Asked by manar
Describe the preparation of 100 ml of 6.0 M HCI from a concentrated solution that has density of 1.18 and is 37 % ( w / w ) HCI ( 36.5 g / mol ) .?
Answers
Answered by
DrBob222
density = 1.18 so 1000 mL of the solution has a mass of 1180 grams. Of that, 37% is HCl so 1180 g x 0.37 = 437 g HCl. How many moles is that? That's 437/36.5 = 11.973 rounds to 12.so the HCl is 12.0 M.
Then mL1 x M1 = mL2 x M2 where 1 stands for the concentration solution of 12.0 M and 2 stands for the
diluted solution of 6.0M.
mL1 x 12.0 = 100 mL x 6.0 M
Solve for mL 1 and I get approximately 50 mL.
Pipet 50,0 mL of the 12.0 M stuff into a 100 mL volumetric flask, add distilled water to the mark on the volumetric flask, stopper, mix thoroughly, label, done.
Then mL1 x M1 = mL2 x M2 where 1 stands for the concentration solution of 12.0 M and 2 stands for the
diluted solution of 6.0M.
mL1 x 12.0 = 100 mL x 6.0 M
Solve for mL 1 and I get approximately 50 mL.
Pipet 50,0 mL of the 12.0 M stuff into a 100 mL volumetric flask, add distilled water to the mark on the volumetric flask, stopper, mix thoroughly, label, done.
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