If 4.0 L of a 4.9 M SrCl2 solution is diluted to 40 L, what is the molarity of the diluted solution?
L x M = L x M
M_1*V_1=M_2*V_2 so,
4.9 M SrCl_2*4.0 L=M_2*40 L then, solve for M_2
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To find the molarity of the diluted solution, we need to use the concept of the dilution formula. The dilution formula is:
M1V1 = M2V2
Where:
M1 = initial molarity of the solution (before dilution)
V1 = initial volume of the solution (before dilution)
M2 = final molarity of the solution (after dilution)
V2 = final volume of the solution (after dilution)
Let's plug in the values given in the question to solve for M2, the final molarity.
M1 = 4.9 M (initial molarity)
V1 = 4.0 L (initial volume)
V2 = 40 L (final volume)
Substituting these values into the dilution formula:
4.9 M x 4.0 L = M2 x 40 L
Now, let's solve for M2.
(4.9 M x 4.0 L) / 40 L = M2
19.6 mol = M2
The molarity of the diluted solution is 19.6 M.