Question

1. given the reactants, _al₂(so₄)₃(aq) + _pb(s) → predict the unbalanced products. □ _pbso₄(aq) + _al(s) □ _pb(so₄)₂(aq) + _al(s) □ _pb(so₄)₂(s) + _al(s) □ _pbso₄(s) + _al(s)

Explanation:

Step1: Identify reaction type

This is a single - displacement reaction where a more reactive metal (Al) can displace a less reactive metal (Pb) from its salt solution. The sulfate ion ($SO_4^{2 - }$) will combine with the lead ion. Lead has a common oxidation state of +2 in most of its compounds in these types of reactions. The sulfate ion has a charge of - 2. So, the lead sulfate formed will be $PbSO_4$.

Step2: Determine product states

In an aqueous solution reaction, if the product is soluble, it will be in the aqueous (aq) state. Aluminum metal will be in the solid (s) state. Lead sulfate is soluble in water in this context.

Answer:

$PbSO_4(aq)+Al(s)$