According to the label on a bottle of concentrated hydrochloric acid, the contents are 36.0% HCl by mass and have a density of 1.18 g/mL.
What volume of it would you need to prepare 401 mL of 2.60 M HCl?
Given:
Mass% of HCl = 36.0%
Density = 1.18g/mL
The molarity of concentrated HCl:
The concentration on the bottle of HCl pertains to the concentration in percent by mass. If we have 1000 mL of a solution, we can determine the mass of solution as shown.
1000 mL×1.18 g1 mL = 1180 g1000 mL×1.18 g1 mL = 1180 g
Calculating for the mass of solute HCl present,
mass HCl = 0.36×1180 gmass HCl = 424.8 gmass HCl = 0.36×1180 gmass HCl = 424.8 g
Thus, we arrive with the molarity below.
[HCl] = 424.8 g36gmol1 L = 11.8 M
HCl volume you need to prepare 401 mL of 2.60 M HCl:
Using the dilution equation, we get
V1 = C2*V2/C1
= (2.60 M)(401mL)(11.8 M)
= 88.35mL
Thus, we take 88.35 mL of 11.8 M HCl and dilute the solution to 401mL.
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