Commercially available conc. HCl contains 38% mass. Find out the molarity of the solution if density of the solution is 1.19 g/ml. What volume of conc. HCl is required to make 1.00 L of 0.10 M HCl?
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We first calculate the concentration of the conc. acid with respect to mol⋅L−1.
Concentration=Moles of HClVolume of solution
=1⋅mL×1.19⋅g⋅mL−1×38%36.46⋅g⋅mol−11⋅mL×10−3⋅L⋅mL−1=12.40⋅mol⋅L−1
; this is very concentrated hydrochloric acid, and would fume at you. The conc. hydrochloric acid that we habitually use in a lab is approx. 10.5⋅mol⋅L−1.
Now we need 1⋅L×0.10⋅mol⋅L−1=0.10⋅mol
And we take the quotient...
0.10⋅mol12.40⋅mol⋅L−1=8.06×10−3⋅1L−1=8.06×10−3⋅11L
=8.1⋅mL
Hope it helps....
Concentration=Moles of HClVolume of solution
=1⋅mL×1.19⋅g⋅mL−1×38%36.46⋅g⋅mol−11⋅mL×10−3⋅L⋅mL−1=12.40⋅mol⋅L−1
; this is very concentrated hydrochloric acid, and would fume at you. The conc. hydrochloric acid that we habitually use in a lab is approx. 10.5⋅mol⋅L−1.
Now we need 1⋅L×0.10⋅mol⋅L−1=0.10⋅mol
And we take the quotient...
0.10⋅mol12.40⋅mol⋅L−1=8.06×10−3⋅1L−1=8.06×10−3⋅11L
=8.1⋅mL
Hope it helps....
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