Predict products and balance equations for the reactants shown.
Pb 2+(aq) + H2PO4 1-(aq)--->?
Pb 2+(aq) + HPO4 2-(aq)--->?
Pb 2+(aq) + PO4 3-(aq)---->?
To predict the products and balance the equations for the given reactants, we need to identify the ions and combine them to form the products. Let's analyze each reaction separately:
Reaction 1: Pb 2+(aq) + H2PO4 1-(aq) ---> ?
In this reaction, the Pb2+ ion and the H2PO4 1- ion are combining. To determine the products, we need to consider the charges and combine them accordingly.
The Pb2+ ion has a charge of +2, and the H2PO4 1- ion has a charge of -1. To balance the charges, we need two H2PO4 1- ions to combine with one Pb2+ ion. The resulting products would be:
Pb(H2PO4)2(s)
Now, let's move on to the next reaction:
Reaction 2: Pb 2+(aq) + HPO4 2-(aq) ---> ?
In this reaction, the Pb2+ ion and the HPO4 2- ion are reacting. Similar to the previous case, we need to balance the charges to determine the products.
The Pb2+ ion has a charge of +2, and the HPO4 2- ion has a charge of -2. In this case, only one HPO4 2- ion is needed to balance the charge of the Pb2+ ion. The resulting products would be:
Pb(HPO4)(s)
Lastly, let's analyze the last reaction:
Reaction 3: Pb 2+(aq) + PO4 3-(aq) ---> ?
In this reaction, the Pb2+ ion and the PO4 3- ion are reacting. Again, balancing the charges is crucial.
The Pb2+ ion has a charge of +2, and the PO4 3- ion has a charge of -3. To balance the charges, we need three PO4 3- ions to combine with two Pb2+ ions. The resulting products would be:
Pb3(PO4)2(s)
Keep in mind that the products are represented as solid precipitates (s) since they are insoluble compounds. Additionally, these reactions are written in a simplified ionic equation form, without considering any spectator ions.