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.