If exactly molecules of urea are present in of its aqueous solution, the molarity of the solution is — Solutions and Colligative Properties Chemistry Question

💡 Solution & Explanation

Moles of urea $= \frac{6.02 \times 10^{20}}{6.02 \times 10^{23}} = 10^{-3}\text{ moles}$. Volume $= 100\text{ mL} = 0.1\text{ L}$. Molarity $= \frac{10^{-3}}{0.1} = 0.01\text{ M}$.