Making 6.00 M Nitric Acid Solution

A) How many moles of nitric acid are in 1.00 L of 6.00 M nitric acid?

B) What volume of concentrated 16.00 M nitric acid will contain this number of moles?

C) If this volume of concentrated nitric acid is diluted to 1.00 liter, what will be the molarity of the solution?

Explanation:

Hello,

A) In this case, from the definition of molarity, we compute the moles for the given volume and concentration:

n = M * V = 1.00 L * 6.00 mol/L = 6.00 mol

B) In this case, from the stock solution, the required volume is:

V = 6.00 mol / 16.00 mol/L = 0.375 L

C) In this case, we apply the following formula for the dilution process:

M1V1 = M2V2

Thus, solving for the final molarity, we obtain:

M2 = (16.00 M * 0.375 L) / 1.00 L = 6.00 M

Regards.