MnCl3(aq)+K3PO4(aq) complete ionic equation
I have MnCl3 in my textbook as well.
To write the complete ionic equation for the reaction between MnCl3(aq) and K3PO4(aq), we need to first write the balanced molecular equation.
The balanced molecular equation for this reaction is:
3 MnCl3(aq) + 2 K3PO4(aq) → Mn3(PO4)2(s) + 6 KCl(aq)
Now, let's break down the compounds into their respective ions in the solution:
3 Mn^3+(aq) + 6 Cl^-(aq) + 2 K^+(aq) + PO4^3-(aq) → Mn3(PO4)2(s) + 6 K^+(aq) + 6 Cl^-(aq)
Finally, we cancel out the spectator ions (ions that appear on both sides of the equation and don't participate in the chemical reaction):
3 Mn^3+(aq) + 2 PO4^3-(aq) → Mn3(PO4)2(s)
This is the complete ionic equation for the reaction between MnCl3(aq) and K3PO4(aq).
To write the complete ionic equation for the reaction between MnCl3(aq) and K3PO4(aq), we first need to know the chemical formulas and their respective ions of the reactants and products.
The reactants are MnCl3(aq) and K3PO4(aq).
- MnCl3 is a salt composed of manganese (Mn) and chloride (Cl) ions.
- K3PO4 is a salt composed of potassium (K) and phosphate (PO4) ions.
The general guideline for writing the complete ionic equation is to separate the soluble ionic compounds into their respective ions.
Now, let's break down each compound into its ions:
MnCl3(aq):
- MnCl3 dissociates into Mn^3+ and Cl^- ions.
K3PO4(aq):
- K3PO4 dissociates into 3K^+ ions and PO4^3- ions.
Now, let's write the complete ionic equation by showing each ion separately:
Mn^3+ + 3Cl^- + 3K^+ + PO4^3- →
Since all ions on the left side of the equation are balanced with the ions on the right side, there are no spectator ions to remove. So, the complete ionic equation for the given reaction is:
Mn^3+ + 3Cl^- + 3K^+ + PO4^3- → Mn^3+ + PO4^3- + 3K^+ + 3Cl^