please help! I don't understand any of this.
Using the Solubility Rules, write the balanced molecular, total ionic, and net ionic equations (including physical states) for the following:
Hints: There is no such thing as an Na3+. Na is in group 1A, so you know it can only form a +1 charge. It will form 3 Na+ ions for each Na3PO4. There is a diatomic molecule Cl2. But when ionic compounds are dissolved in water, they form ions so the dissociation is to 2 Cl- from the MgCl2.
1. Na3PO4 (aq) + MgCl2 (aq) ->
2. Al(CH3COO)3 (aq) + KOH (aq) ->
molecular equation is
2Na3PO4(aq) + 3MgCl2(aq) ==>Mg3(PO4)2(s) + 6NaCl(aq)
total ionic BUT you add the phases.
6Na^+ + 2PO4^3- + 3Mg^2+ + 6Cl^- ==> Mg3(PO4)2(s) + 6Na^+ + 6 Cl^-
net ionic. cancel those ions that appear on both sides of th equation and you will be left with
2PO4^3-(aq) + 3Mg^2+(aq) ==> Mg3(PO4)2(s)
To write the balanced molecular, total ionic, and net ionic equations for the given reactions, we can follow these steps:
1. Na3PO4 (aq) + MgCl2 (aq) ->
- Identify the ions present in the reactants: Na3PO4 dissociates into Na+ and PO4^3- ions, while MgCl2 dissociates into Mg^2+ and 2 Cl- ions.
- Write the balanced molecular equation by combining the ions:
3 Na+ + PO4^3- + Mg^2+ + 2 Cl- -> Na3PO4 + MgCl2
- Write the total ionic equation by representing the ions individually (aqueous substances are split into their respective ions):
3 Na+ + PO4^3- + Mg^2+ + 2 Cl- -> Na+ + Na+ + Na+ + PO4^3- + Mg^2+ + Cl- + Cl-
- Write the net ionic equation by eliminating the spectator ions (ions that appear on both sides of the equation):
3 Na+ + PO4^3- + Mg^2+ + 2 Cl- -> Na3PO4 + MgCl2
2. Al(CH3COO)3 (aq) + KOH (aq) ->
- Identify the ions present in the reactants: Al(CH3COO)3 dissociates into Al^3+ and 3 CH3COO- ions, while KOH dissociates into K+ and OH- ions.
- Write the balanced molecular equation by combining the ions:
Al^3+ + 3 CH3COO- + K+ + OH- -> Al(CH3COO)3 + KOH
- Write the total ionic equation by representing the ions individually (aqueous substances are split into their respective ions):
Al^3+ + 3 CH3COO- + K+ + OH- -> Al^3+ + 3 CH3COO- + K+ + OH-
- Write the net ionic equation by eliminating the spectator ions (ions that appear on both sides of the equation):
Al^3+ + OH- -> Al(OH)3
Remember to include the physical states (s for solid, l for liquid, g for gas, and aq for aqueous) for each substance in the equation.
Sure! Let's break it down step by step.
1. Na3PO4 (aq) + MgCl2 (aq) ->
To write the balanced molecular equation, we need to identify the ions that form when these compounds dissociate in water.
Na3PO4 dissociates into 3 Na+ ions and 1 PO4^3- ion:
Na3PO4 (aq) -> 3 Na+ (aq) + 1 PO4^3- (aq)
MgCl2 dissociates into 1 Mg^2+ ion and 2 Cl- ions:
MgCl2 (aq) -> 1 Mg^2+ (aq) + 2 Cl- (aq)
Now, we can combine the ions to form the balanced molecular equation:
3 Na+ (aq) + 1 PO4^3- (aq) + 1 Mg^2+ (aq) + 2 Cl- (aq) -> Na3PO4 (aq) + MgCl2 (aq)
Next, let's write the total ionic equation. In the total ionic equation, we write out all the ions that are present in the solution.
The Na+ and Cl- ions are spectator ions, meaning they don't participate in any chemical reaction. We can omit them from the total ionic equation.
Total ionic equation:
3 Na+ (aq) + 1 PO4^3- (aq) + 1 Mg^2+ (aq) + 2 Cl- (aq) -> Na3PO4 (aq) + MgCl2 (aq)
Finally, we can simplify the equation by canceling out the ions that appear on both sides of the equation. This gives us the net ionic equation:
Net ionic equation:
PO4^3- (aq) + Mg^2+ (aq) -> Mg3(PO4)2 (s)
2. Al(CH3COO)3 (aq) + KOH (aq) ->
Using the same process as before, we can write the balanced molecular equation:
Al(CH3COO)3 (aq) + 3 KOH (aq) -> Al(OH)3 (s) + 3 CH3COOK (aq)
Next, let's write the total ionic equation:
Total ionic equation:
Al3+ (aq) + 3 CH3COO- (aq) + 3 K+ (aq) + 3 OH- (aq) -> Al(OH)3 (s) + 3 CH3COOK (aq)
Finally, we can simplify the equation by canceling out the ions that appear on both sides of the equation. This gives us the net ionic equation:
Net ionic equation:
Al3+ (aq) + 3 OH- (aq) -> Al(OH)3 (s)
I hope this explanation helps clarify the process of writing balanced molecular, total ionic, and net ionic equations using solubility rules. If you have any further questions, please feel free to ask!