Question

Nitric acid is commercially available at a concentration of 15.9 M. What volume of this solution must be diluted to a final volume of 1.00 L to prepare a 4.00 M solution?

Answer 1

Answer:

V1= 0.252 L

Step-by-step explanation:

Let V be the volume of the 15.9 M nitric acid solution that needs to be diluted.

According to the dilution formula, the moles of solute before and after dilution are equal. Therefore, we can write:

M1V1 = M2V2

where M1 is the initial concentration (15.9 M), V1 is the initial volume (unknown), M2 is the final concentration (4.00 M), and V2 is the final volume (1.00 L).

Solving for V1, we get:

V1 = (M2V2)/M1
= (4.00 M)(1.00 L)/(15.9 M)
= 0.252 L or 252 mL (rounded to three significant figures)

Therefore, 252 mL of the 15.9 M nitric acid solution must be diluted to a final volume of 1.00 L to prepare a 4.00 M solution.