How to dilute 2.00mol of hydrochloric acid to 0.02mol?

Question

The acid is too concentrated to use in a titration.

Answer 1

You want a solution which is

0.02 / 2.00 = 0.01 = 1/100 th of the original

Dilute 1.00 mL of the 2.00 M solution to 100 mL in a volumetric flask using pure water for the dilution.

Answer 2

assuming this is mass by volume molar solution. 2.0m HCL would be two moles of HCL per Liter of water. add 1 gram of 2m HCL to 100mL in a vol flask. This is the only way to do it you cannot add 1mL to 100mL because the HCL was made from a solid and most likely a m/v molar solution. This molarity would not be the same if you changed from m/v to mass by mass or volume by volume

Make sure you use DI water. Also must be CO2 free because this will affect the pH pushing back the dissociation of HCL

Answer 3

hello! Using the formula M1 x L1 = M2 x L2... "M" is Molarity (moles/liter) and "L" is Liters....So 2 x 1 = .02 x L2. L2 will be 100L. Take 1 Liter of 2 Molar HCl and add water until 100 liters. You can chance L1 to a smaller quantity if you need less of .02 M concentration....

Answer 4

here is the formula to calculate this and other dilution:

C1*V1 = C2*V2
where C1 = the concentration of solution u have now(in your case 2.00mol)
V1= volume of solution u have
C2= the NEW concentration you want to make(in this case 0.02mol)
and V2= volume of that NEW concentration needed.

So if you had to make 10ml(V2) of 0.02mol HCl(C2) the volume of 2.00mol (V1)will be:

V1= (C2*V2)/C1
V1 = (0.02*10)/2 = 0.1ml

What that means is that you need 0.1ml of 2.0mol of HCl and you add 9.9ml of Distilled water.

So when ever you get information like this all you have to do is plug in the values
Hope this help.

Answer 5

dilute 2.00mol acid in 100mol water.

Answer 6

don't they do that sort of thing in school these day's...pay attention in class next time..