what is the final M solution prepared by diluting 5.0 mL of 6.0 M HCl to 60.0 mL
you have diuted it 12 times. 6/12 M
To find the final molarity (M) of the solution prepared by diluting 5.0 mL of 6.0 M HCl to a total volume of 60.0 mL, you can use the equation for dilution:
M1V1 = M2V2
Where:
M1 = initial molarity
V1 = initial volume
M2 = final molarity
V2 = final volume
In this case, we have:
M1 = 6.0 M (initial molarity of HCl)
V1 = 5.0 mL (initial volume of HCl)
M2 = unknown (final molarity of the diluted solution)
V2 = 60.0 mL (final volume of the diluted solution)
Plugging these values into the equation, we get:
(6.0 M)(5.0 mL) = M2(60.0 mL)
Simplifying, we have:
30 = M2(60.0 mL)
Now we can solve for M2 by rearranging the equation:
M2 = 30 / 60.0
Calculating, we find:
M2 ≈ 0.50 M
Therefore, the final molarity of the solution prepared by diluting 5.0 mL of 6.0 M HCl to a total volume of 60.0 mL is approximately 0.50 M.