Experiment 12

Experiment Twelve Double Replacement (Ionic) reactions Solubility Rules for Salts and Bases Rule 1. All compounds containing group IA cations (Alkali metals) or the ammonium ion (NH4+) are soluble. Rule 2. All nitrate, acetate and chlorate compounds are soluble. Rule 3. Most sulfate salts are soluble, except the sulfate salts of Pb2+, Ag+, Hg, Ba2+, Sr2+ and Ca2+. Rule 4. Most chlorides, bromides and iodides are soluble except for the compounds of these salts that contain Ag+, Pb2+ and Hg22+, and Cu+ . Rule 5. Most carbonates, sulfites and phosphates are insoluble, except those identified in Rule 1. Rule 6. Most hydroxides are insoluble except those identified in Rule 1, Sr2+ and Ba2+. Rule 7. Most dichromate salts are insoluble except those identified in Rule 1. Procedure Mix 20 drops each of the 2 indicated solutions in a test tube. Agitate the mixture by tapping the bottom of the tube with two fingers and let the mixture sit for one to two minutes. The formation of a precipitate indicates that a reaction has occurred. If a precipitate appears, use the solubility rules to determine which product is the precipitate and specify its color. Write a balanced molecular equation with state symbols, (aq) for soluble substances, (s) for precipitates and solid elements, (l) for liquid substances, and (g) for gaseous substances. In addition to the balanced molecular equation, write a complete ionic equation, and the net ionic equation. If no reaction occurs, write “NO REACTION or NR.” Write all the indicated information in your notebook. Example: Mix and briefly agitate 20 drops of Silver nitrate and potassium dichromate Complete Molecular Equation (CME): Color of precipitate: Ruby red______ 2 AgNO3(aq) + K2Cr2O7(aq) ⎯→ Ag2Cr2O7(s) + 2 KNO3(aq) Complete Ionice Equation (CIE): 2 Ag+(aq) + 2 NO3-‐(aq) + 2 K+(aq) + Cr2O72-‐(aq) ⎯→ Ag2Cr2O7(s) + 2 K+(aq) + 2 NO3-‐(aq) Net ionic equation (NIE): 2 Ag+(aq) + Cr2O72-‐(aq) ⎯→ Ag2Cr2O7(s) Part 1 Mix and briefly agitate 20 drops each of a. Lead(II) nitrate and potassium chromate CME: CIE: NIE: Color of precipitate ________________ b. Lead(II) nitrate and potassium dichromate CME: CIE: NIE: Color of precipitate ________________ c. Lead(II) nitrate and potassium iodide CME: CIE: NIE: d. Barium chloride and potassium chromate CME: CIE: NIE: Color of precipitate ________________ Color of precipitate ________________ Part 2 Mix and briefly agitate 20 drops each of a. Sodium sulfate and barium chloride CME: CIE: NIE: b. Copper(II) sulfate and barium nitrate CME: CIE: NIE: Color of precipitate ________________ Color of precipitate ________________ c. Aluminum sulfate and barium nitrate CME: CIE: NIE: Color of precipitate ________________ Part 3 Mix and briefly agitate 20 drops each of a. Sodium chloride and silver nitrate CME: CIE: NIE: Color of precipitate ________________ b. Potassium bromide and silver nitrate CME: CIE: NIE: c. Potassium bromide and ammonium chloride CME: CIE: NIE: Color of precipitate ________________ d. Sodium iodide and silver nitrate CME: CIE: NIE: Color of precipitate ________________ Color of precipitate ________________ Color of precipitate ________________ Part 4 Mix and briefly agitate 20 drops each of a. Iron(III) chloride and barium hydroxide CME: CIE: NIE: b. Cobalt(II) chloride and barium hydroxide CME: CIE: NIE: Color of precipitate ________________ c. Nickel(II) chloride and sodium hydroxide CME: CIE: NIE: Color of precipitate ________________ d. Copper(II) chloride and sodium hydroxide CME: CIE: NIE: Color of precipitate ________________

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