Question

question 2 of 30 if a precipitation reaction occurs, what will be the products of the unbalanced reaction shown below? pb(no3)2(aq) + k2(so4)(aq) → solubility table a. pbso4(s) + kno3(s) b. no precipitate will form. c. pbso4(s) + kno3(aq) d. pbso4(aq) + kno3(s)

Explanation:

Step1: Identify the reaction type

This is a double - displacement reaction. In a double - displacement reaction of the form $AB + CD
ightarrow AD+CB$, for $Pb(NO_3)_2(aq)+K_2(SO_4)(aq)$, the cations ($Pb^{2 + }$ and $K^+$) and anions ($NO_3^-$ and $SO_4^{2 - }$) switch partners. So the products are $PbSO_4$ and $KNO_3$.

Step2: Use the solubility rules

According to the solubility table, potassium nitrate ($KNO_3$) is soluble in water and will be in the aqueous state ($KNO_3(aq)$), while lead(II) sulfate ($PbSO_4$) is insoluble in water and will form a precipitate ($PbSO_4(s)$).

Answer:

C. $PbSO_4(s)+KNO_3(aq)$