How many liters of each solution do you need to get 3.0 mol of HCl?

a. 12.0 M HCl
b. 2 M HCl
c. 0.5 M HCl
d. 0.010 M HCl

1 Answer
Mar 21, 2018

By definition...#"concentration"="moles of solute"/"volume of solution"#

Explanation:

And so to gets the #"volume"#..we arrange the given quotient..

#"volume of solution"="moles of solute"/"concentration"#

#a.# And so if #3.0*mol# are required from #12.0*mol*L^-1# #HCl#...we take the quotient...

#(3.0*mol)/(12.0*mol*L^-1)=0.250*L# (mind you I don't think you can get #HCl# at this concentration....)

#b.# And if #3.0*mol# are required from #2.0*mol*L^-1# #HCl#...we take the quotient...

#(3.0*mol)/(2.0*mol*L^-1)=1.50*L#

#c.# And if #3.0*mol# are required from #0.5*mol*L^-1# #HCl#...we take the quotient...

#(3.0*mol)/(0.50*mol*L^-1)=6.0*L#

#d.# And if #3.0*mol# are required from #0.010*mol*L^-1# #HCl#...we take the quotient...

#(3.0*mol)/(0.010*mol*L^-1)=300.0*L#

And clearly this last is an impratical proposition....