If 25.0mL of 0.56 M H2SO4 is diluted to a volume of 125 mL, what is the molarity of the resulting solution?
Use the dilution formula of
c1v1 = c2v2
c = concn
v = volume
i do not understand how to work the problem out.
Can you substitute for c1, c2, v1, and v2 from the problem? Do that, then tell me what you don't understand from there.
To find the molarity of the resulting solution after dilution, we can use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity of the solution
V1 = initial volume of the solution
M2 = final molarity of the solution (what we need to find)
V2 = final volume of the solution
Given:
M1 = 0.56 M (molarity of the initial solution)
V1 = 25.0 mL (initial volume of the solution)
V2 = 125 mL (final volume of the solution)
Now, let's substitute the values into the equation and solve for M2:
(0.56 M) * (25.0 mL) = M2 * (125 mL)
14.0 = M2 * 125
M2 = 14.0 / 125
M2 ≈ 0.112 M
Therefore, the molarity of the resulting solution after dilution is approximately 0.112 M.