Question

It is desired to make 1.00 liter of 6.00 M nitric acid from concentrated 16.00 M HNO3.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 (answer to b) is diluted to 1.00 liter, what will be the molarity of the solution?

Answer 1

Answer:

A) 6.00 mol.

B) 0.375 L or 375 mL

C) 6.00 M

Explanation:

Hello,

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

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

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

$V=\frac{6.00mol}{16.00mol/L}=0.375L$

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

$M_1V_1=M_2V_2$

Thus, solving for the final molarity, we obtain:

$M_2=\frac{M_1V_1}{V_2}=\frac{16.00M*0.375L}{1.00L}\\ \\M_2=6.00M$

Regards.