If 0.500 L of a 4.00-M solution of copper nitrate, Cu (NO3) 2, is diluted to a volume of 1.50 L by the addition of water, what is the molarity of the diluted solution?

1.33 M

Explanation:

We'll begin by writing out the data obtained from the question. This includes the following:

Volume of the stock solution (V1) = 0.5L

Molarity of the stock solution (M1) = 4M

Volume of diluted solution (V2) = 1.5L

Molarity of the diluted solution (M2) =.?

With the application of the dilution formula, the molarity of the diluted solution can be obtained as follow:

M1V1 = M2V2

4 x 0.5 = M2 x 1.5

Divide both side by 1.5

M2 = (4 x 0.5) / 1.5

M2 = 1.33 M

Therefore the molarity of the diluted solution is 1.33 M