To calculate the quantity of heat required to melt 50.0 g of ice at its melting point, we can use the formula:q = n Hfwhere q is the heat required, n is the number of moles of ice, and Hf is the enthalpy of fusion of water.First, we need to calculate the number of moles of ice. The molar mass of water HO is 18.015 g/mol. So, we can find the number of moles n using the formula:n = mass / molar massn = 50.0 g / 18.015 g/moln 2.776 molesNow, we can calculate the heat required q using the enthalpy of fusion of water 6.01 kJ/mol :q = n Hfq = 2.776 moles 6.01 kJ/molq 16.68 kJTherefore, the quantity of heat required to melt 50.0 g of ice at its melting point is approximately 16.68 kJ.