How many ml of concentrated nitric acid (hno3, 16.0 m) should be diluted with water in order to make 2.00 l of 2.00 m solution?

Taking into account the definition of dilution, 250 mL of concentrated nitric acid 16 M should be diluted with water in order to make 2.00 L of 2.00 M solution.

Dilution is the process of reducing the concentration of solute in solution, which is accomplished by simply adding more solvent to the solution at the same amount of solute.

In a dilution the amount of solute does not change, but as more solvent is added, the concentration of the solute decreases, as the volume (and weight) of the solution increases.

A dilution is mathematically expressed as:

Ci×Vi = Cf×Vf

where

In this case, you know:

Replacing:

16 M× Vi= 2 M× 2 L

Solving:

Vi= 0.25 L= 250 mL (being 1 L= 1000 mL)

In summary, 250 mL of concentrated nitric acid 16 M should be diluted with water in order to make 2.00 L of 2.00 M solution.

Learn more about dilution:

250 ml

Explanation:

According to the dilution law,

where,

= molarity of stock solution = 16 M

= volume of stock solution = ?

= molarity of diluted solution = 2.00 M

= volume of diluted solution = 2.00 L

     (Conversion factor: 1L=1000ml)

Therefore, 250 ml of concentrated nitric acid should be diluted with water.

it would be a gas formation

4d^55s^1 ( third choice)