A 5.0−L sample of a 5.4M NaCl solution is diluted to 70L . What is the molarity of the diluted solution?
How would you set this up and answer it?
To set up and solve this problem, we need to use the concept of molarity and the dilution equation. The dilution equation is given by:
C1V1 = C2V2
where C1 and V1 are the initial concentration and volume, and C2 and V2 are the final concentration and volume.
In this case, the initial concentration (C1) is 5.4 M and the initial volume (V1) is 5.0 L. The final volume (V2) is 70 L. We need to find the final concentration (C2).
Substituting these values into the dilution equation, we have:
5.4 M x 5.0 L = C2 x 70 L
Rearranging the equation, we have:
C2 = (5.4 M x 5.0 L) / 70 L
Simplifying this equation gives us:
C2 = 0.386 M
Therefore, the molarity of the diluted solution is 0.386 M.