To understand why, let's consider the intermolecular forces between the molecules of each liquid. In water, the molecules are held together by strong hydrogen bonds. These hydrogen bonds are a type of dipole-dipole interaction that occurs between the hydrogen atoms of one molecule and the oxygen atom of another molecule. In contrast, the molecules of alcohol are held together by weaker van der Waals forces. Van der Waals forces are a type of temporary dipole-dipole interaction that occurs between any two molecules that are close to each other.
Because the hydrogen bonds in water are stronger than the van der Waals forces in alcohol, it takes more energy to break the hydrogen bonds and evaporate water. In other words, it takes more energy to overcome the intermolecular forces and separate the molecules of water from each other. As a result, water has a higher boiling point than alcohol.