CHEM-C 101 Lecture Notes - Lecture 20: Chemical Equation, Barium Chloride, Sodium Sulfate

You will have an opportunity to examine certain precipitation reactions and test the solubility rules shown in the table below. Empirical Rules for the Solubilities of Common Ionic Compounds Soluble Compounds Exceptions None Sodium, potassium, and ammonium compounds Acetates and nitrates Chlorides Sulfates None Lead and silver chlorides are insoluble. Calcium, barium, and lead(II) sulfates are insoluble. Insoluble Compounds Exceptions Carbonates and phosphates Sodium, potassium, and ammonium compounds are soluble. Hydroxides Sodium, potassium, and calcium compounds are soluble. Sodium, potassium, calcium, and ammonium compounds are soluble. Sulfides You will also examine a reaction in which a gas is formed and some reactions of acids

Solution A Solution B Sodium sulfate Barium chloride Sodium chloride 2 Silver nitrate 3 Lead(II) nitrate Potassium iodide 4 Barium chloride Sodium carbonate 5 Sodium hydroxide Ammonium chloride 6 Lead(II) nitrate Sodium sulfide Hydrochloric acid 7 Sodium sulfide 8 Copper(II) sulfate Sodium hydroxide Potassium chromate 9 Lead (II) nitrate Sodium hydroxide 10 ron (III) nitrate Sodium hydroxide 11 Silver nitrate 12 sodium chloride Calcium nitrate

Predict the solubility of the following salts: sodium sulfate potassium chromate silver bromide nickel (II) hydroxide aluminum nitrate barium sulfide ammonium acetate strontium iodide Write the ions that are produced when the following substances dissolve in water: Mg(OH)_2 K_2SO_4 NaHCO_3 (NH_4)_3PO_4 NaCIO Predict whether or not the following reactions will lead to a precipitate Write detailed and net ionic equations for all the reactions. a. potassium chromate and lead acetate b. silver perchlorate and ammonium chloride c. potassium carbonate and copper acetate d. sodium fluoride and magnesium iodide e. barium nitrate and potassium sulfate