Question

I need 500 ml of 0.10 m HCL solution. I have a 3.785 liter container of HCL at 31.45% concentration. How do I acheive my objective?

Answer 1

Is that 31.45% by mass. If so, then the solution is 12.58 m.
31.45 g HCl(31.45 g HCl + 68.55 g H2O) and
31.45/36.46 = 0.8625 moles HCl in 0.06855 kg solvent which makes the solution 12.58%.
Then m x grams soln = m wanted x grams wanted
12.58 m x grams soln = 0.1 m x 500
Solve for grams of the 31.45% solution. This will not give you exactly 500 mL since the density is not known but it should be close.

Answer 2

the solution is 31.45% by weight. I am trying to find out how much of the HCL i use as a base and how much water I need to add to make 500 ml or more at 0.10 m HCL

Answer 3

also the hcl is liquid form.

Answer 4

So you follow the equation I gave above and solve for grams stock solution.

<b>12.58 m x grams soln = 0.1 m x 500
grams soln = 0.1 x 500/12.58 = 3.97 g
</b>
If you know the density you can convert 3.97g to mL. The density of 31% HCl is about 1.16 in my tables. Again, that won't be exactly 500 mL and it won't be exactly 0.1 m but close.

Answer 5

Thank you very much ... extremely helpful and very generous of you to volunteer your time and knowledge for this project.