Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL.
How much concentrated solution would you take to prepare 3.00L of 0.525M HCl by mixing with water?
Trevor H
Favorite Answer
Calculate the molarity of the concentrated HCl solution:
Take 1.00L of the solution . This has mass = 1000* 1.20 = 1200g
It is 37.0% HCl by mass
Mass of HCl in 1.00L of solution = 37.0/100*1200 = 444g / L
Molar mass HCl = 36.46 g/mol
mol HCl in 444g = 444/36.46 = 12.18 M solution :
Now use the dilution equation:
M1V1 = M2V2
12.18*V1 = 0.525*3000
V1 = 0.525*3000/12.18
V1 = 129 mL of the concentrated HCl solution , diluted to a final volume of 3000mL or 3.0L.
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