Final answer:
The final temperature of water when ice is added is calculated using the conservation of energy and the specific heat capacities and latent heat of fusion for water. However, insufficient information was provided to complete the calculation in this case.
Step-by-step explanation:
To find the final temperature of water when a 0.035-kg ice cube at -30.0°C is placed in 0.435 kg of 35.0°C water, we must consider the heat energy required to (1) warm the ice to 0°C, (2) melt the ice, and (3) equilibrate the melted ice with the warmer water. The problem is based on the principle of conservation of energy, which states that the heat lost by the warm water will be gained by the ice (to raise its temperature and melt it). As the water and ice are in a well-insulated container, we assume no heat loss to the environment.
To solve for the final temperature, you need to use the specific heat capacities of water and ice, as well as the latent heat of fusion for water. Unfortunately, there was insufficient information given to solve the problem here, as the specific heats for water and ice were not provided. Typically, though, the process would involve calculating the heat required to raise the temperature of the ice to 0°C, the heat required to melt the ice, and the heat exchanged between the melted ice and the warm water until thermal equilibrium is reached.