How many mL of 13.00 M nitric acid must be diluted with water to prepare?

Question

1.60 L
of a 0.140 M HNO3 solution?

Answer 1

17.23 mL of 13M nitric acid

13M * x = 1.6 L * .140M
x=0.01723 L = 17.23 mL

Answer 2

If you can't remember the formula M1V1 = M2V2, you can still figure this out because it follows a very logical path. All you need to really know is (1) how many moles of HNO3 is in 1.60 liters of 0.14 M HNO3 and (2) hom many liters of 13 M HNO3 has that same number of moles. To get the moles of solute, you always multiply molarity by volume.

So, the number of moles of HNO3 in 1.60 liters of 0.14 M HNO3 is equal to 1.6 L x 0.14 mol/L. The result is 0.224 moles.

So, how many liters of 13 M (mol/liter) do we need to equal this? Well, since the mass of solute equals the concentration times the volume, then the volume is equal to the mass divided by the concentration. V = 0.224 mol / 13 mol/liter = 0.0172 liters, or 17.2 ml.

Answer 3

Diluted answer is composed of: 0.440 [mol/L] * a million.20 [L] = 0.528 mol HCl even though if, the style of moles of HCl does not substitute, so the unique answer has an identical 0.528 mol HCl 0.528 [mol] / 13.00 [mol/L] = 0.040615 L = 40.sixty two mL

Answer 4

13M HNO3 is nothing but 0.819g/ml of HNO3.

we require 14.11g of HNO3 in 1600ml to prepare 0.14M HNO3.

Which is nothing but 17.23 ml of HNO3.