"To determine ΔHfusion of water you will essentially add ice to water, allow the ice to melt, and note the temperature change of the water. Let's first get an idea of the ratio of water to ice that you will need.
The value for the ΔHfusion of water is 6.0 kJ/mol. Let's suppose you start with 31.5 g of ice. Determine ΔH for melting 31.5 g of ice."
Now let's suppose you add the 31.5 g of ice to water at a normal temperature in the lab (25°C).
If you want to add the ice to a minimum amount of water to melt all of the ice, what will the final temperature of the water in the calorimeter be after all of the ice has melted?
What is the minimum mass of 25°C water required to melt all 31.5 g of ice?
Given that the density of water at 25°C is 0.9970 g/mL, what is the minimum volume of water required to melt 31.5 g of ice?