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

1 Answer
Jan 17, 2017

Answer:

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

Explanation:

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.