Question

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

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.

Homework Answers

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

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