Question

11. Each of the following reactions results in one water-soluble product, and one solid precipitate. Complete and balance each reaction, and show phases is or ag) to indicate whether the products are aqueous or solid KCI) Pb(NO hal KOH(aq) + FeCl, (aq) → Bacl, (aq) + K,PO. (aq) → 14. Predict the products (based on the type of chemical reaction) and balance each chemical reaction equation AgC,H,O, (aq) + NaCl(aq) → Na (s) + Cl, (g) → HCl(aq) + Ba(OH)2 (aq) → CuHz () + O2(g) → Solubility Rules Compounds containing these ions are always soluble Alkali metals: LI', Na, K, Rb* Ammonium: NH4* Large -1 oxyanions NO,, CIOs, CIOs, CyH2O2 Compounds containing these ions are usually soluble Halides: F, CIF, Br, (except Pb, Ag*) Sulfate SO (except Ba?, Cap, Pb?, Ag") Not Soluble Most other ions

Answer 1

11. KCl (aq) + Pb(NO3)2 (aq)  $\rightarrow$ PbCl2 (s) + KNO3 (aq)

The reaction between Potassium chloride (KCl) and Lead nitrate (Pb(NO3)2) results in the formation of the solid precipitate of Lead chloride (PbCl2) and aqueous Potassium nitrate (KNO3).

KOH (aq) + FeCl3 (aq)  $\rightarrow$ Fe(OH)3 (s) + KCl (aq)

The reaction between Potassium hydroxide (KOH) and Ferric chloride (FeCl3) results in the formation of the solid precipitate of Ferric hydroxide (Fe(OH)3) and aqueous Potassium chloride (KCl).

BaCl2 (aq) + K3PO4 (aq)  $\rightarrow$ Ba3(PO4)2 (s) + KCl (aq)

The reaction between Barium chloride (BaCl2) and Potassium phosphate (K3PO4) results in the formation of the solid precipitate of Barium phosphate (Ba3(PO4)2) and aqueous Potassium chloride (KCl).

These are the required precipitation reactions along with the states of reactants and products. The formation of a specific precipitate depends on the ions present in the reactants.