Solutions of #Li_2CO_3# and #MgCl_2# are mixed. a) What is the formula of the precipitate that forms? b) Write the equation for the reaction. c) Write the equation in ionic form. d) What is the net ionic equation of the reaction?

1 Answer
Apr 27, 2017

Answer:

See details below...

Explanation:

a) Since you are combining #Mg^(2+)# ions and #CO_3^(2-)# ions, a precipitate of the slightly soluble salt #MgCO_3# will form.

b) #Li_2CO_3(aq)+MgCl_2(aq) rarr 2 LiCl(aq) + MgCO_3(s)darr#

c) #2 Li^+(aq) + CO_3^(2-)(aq)+Mg^(2+)(aq) + 2Cl^-##(aq) rarr 2 Li^+(aq) + 2 Cl^-##(aq) + MgCO_3(s)darr#

d) Since they do not participate in any reaction, #Li^+# and #Cl^-# are referred to as spectator ions.

e) #Mg^(2+)(aq) + CO_3^(2-)(aq) rarr MgCO_3(s)darr#

Hopefully that covers it!