Question

What are the products for the following reactions? Write the molecular equation, total ionic equation, and the net equation.

A) CoCl2+AgNO3—->

B) AgNO3+Na2CO3—>

C) Na2CO3+CuSO4—->

D) BaCl2+CuSO4—>

E) CuSO4+Na3PO4—>

F) Na3PO4+NiCl2—>

What are the phases of each and how can you tell? I am having trouble understanding how you would determine the phases.

Answer 1

In order to determine phases:

Solubility rules:

- Most alkali metal (group I metals) are always soluble

- Cations/Anions such as NH4+, HCO3-; ClO3-, NO3- are always soluble

- Most halides are soluble, F-,Cl-,Br-,I-, exceptions = Ag+, Hg2+2, Pb+2 compounds

- Most sulfates are soluble (SO4-2); exceptions = Ag+, Ca+2, Sr+2, Ba+2, Hg2+2, Pb+2 compounds

- In general (except all alkali metals) these ions will NOT be soluble: PO4-3, CrO4-2, S-2, CO3-2

now.. we know what solids can be formed

all other material islikely to remain i n(aq) solution, tha tis , auqeous

therefore...

A) CoCl2+AgNO3—-> AgCl(s) forms

B) AgNO3+Na2CO3—> Ag2CO3(s)

C) Na2CO3+CuSO4—-> CuCO3(s)

D) BaCl2+CuSO4—> BaSO4(s)

E) CuSO4+Na3PO4—> Cu3(PO4)2

F) Na3PO4+NiCl2—> Ni3(PO4)2

all other materials will remain in ions