Silver Nitrate Reaction

Conclusions
The experiment contained six ionic aqueous compounds that reacted and formed new products. The reactants were barium chloride, potassium nitrate, silver nitrate, sodium carbonate, calcium sulfate, and sodium phosphate. In Station 1, barium chloride and potassium nitrate did not react. Barium chloride and silver nitrate created aqueous barium nitrate and the precipitate silver chloride. In Station 2, potassium nitrate and silver nitrate did not react. Potassium nitrate and calcium sulfate did not react as well. In Station 3, sodium carbonate and calcium sulfate created aqueous sodium sulfate and the precipitate calcium carbonate. Sodium carbonate and potassium nitrate did not react. In Station 4, sodium phosphate and silver nitrate

The solubility rules determined whether a compound would form a precipitate or not. These rules have stated that some compounds such as acetates, nitrates, and iodides are soluble. Similarly, compounds such as carbonates, phosphates, and sulfides have been stated as insoluble. These rules helped to predict the products of the new compounds that were created. The reactions that took place were are double replacement reactions. Each reaction was composed of two compounds as the reactants and two compounds as the products. The metal in each of the reactants bonded with the opposite compound’s nonmetal and created a new product. For example, barium chloride and silver nitrate reacted and yielded barium nitrate and silver chloride. The ionic salt products could be dissolved in water. When this occurred, H20 weakened the bond between the ions and surrounds the two ions individually because of an attraction to create a solution. The dipolar forces of water surrounded the separated ions and kept them in solution which was a manifestation of intermolecular forces. The dipole of water interacted with the dipole of the salt, due to the anion and cation composing the salt, and divided into detached