the equation for heat balance: the heat gained by the ice (from steps 1 and 2) is equal to the heat lost by the water (from step 3). Solve for the final temperature \( T_f \).