What is the molarity of a nitric acid solution prepared by diluting 1.5L of 3.00M HNO3 to a total volume of 2.50L? Is the correct answer 1.8M or do I have to do more???
The answer is 1.8 M but since you didn't show how you obtained that answer I don't know if you need to do more or not.
To determine the molarity of a solution, you need to use the formula:
M1V1 = M2V2
where M1 and V1 are the initial molarity and volume of the concentrated solution, and M2 and V2 are the final molarity and volume of the diluted solution, respectively.
In this case, M1 is 3.00M (the initial molarity of the concentrated nitric acid solution) and V1 is 1.5L (the initial volume). M2 is the unknown we are trying to determine, and V2 is 2.50L (the final volume after dilution).
Using the formula, we can rearrange it to solve for M2:
M2 = (M1 * V1) / V2
Plugging in the values, we get:
M2 = (3.00M * 1.5L) / 2.50L
M2 = 4.50M / 2.50L
M2 = 1.8M
So, the correct answer is indeed 1.8M. Therefore, you do not need to do any further calculations.