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.
Observing Changes – Materials & Procedures Materials Water Copper (II) sulphate (Powder) Copper (II) sulphate solution Iron nail Sodium carbonate Hydrochloric acid Magnesium ribbon Flame (candle) Sugar Aluminum foil Test tubes Test tube rack Tongs Medicine dropper Spoons Beakers Safety goggles Scoopulas Procedures Water and Copper (II) Sulphate Procedure 1. Add a small amount of solid copper (II) sulphate to a test tube with a scoopula. Record the physical properties. 2. Write a hypothesis on what you think will happen when water is added.
The Cover Sheet to the Confidence Report South Street Seaweed Seaport Tabulated test Results Name of Test Requirements Result Test for Iodine If the mineral oil turns a shade of purple (either dark, or light such as pink), then the Tincture is positive for iodine. The solution became light lavender/pink. This shows that the tincture is positive for iodine. Test for Iodide ion A few things can happen: 1) A white precipitate only, indicating chloride ion is present predominantly (Na Cl in salt water). 2) A yellow precipitate only, indicating iodide ion is present predominantly.
NaHCO3 (sodium bicarbonate - baking soda) and HCl (hydrochloric acid). The bubbles formed are carbon dioxide. HCl (hydrochloric acid) and BTB (bromothymol blue). Bromothymol blue is one of many acid-base indicators. What color do you observe?
During the electrolysis, a gray solid formed on the negative wire of the battery and the dark red solution formed at the positive wire of the batter. Account for this in terms of the positive and negative ions. Iodide ions have the symbol I-, indicating they are negatively charged, which cause them to be attracted to be something with a positive charge, which is why there was a red-brown solution at the positive end. Zinc ions have the symbol Zn2+, indicating a postive charge, which cause them to be attracted to something with a negative charge, which is why a grayish solid formed at the negative wire. 3.
(2 points) Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) 2. Determine the partial pressure of the hydrogen gas collected in the gas collection tube. (3 points) partial pressure H2 = total pressure - vapor pressure of water = 746mmHg - 19.8mmHg = 726mmHg 3. Calculate the moles of hydrogen gas collected. (4 points) n = 125 4.
Results APPEARANCES OF MATERIALS USED Substance Physical Appearance Zinc Carbonate White; powderish Calcium Hydroxide White; powderish; like zinc carbonate 3 M HCL Clear liquid, resembles water 20 mesh granular zinc Grey, metallic, shiny 3% hydrogen peroxide Clear liquid; resembles water Manganese dioxide Very dark grey, black and powdery Copper sulfate Blue, crystalline in structure. Sky blue Zinc iodide Very dark purple, shiny and crystalline in structure 0.1 M acetic acid Clear liquid, resembles water Zinc oxide Very white powdery substance RAW RESULTS Data Specifided (Page 112 CRC handbook) Raw data Volume of Gas Collection Bottle (Average of 3 Trials) 14.04mL Mass of boiling tube (empty) 41.57g Mass of boiling tube with zinc carbonate 43.42g Mass of zinc carbonate 1.75g Volume of water in gas collection bottle after reaction 78.5mL Volume of gas product collected 185.2mL Mass of solid product with boiling tube after reaction 1.11g QUALITATIVE TEST RESULTS Group # Test Observation: Standard Positive/Negative Observation: Experimental Positive/Negative 1 H2 HCL + Zinc bubbling + flaming stick POP! + + flaming splint no POP - 2 CO2 Turned cloudy + Negated from experiment Negated from experiment 3 O2 MgO2 + Hydrogen Peroxide bubbling. Glow stick re-ignited + + wooden splint; glowing stick went out - 4 H2) Added 1 pea size CuSulfate + 1 drop of deionized water; blue, positive + Copper sulfate did not change color when put into wet filter paper - 5 Zn (OH)2 Zinc iodide + 3mL H2O Clear suspension + Visual inspection; cloudy. Acid test= solid + 3M Acetic acid cloudy + 6 ZnO ZnO + Heat yellow Zn Cooled White + ZnCO3 + heat yellow solid.
Use a calorimeter to measure the temperature change in each of three reactions. Calculate the heat of reaction, ∆H, for the three reactions. Use the results to confirm Hess’s law. Ev al Figure 1 ua tio Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) → H2O(l) + Na+(aq) + Cl–(aq) ∆H3 = ? n (3) Solutions of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride.
Measuring Cylinder (1) f. Beaker (1) Results Table: Name of Compound | Observe atomic admission | Calcium Chloride CaCl2 | The flames turned into an orangey color then gradually turned redish brown with a bit of orange. | Barium Chloride BcCl2 | The flames turned into yellowish color then it became whitish and brownish and eventually turning green. | Magnesium ChlorideMgCl2 | The metal salt bubbled when it hit the flames then its flames turned orange and yellow. And the substance that is left on the spatula turned into a glue like white mask. | Nickel ChlorideNiC12 | The substance was green originally but turned yellow after being exposed to the flames.
-Repeat above steps (middle section) for all metallic salts (five total). -Record your observations for the flame color produced by each metallic salt in the Data Table. Qualitative Data- Compound Element Wavelength (nm) Wavelength (m) ΔE (J) KCL 650 6.5 x 10^11 3.07 E-28 Copper Chloride 490 4.9 x 10^11 4.08 E-28 SrCl2 650 6.5 x 10^11 3.07 E-28 CaCl2 600 6.0 x 10^11 3.33 E-28 Lithium 400 4.0 x 10^11 5.00 E-28 Sodium Chloride 600 6.0 x 10^11 3.33 E-28 Wavelength: KCL = 650 Copper Chloride = 490 SrCl2 = 650 Cacl2 =