Consider the following double displacement reactions.
For each reaction, complete and balance the equation and give the net ionic equation.
NH4Cl(aq)+Ca(NO3)2(aq) -> NH4(NO3)2+CaCl
the second half of the equation is what I had done but I think its not right...
You're right, the correct formula for calcium chloride is CaCl2; however, I don't think there is a reaction between NH4Cl and Ca(NO3)2. I would write
NH4Cl(aq) + Ca(NO3)2(aq) ==> No reaction.
To balance the equation, let's start by writing out the chemical formulas of each compound:
NH4Cl(aq) + Ca(NO3)2(aq) → NH4(NO3)2 + CaCl2(s)
Now, let's balance the equation by ensuring that the number of atoms of each element is the same on both sides:
2 NH4Cl(aq) + Ca(NO3)2(aq) → 2 NH4(NO3)2 + CaCl2(s)
To write the net ionic equation, we need to determine which ions are present both as reactants and products.
The net ionic equation considers only the ions that undergo a change during the reaction. In this case, the "spectator ions" (ions that do not participate in the reaction) are NH4+ and NO3- ions. They remain in solution and do not undergo any change.
The net ionic equation for this reaction is:
2 Cl-(aq) + Ca2+(aq) → CaCl2(s)
Please note that NH4+ and NO3- ions are not included in the net ionic equation because they are spectator ions.
To complete and balance the equation, you need to ensure that the number of atoms of each element is the same on both sides of the equation. Let's complete and balance the equation step by step:
Step 1: Write the cation and anion components separately.
NH4Cl(aq) + Ca(NO3)2(aq) -> _____ + _____
Step 2: Identify the possible double displacement products by swapping the cation and anion components.
Possible products: NH4NO3 and CaCl2
Step 3: Write the complete and balanced equation using the correct formulas for the products.
NH4Cl(aq) + Ca(NO3)2(aq) -> NH4NO3(aq) + CaCl2(aq)
Step 4: Check if the equation is balanced. Count the number of atoms for each element on both sides of the equation.
On the left side: 1 N, 4 H, 2 Cl, 1 Ca, 2 O
On the right side: 1 N, 3 H, 2 Cl, 1 Ca, 2 O
The Cl and H atoms are not balanced. Let's balance them.
Step 5: Balance the Cl atoms by placing the coefficient 2 in front of CaCl2.
NH4Cl(aq) + Ca(NO3)2(aq) -> NH4NO3(aq) + 2 CaCl2(aq)
Step 6: Balance the H atoms by placing the coefficient 2 in front of NH4NO3.
2 NH4Cl(aq) + Ca(NO3)2(aq) -> 2 NH4NO3(aq) + 2 CaCl2(aq)
Now, let's write the net ionic equation. The net ionic equation only includes the species that undergo a chemical change.
Step 7: Convert the complete balanced equation into the net ionic equation.
To do this, you need to determine which ions are soluble and which form precipitates. You can use a solubility table to determine the solubility of the compounds.
Using the solubility rules:
NH4Cl and CaCl2 are soluble in water.
NH4NO3 is soluble in water.
Ca(NO3)2 is soluble in water.
Therefore, all the compounds are soluble and do not form precipitates. In this case, the net ionic equation will be the same as the complete ionic equation.
The net ionic equation is:
2 NH4+(aq) + 2 Cl-(aq) + Ca2+(aq) + 2 NO3-(aq) -> 2 NH4+(aq) + 2 NO3-(aq) + Ca2+(aq) + 2 Cl-(aq)
Note: The net ionic equation shows the ions that participate in the reaction, excluding spectator ions (ions that do not undergo a chemical change).