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 3.05 L of 0.545 M HCl by mixing with water?
Let the volume of solution be 100 ml
D = M / V
1.2 = M / 100
M = 120 g
37% HCl will be (37 x 120) / 100 = 44.4 g
Number of moles of HCl = 44.4 / 36.5 = 1.22
Molarity = no. of moles / volume of solution in litre
M = 1.22 / 0.100
M = 12.2 M
Now using the formula
M1 V1 = M2 V2
12.2 x V1 = 0.545 x 3.05
V1 = 0.13625 L
or 136.25 mL
Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and...
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