Consider the following reaction: #Li_2S(aq) + Co(NO_3)_2 (aq) -> 2LiNO_3(aq) + CoS(s)#. What volume of #0.160# #mol*L^-1# #Li_2S#, solution is required to completely react with #0.130# #mol*L^-1# #Co(NO_3)_2#?

1 Answer
May 6, 2018

Answer:

Well the reaction relies on the brick-like solubility of transition-metal sulfides.

Explanation:

We gots...

#Li_2S(aq) + Co(NO_3)_2(aq) rarr CoS(s)darr + 2LiNO_3(aq)#..

Else we could write the net ionic equation:

#Co^(2+) + S^(2-) rarr CoS(s)darr#

And so we gots with respect to #Co^(2+)# #0.130*mol*L^-1#...

#0.130*mol*L^-1xx100*mLxx10^-3*L*mL^-1=0.0130*mol#...the volume of the cobalt ion solution was interpolated.

And given the 1:1 stoichiometry....we take the quotient...

#(0.0130*mol)/(0.160*mol*L^-1)xx1000*mL*L^-1=81.3*mL# of the lithium sulfide solution. Ad please note that I had to interpolate the concentration of lithium sulfide.