There is a question in my coursework:
0.76g of substance of R.M.M. = 132 is dissolved in 27g of water and raises its boiling point by 0.333oC. Calculate the apparent boiling-point constant for water and compare it with the actual value of 0.52 K mol-1 1000g-1. Explain this anomaly.
Here is my working,
n=0.76/132 = 5.758X10-3 mol of substance
5.758X10-3 mol of substance = 0.027Kg H2O X m/Kg H2O
X = 0.213m
let kb as Y,
0.333/Y=0.213m, Y = 1.562.
1.562 compares to 0.52 which is 3 times larger than the actual value, how to explain this anomaly?