I'm not sure if I remember how to solve these kinds of problems but I'll give it a shot.

Assuming the heat of fusion for ice is 334 J/g, the amount of energy required to melt 100g of ice is (100g)*(334J/g) = 33400J. This amount of energy must be absorbed from the rest of the system. The following equation can be used to determine the temperature change of the water:

(q is the energy transferred, m is the mass of the substance, c is specific heat capacity of the substance, delta T is the change in temperature)

Substituting in all known values, we are left with

-33400J = (1000g)*(4.184J/g*C)*delta T

Solving for delta T, we have

delta T = (-33400J)/[(1000g)*(4.184J/g*C)] ≈ -7.98 degree C

Solving for the final temperature, we get

80 degree C + (-7.98 degree C) = 72.0 degree C

You can adjust these values for significant figures as you see fit. You also may want to check my work to see if I made any mistakes.

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