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What volume of concentrated hydrochloric acid (12.0 M #HCl#) is require to make 2.0 liters of a 3.0 M #HCl# solution?

Answer 1

#500*mL# of #12.0*mol*L^-1# #HCl*(aq)# are required.

The product #C_1V_1# is #"concentration"xx"volume"#, and when we multiply the typical units we get #mol*cancel(L^-1)xxcancelL#, i.e. units of #"moles"# as required.

Anyway, as to your problem, #C_1V_1=C_2V_2#, because both sides have the units of moles.

#V_1=(C_2V_2)/C_1=(3.0*mol*L^-1xx2.0*L)/(12.0*mol*L^-1)#

#=1/2*L#

Note that we typically buy conc. #HCl# as a #32%(w/w)# solution, and this is about #10*mol*L^-1#. This question was not well proposed.

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Answer 2

Olivia Anton

To make 2.0 liters of a 3.0 M HCl solution, you would need 0.5 liters of concentrated hydrochloric acid (12.0 M HCl).

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.