i need a molecular, ionic and net ionic equation for this :
K_3 PO_4 + BaCl_2
The balanced molecular equation.
2K3PO4 + 3BaCl2==>Ba3(PO4)2 + 6KCl
You separate into the ionic equation.
The net ionic equation is
3Ba^2+(aq) + 2PO4^3-(aq) ==>Ba3(PO4)2(s)
To write the molecular, ionic, and net ionic equations for the reaction between K₃PO₄ and BaCl₂, we need to consider the solubility of the compounds involved.
First, let's write the chemical formula for the compounds:
- K₃PO₄: Potassium phosphate
- BaCl₂: Barium chloride
Step 1: Writing the molecular equation
The molecular equation represents the reaction as if all species were in their molecular form:
K₃PO₄ (aq) + BaCl₂ (aq) →
Step 2: Determining the states of reactants and products
Based on their solubility, we can identify the states of the reactants and products:
- K₃PO₄ is an ionic compound and is typically soluble in water, so it remains as an aqueous (aq) solution.
- BaCl₂ is also an ionic compound but is generally soluble in water.
So, both K₃PO₄ and BaCl₂ are written as aqueous solutions (aq).
Step 3: Writing the ionic equation
The ionic equation shows the dissociation of the compounds into their respective ions:
K₃PO₄ (aq) + BaCl₂ (aq) → 3K⁺ (aq) + PO₄³⁻ (aq) + Ba²⁺ (aq) + 2Cl⁻ (aq)
Step 4: Writing the net ionic equation
The net ionic equation shows only the species that undergo a chemical change and excludes the spectator ions (ions that are present but do not participate in the reaction):
In this case, the spectator ions are K⁺ and Cl⁻, since they appear both as reactants and products. The ions that undergo a chemical change are PO₄³⁻ and Ba²⁺:
PO₄³⁻ (aq) + Ba²⁺ (aq) →
Therefore, the net ionic equation for the reaction between K₃PO₄ and BaCl₂ is:
PO₄³⁻ (aq) + Ba²⁺ (aq) →