Questions: Refer to the following incomplete precipitation reaction: Ni2(SO3)3(aq) + (NH4)3PO4(aq) → a. For the reaction above, provide the balanced molecular equation. Be sure to include states of matter and show all work.

Refer to the following incomplete precipitation reaction:
Ni2(SO3)3(aq) + (NH4)3PO4(aq) →
a. For the reaction above, provide the balanced molecular equation. Be sure to include states of matter and show all work.

Transcript text: Refer to the following incomplete precipitation reaction: $\mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}(a q)+\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(a q) \rightarrow$ a. For the reaction above, provide the balanced molecular equation. Be sure to include states of matter and show all work.

Solution

Solution Steps

Step 1: Identify the Reactants and Products

The given reaction involves nickel(III) sulfite, $\mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}$, and ammonium phosphate, $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$. These reactants are in aqueous form, as indicated by the (aq) state. The reaction is a precipitation reaction, which typically results in the formation of an insoluble solid (precipitate) and possibly other soluble products.

Step 2: Determine the Possible Products

In a precipitation reaction, the cations and anions from the reactants exchange partners. The possible products are nickel(III) phosphate, $\mathrm{NiPO}_{4}$, and ammonium sulfite, $\mathrm{(NH}_{4})_{2}\mathrm{SO}_{3}$.

Step 3: Write the Unbalanced Molecular Equation

The unbalanced molecular equation for the reaction is: \[ \mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}(aq) + \left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(aq) \rightarrow \mathrm{NiPO}_{4}(s) + \mathrm{(NH}_{4})_{2}\mathrm{SO}_{3}(aq) \]

Step 4: Balance the Chemical Equation

To balance the equation, ensure that the number of each type of atom is the same on both sides of the equation.

Nickel (Ni): There are 2 Ni atoms in $\mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}$, so we need 2 $\mathrm{NiPO}_{4}$ on the product side.
Sulfite (SO$_3$): There are 3 SO$_3$ groups in $\mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}$, so we need 3 $\mathrm{(NH}_{4})_{2}\mathrm{SO}_{3}$ on the product side.
Ammonium (NH$_4$): There are 3 NH$_4$ groups in $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$, so we need 2 $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$ on the reactant side to balance with 3 $\mathrm{(NH}_{4})_{2}\mathrm{SO}_{3}$.

The balanced equation is: \[ \mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}(aq) + 2\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(aq) \rightarrow 2\mathrm{NiPO}_{4}(s) + 3\mathrm{(NH}_{4})_{2}\mathrm{SO}_{3}(aq) \]

Final Answer

The balanced molecular equation for the reaction is: \[ \boxed{\mathrm{Ni}_{2}\left(\mathrm{SO}_{3}\right)_{3}(aq) + 2\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(aq) \rightarrow 2\mathrm{NiPO}_{4}(s) + 3\mathrm{(NH}_{4})_{2}\mathrm{SO}_{3}(aq)} \]

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