$$\Delta T_b = K_b \cdot m$$
where $\Delta T_b$ is the boiling point elevation, $K_b$ is the boiling point elevation constant of the solvent, and $m$ is the molality of the solution.
For water, the boiling point elevation constant is $K_b = 0.512 \degree\text{C/m}$. If the boiling point of water increases to $0.75 \degree\text{C}$ when a solute is added, then the molality of the solution is:
$$m = \frac{\Delta T_b}{K_b} = \frac{0.75 \degree\text{C}}{0.512 \degree\text{C/m}} = 1.46 \text{ m}$$
Therefore, the boiling point of water increases to $100.75 \degree\text{C}$ when a solute is added that increases the molality of the solution to $1.46 \text{ m}$.
