When in a large block of ice at -5 degrees C a small hole is made and water at +50 degrees C is poured, initially ice in an area near the small hole will melt. After some time, though thermal eqilibrium will be established and what happens ultimately is dependent upon the relative sizes of both the ice block and the hole. The hot water will transfer heat to the ice block. Let the mass of the ice block be m, that of the hot water be m' and the final temperature 't'. Amount of heat released by the hot water = m'x1x(50-t) calories. This will be absorbed by the ice block to raise its temperature upto 't', requiring mx1x1 = m calories of heat per degree rise in temperature. Here, the ice block is large, so m is quite large in comparison to m', and the hole small, so 't' must be less than zero. Hence the water in the small hole too will freeze ultimately, and the temperature of the whole ice block will rise somewhat above -5 degrees C.