Question

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`?

Answer 1

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.