A solution of $$\text{CuSO}_4 \cdot 5\text{H}_2\text{O}$$ in methanol has $$[\text{Cu}^{2+}] = 1.00$$ mg per 1000 g of methanol. The molarity of $$\text{Cu}^{2+}$$ in this solution is $$Y \times 10^{-5}$$ mol $$\text{L}^{-1}$$. Given that the density of methanol is 0.792 g $$\text{mL}^{-1}$$, Y is

A

1.57

B

5.04

C

1.25

D

3.99