An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. Identify the solid in the balanced equation. A) (NH4 )2 SO4 B) Pb(NO3 )2 C) PbSO4 D) NH4 NO3 E) There is no solid formed when the two solutions are mixed. ____ 11. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride.
Experiment 6: Physical & Chemical Properties Title and Identifiers: Heating of chemical properties 01/23/15 Purpose / Objective: • To investigate the chemical properties of pure chemical substances • To investigate the physical properties of pure chemical substances Procedural Outline: • Matches • Beaker, 100 mL, glass • Burner-fuel • Goggles-Safety • Stirring rod - Glass • Test Tube(5), 13 x 100 mm in Bubble Bag • Test-tube-clamp-holder • Test-tube-cleaning-brush • Well-Plate-24 • Well-Plate-96 • Litmus Paper, Blue • Litmus paper, Red • Copper (II) Carbonate in Vial, 1/2 Full • Copper (II) Nitrate Crystals in Vial • Copper Metal
Zinc ion and Iodine-iodide-triodide ion in water: It was a liquid solution in a bottle, it was very dark orange-brown color. Solid Zinc Iodide: A very white powdery substance that had several clumps within it. It was also very dry in nature. Mass Table Substance Amount of Mass Measured for Actual Mass Granular Zinc 2.0 grams 1.9 grams Iodine Crystals 2.0 grams 2.1 grams Observation of Reaction Shown below and Included within the lab notes on pages 12 and on page 14. Placing Acetic Acid in Zinc and Iodine test tube After placing the Acetic Acid in a normally unreactive test tube containing Zinc and Iodine, the solution changed to a more orange and then to a more red-brown color.
Contents Abstract – Page 2 Summary of Results – Page 3 Focus Question – Page 5,6 What if… - Page 6 Confidence Report – Page 7,8 Abstract Summary of Results Observations of Reactions – Trials 1 , 2 & 3 | Dissolving Barium Iodide and Zinc Sulfate in deionized water | As the substances dissolve the water becomes cloudy and acquired a white tint. | Centrifuging up the solution obtained in previous reaction | The precipitate and the liquid seperated, and there was more precipitate in one of the test tubes. The precipitate was a thick white color, not transparent. | Heating the Precipitate in a boiling tube containing 2 boiling chips | The mixture began producing a large amount of bubbles, as we continued heating it only white powder remained. | Observations of Chemicals | Zinc Sulfate | Powder of a white solid | Barium Iodide | Powder of a white solid.
We resulted that lead, silver, and copper are the strongest oxidizing agents, and that magnesium and zinc are the weak oxidizing agents. The strong oxidizing agent oxidized the weak oxidizing agent and in turn the strong oxidizing agent got reduced while oxidizing the weak agent. When a reaction occurred, the solid metal reduced the ion, and in turn made it the more reactive metal. In part two we used a solvent extraction technique to derive an activity series for the halogens. With the use of this technique we placed chlorine, bromine, and iodine into solutions containing chloride, bromide, and iodide.
____ HCl + ____Ba(OH)2 ( ____ BaCl2 + ____ H2O 12. ____ Na + ____ O2 ( ____ Na2O 13. ____KClO3 ( ____ KCl + ____ O2 14. ____ Al + ____O2 ( ____ Al2O3 15. ____ Al + ____ CuCl2 ( ____ Cu + ____
Kumari Biswas Chem 106 – 07 October 06, 2014 Menglu Shi Group member: Shemeika McLaren, Jose Suarez, Colleen Shum Lab 3: Redox Arena Redox Arena Lab Part I Observations and Data Observations of starting materials and standards Chemicals | Observations | The Four standards | Granular zinc | Silver-gray irregular solids | Iodine crystals | Purple-black spherical solids, strong smell | Zinc ion and iodine-iodide-triiodide ion in H2O | Red brown liquid | Zinc iodide | Gray white solid powder | Chemicals used for tests | 0.17 M acetic acid | Clear liquid | Mineral oil | Thick clear liquid | Silver nitrate (AgNO3) | Clear liquid | Magnesium turnings | Solid curled metals | 3 M HCl | Clear liquid | Other chemicals
Abstract The purpose of the experiment was to identify unknown ionic compound #. After many tests, the unknown was identified as sodium chloride. The cation (Na+) was determined by having a yellow/orange color flame test. The anion (Cl-) was determined by the chloride anion test when the unknown test solution showed a positive test for chloride. The synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride.
The well that contained NaCl turned white, NaBr turned yellowish, and NaI turned green. When calcium was dropped into the beaker, the water turned purple as Ca moved around quickly on the surface of the water releasing smoke. When potassium was dropped into the beaker, it created a ball of fire and shot around the beaker quickly, releasing smoke and turning the water purple. Questions Most, if not all, elements in the families reacted similarly to those in the same family. The metallic elements in this experiment support that they form acidic oxides.
Jose Flores 6th period 1-27-14 LAB REPORT Introduction: A substance can conduct an electrical current if it is made of positively charged and negatively charged particles that are free to move about and is called a conductor. The purpose is to figure out conductivity of substances and to check which one conducts electricity. The hypothesis is that sucrose would be the only one that could not conduct out of the other six solutions. Materials: The materials used in this lab where six solutions , napkins, 2 pairs of gloves, 2 cups (1 cup with distilled water and 1 cup with solid NaCI) and a conductivity meter. The six solutions are sodium chloride, hydrochloric acid, sodium hydroxide, acetic acid, ammonia and sucrose.