The reaction that occurred with this step was displacement and metathesis in the form of gas formation. The balanced equation of this step looks as follows: CuSO4aq+Zns→Cus+ZnSO4(aq) Once this step was finished, the remaining copper was retrieved. First, to recover the copper HCl was added to remove all the zinc. When this happened, a yellow tint was observed in the liquid, as well as bubbling as the zinc was broken down. Once the copper dried out, it was weighed and came to a total of 240 mg.
What are the identities of the substances found after electrolysis and heating? The identities of the substances found were Iodine, Iodide ion (I-), Triodide ion(I3-), Zinc metal and Zinc ion(Zn2+) Post Lab questions: 1. What did this experiment convincingly show about the composition of the white solid? I put that the experiment showed us the white substance was comprised of Zinc ions and iodide ions, and that the two ions and be separated back into their respective elements 2. 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.
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.
Halides Lab: Background information: Halide ions are reactive and useful. Salts are positively charged ions (metals) combined with any negative ions (nonmetal), and when placed in a solution (water) it separates into the cations and anions that made it up. The Purpose of this lab is to find out how the Halides react with the indicators, and to determine the identity of the two unknown solutions (A and B). Color of solutions prior to experiment: NaF | NaCI | KBr | KI | Unknown A | Unknown B | clear | clear | clear | clear | clear | clear | Color of indicator prior to experiment: 5% Bleach (NaOCI) | 0.2 M Na2S2O3 | 0.1 M AgNO3 | 0.5 M Ca(NO3)2 | clear | clear | clear | clear | Halide solutions | NaF | NaCI | KBr | KI | unknown A | unknown B | Test 1: Ca(NO3)2 | Cloudy White (Nothing) | Clear | Nothing | light yellow (Nothing) | Nothing | Nothing | Test 2, Part A: AgNO3 | clear (Nothing) | Milky White | Gold (Cloudy yellow) | milky green (Cloudy yellow) | turned white, film developed on top layer | Milky | Test 2, Part B: add Na2S2O3 to test tube from part A | Dark Orange/brown | Clear | Dark Gold(precipitate yellow then clear) | milky green (no change) | white precipitation, settled on bottom | Milky | Test 3: NaOCI (Bleach) | Clear (Nothing) | Nothing | Nothing | Orange (Clear) | Nothing | Orange | Unknown A is identified as NaCI (Sodium Chloride), because in test#1 the solution turned a cloudy white color when Ca(NO3)2 (Calcium nitrate) was added. In the first part of test#2, when AgNO3 (Silver nitrate) is added, the solution turned white, with a thin layer of film developing on the surface.
Carboxylic acids, their derivatives and Amines Experiment 1 5 cm3 of dilute ethanoic acid with : | Turned: | A few drops of U.I solution | Pinky red | Strip of magnesium | Effervescence | ½ spatula of sodium hydrogen carbonate | effervescence | ¼ spatula of Copper (2) oxide | Turns brown/black then goes deep blue | 3cm3 of ethanol + Conc H2SO4 + sodium carbonate solution | Smelt like modelling glue | Equations: 1. A) CH3COOH -> CH3COO- + H+ B) 2CH3COOH + Mg ---> (CH3COO)2 Mg + H2 C) CH3COOH +NaHCO3--->NaCH3COO + CO2 +H2O D) 2CH3COOH + CuO ---> (CH3COO) 2Cu + H2O E) Method 1. Set up a testube rack, with 5 test tubes. 2. Within each testube add 5cm3 of ethanoic acid 3.
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.
high melting point, hard, brittle, slightly soluble in water, conductor of electricity when melted or in solution Molecular solid - crystalline solid that has molecules arranged in a particular configuration. low melting point, generally insoluble in water, nonconductor of electricity. Metallic solid - crystalline solid that has atoms of metals arranged in a definite pattern. low to high melting point, malleable, ductile, conductor of electricity, insoluble in most solvents. Lesson 13.6 Changes of physical state: * necessary to draw a temperature-energy graph to see the change in temperature with a constant application of heat Heat of fusion - the amount of heat required to melt 1.00 g of substance.
Jessica Atanova CHEM 104 lab 03/10/14 SUBSTANCES Granular zinc- gray crystal like | Iodine crystals- dark, circular, rock-like | De-ionized water: used for standard Zinc Ion procedure. | Materials: Boiling tube: for products. | Small test tubes: used to centrifuge the solution and precipitate | Graduated cylinder: used for measurement of water | Stirring rod: used various times to stir samples and solutions. | Spatula: used to measure and transfer the substances. | Centrifuge: used to isolate the solid from the solution | .
The first chemical reaction was in well A-1, two drops of NaHCO3 (sodium bicarbonate) was added to the well followed by two drops of HCl (hydrochloric acid). Bubbles were formed immediately; these bubbles formed are carbon dioxide. The next reaction was in well B-1, two drops of HCl (hydrochloric acid) was added to the well followed by two drops of BTB (bromothylmol blue), this
Answer: Mg bubbled and increased in temperature when HCl was added Zn bubbled and smoked when HCl was added CU(NO3)2 changed from blue to green when HCl was added (4) Question: Classify the following properties of sodium metal as physical or chemical Answer: Silver Metallic Color: Physical Turns Gray in air: Chemical Melts at 98 C: Physical Reacts explosively with Chlorine Gas Chemical (5) Question: Classify the following changes as physical or chemical Answer: Water freezes at 0 C Physical Baking soda when combined with Vinegar produces butter Chemical Mothballs gradually disappear at room temperature Physical Ice cubes in a freezer get smaller with time Chemical Tarnishing of Silver Chemical (6) How would you show that dissolving table salt is a physical change? After table salt is dissolved in water it can be extracted again by letting the water evaporate since it doesn’t chemically