Answer
a. No reaction.
b. $2 NaCl(aq) + Hg_2(C_2H_3O_2)_2(aq) \longrightarrow 2 NaC_2H_3O_2(aq) + Hg_2Cl_2(s)$
c. $(NH_4)_2SO_4(aq) + SrCl_2(aq) \longrightarrow 2 NH_4Cl(aq) + SrSO_4(s)$
d. $NH_4Cl(aq) + AgNO_3(aq) \longrightarrow AgCl(s) + NH_4NO_3(aq)$
Work Step by Step
1. Determine the resulting ionic compounds by switching the anions (or cations):
a. $NaCl$ and $KNO_3$
b. $NaC_2H_3O_2$ and $Hg_2Cl_2$
c. $NH_4Cl$ and $SrSO_4$
d. $NH_4NO_3$ and $AgCl$
2. Determine if they are soluble or insoluble.
a. Both are soluble.
b. $Hg_2Cl_2$ is insoluble.
c. $SrSO_4$ is insoluble.
d. $AgCl$ is insoluble.
3. If both compounds are soluble, there will be no reaction. If some are insoluble, there will occur their precipitation. Do not forget to balance the reaction.
a. No reaction.
b. $2 NaCl(aq) + Hg_2(C_2H_3O_2)_2(aq) \longrightarrow 2 NaC_2H_3O_2(aq) + Hg_2Cl_2(s)$
c. $(NH_4)_2SO_4(aq) + SrCl_2(aq) \longrightarrow 2 NH_4Cl(aq) + SrSO_4(s)$
d. $NH_4Cl(aq) + AgNO_3(aq) \longrightarrow AgCl(s) + NH_4NO_3(aq)$
