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It is referred to as the freezing point when temperatures decrease below 32Â°F (0Â°C), causing water to change state from a liquid to a solid (ice), as happened with the cup of crushed ice immersed in the very cold salt/ice mixture.
You have a supply of ice in a freezer at -10.0 C and a glass containing 150 g of water at 25.0 C. How many grams of ice at -10.0 C must be added to the water to reduce the temperature of the water to 1.0 C? Ignore the heat capacity of the glass container. heat absorbed by the ice to warm it to 0Â°C (call it q1). 2  heat absorbed by the ice to melt it at 0Â°C (call it q2). 3  heat absorbed by the melted ice to warm it from 0.0 to 1.0 Â°C (call it q3). 4  heat released by the water to cool it from 25.0Â°C to 1.0 Â°C (call it q4). 5  Set up an energy conservation equation.