If 3.0 L of a 5.0 M SrCl_2 solution is diluted to 40 L, what is the molarity of the diluted solution?

To find the molarity (M) of the diluted solution, you can use the formula:

M₁V₁ = M₂V₂

Where:
M₁ = initial molarity of the solution
V₁ = initial volume of the solution
M₂ = final molarity of the solution
V₂ = final volume of the solution

Given:
M₁ = 5.0 M (initial molarity of the solution)
V₁ = 3.0 L (initial volume of the solution)
V₂ = 40 L (final volume of the solution)

Substituting the given values into the formula, we have:

(5.0 M)(3.0 L) = M₂(40 L)

Now, we can solve for M₂ (final molarity of the solution):

(5.0 M)(3.0 L) = M₂(40 L)

15.0 L·M = 40 L·M₂

Divide both sides by 40 L:

(15.0 L·M) / 40 L = M₂

Simplifying the equation, we get:

0.375 M = M₂

Therefore, the molarity of the diluted solution is 0.375 M.