If 1.0 mL of 6.0M HCl is added to 499 mL of water to give exactly a 500 mL solution, what is the molarity of the dilute solution?
6.00 M x (1.00/500.00) = ?
To find the molarity of the dilute solution, we need to use the equation M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume.
Given:
Initial concentration (M1) = 6.0 M
Initial volume (V1) = 1.0 mL = 0.001 L
Final volume (V2) = 500 mL = 0.5 L
Let's substitute the values into the equation and solve for M2:
M1V1 = M2V2
(6.0 M)(0.001 L) = M2(0.5 L)
M2 = (6.0 M)(0.001 L) / (0.5 L)
M2 = 0.006 M
Therefore, the molarity of the dilute solution is 0.006 M.
To find the molarity of the dilute solution, you need to use the formula:
M1V1 = M2V2
Where:
M1 = initial molarity of the concentrated solution
V1 = initial volume of the concentrated solution
M2 = final molarity of the dilute solution
V2 = final volume of the dilute solution
In this case, the initial solution has a molarity of 6.0 M and a volume of 1.0 mL, while the final solution has a volume of 500 mL (which is the sum of 1.0 mL of concentrated HCl and 499 mL of water). We want to find the final molarity of the dilute solution.
Rearranging the formula, we have:
M2 = (M1 * V1) / V2
Substituting in the values:
M2 = (6.0 M * 1.0 mL) / 500 mL
Simplifying the expression, we have:
M2 = 0.012 M
Therefore, the molarity of the dilute solution is 0.012 M.