Write the balanced chemical equation for each of these reactions. Include phases. However, when additional aqueous hydroxide is added the precipitate redissolves forming a soluble [Pb(OH)4]2–(aq) complex ion.
Didn't I do this one for you earlier?
To write the balanced chemical equation for this reaction, we first need to identify the reactants and products involved.
Reactants:
1. Lead(II) ion (Pb2+)
2. Hydroxide ion (OH-)
Product:
[Pb(OH)4]2- complex ion
The balanced equation for this reaction can be written as follows:
Pb2+(aq) + 4OH-(aq) → [Pb(OH)4]2-(aq)
In this equation, (aq) represents an aqueous solution, indicating that the ions are dissolved in water. The subscript 2- indicates that the [Pb(OH)4] complex ion carries a -2 charge.
To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation. In this case, there is only one atom of each element on both sides, so the equation is already balanced.