White precipitate shows the presence of chloride (Cl-). Chloride anion equation: HCl(aq) + AgNO3 (aq) → HNO3 (aq) + AgCl(s). The nitrate anion test involves cooling a mixture containing 1 mL of test solution and 3mL 18M H2SO4. 2mL is poured down the inner test tube side and the presence of a brown ring shows nitrate (NO3-) to be present. The carbonate anion test mixes 1 mL of test solution and drops of 6M HCl.
After a small amount of time the solution began to produce gas and the copper was being used up in the reaction. The solution turned an aqua like blue and eventually all of the copper had now been used into this blue solution which was copper nitrate and water, the gas being produced was nitrogen dioxide and the fume hood had removed it during the reaction. Next we slowly added drops of 6 molar sodium hydroxide to the solution until it became basic and turned a red piece of litmus paper blue. While we added NaOH the solution turned green indicating a new reaction had occurred and turned the litmus paper blue. We then began to heat and stir the solution until it changed color again and it turned black with a layer of water on top.
| | | An Activity Series 1/9/13 Makieya DunhamPartners: Jasmine Lewis and Danielle Anderson | | | Problem Statement: In this lab we determined the activity series for five metals and for three halogens. In the first part of the lab we used a microscale technique to rank the metals that reacted with the other metal nitrates from most reactive to least reactive. The metal that reacts with another metal nitrate, then the solid metal have reduced the other metal ion and is the more reactive metal of the two. In the second part of the lab we used the solvent extraction technique to derive an activity series for the halogens. Safety Precautions: When in the lab we wore goggles, an apron, and gloves the entire time.
Name: Melody Wong N8426066 Cation and Anion Reaction 1. Objectives Educational Aims * To learn how to set up a practical experiment * To compare experimental results with the theoretical results and explain any discrepancies. Experimental Aim * To examine the reaction between cations and anions 2. Theory A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions occur whenever bonds are formed or broken between molecules.
Let’s experiment and observe Whether these ions will have a reaction or indeed soluble in water. Experimental Procedure Let’s begin this experiment by obtaining a 100ml beaker from our equipment tool bar list, then we are going to add 50ml(s) of Potassium Chromate 1M solution to that beaker, The next step we are going to add another ionic compound of 50ml of Lead (11) nitrate 1M into the same beaker as the Potassium Chromate. As we observe the beaker, we notice a reaction has occurred and a precipitate has formed and settled on the bottom of the beaker. The next step is we are going to filter the resulting precipitate into a 250 ml Erlenmeyer Flask with a Buchner funnel. Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight.
12. Place a paper towel over the drain, pour the content of the well plate, throw the paper towel and rinse the well plate. DATA, OBSERVATIONS, AND CALCULATIONS: Data Table: Oxidation - Reduction | | Reactions | Mg in Na2SO4 | Bubbles | Zn in MgSO4 | Small bubbles | Pb in Zn(NO3)2 | Dark lead changed into lighter color | Pb in FeCl3 | Changed the lead into slight green yellow | Fe in CuSO4 | Changed the iron into orange color | Note: I added more than 10 drops to make sure that the pieces are well covered. QUESTIONS: A. Based on your observations make an activity series of the metals used.
After 10 seconds, the colorless mixture suddenly turns blue. Concept: Demonstrates a typical clock reaction; shows the effect of the interaction between chemical reactions that have different rates. Materials: • Solution A o 0.6 grams Starch o 30 mLs of Acetic Acid o 4.1 grams of Sodium Acetate o 50 grams of Potassium Iodide o 4.7 grams of Sodium Thiosulfate ▪ Allow mixture to cool and dilute to 1 liter with distilled water o 1 liter flask • Solution B o 500 mLs of 3% Hydrogen Peroxide o 500 mLs of distilled water o 1 liter flask o Safety: Hydrogen Peroxide can be irritating to skin and eyes. Wear safety goggles and gloves. Procedure: Mix the two solutions together.
Part 1 of The Redox Arena Objective: In this experiment, we had to conduct research on zinc, iodide, and acidified water. What my partner and I did was we mixed the aforementioned elements with acidified water to see what would happen. We took notes on the physical traits of each, and then we compared out qualitative results with the three samples we had. Materials & Observations: * electronic balance * Bunsen burner * Parafilm * Spatula * Boiling tube * Corks * large beaker * Stirring rod * large test tube * test tube rack * small graduated cylinder * pipets * grease pencil * Ziploc bag * Boiling chips- off white, small pebble like pieces * Desiccant- white small rocks, chalky * Acidified water- clear liquid * Sodium thiosulfate- clear liquid * Granular zinc- gray, small, mineral like * Iodine crystals- dark grey, shiny solid * Zinc ion- grey, irregular shaped * Solid zinc iodide- white solid * Mineral oil- colorless solution The Mass table was as followed: Chemicals | Amount | Granular Zinc | 2.01 grams | Iodine Crystals | 2.01 grams | Acidified Water | 5.0 mL | Procedure: 1. Obtain a boiling tube, a large test tube and a small test tube.
The reduction of permanganate requires strong acidic conditions. Introduction: In this experiment a purple colored solution of potassium permanganate, with an approximate concentration of 0.025M, will be added to a solution containing Fe2+ ions. The manganese is reduced from a 7+ oxidation state in the permanganate ion to form colorless Mn2+ ions. The equivalence point is indicated at the point when all of the Fe2+ ions in the solution are oxidized and the colorless mixture retains a purple tint. Procedure: Fill a buret and tip with KMnO4.
Chemistry Lab Types of Chemical Reactions OBSERVATION DATA TABLE Step|Name of Reactants|Description of Reactants|Description of reaction taking place (evidence of chemical reaction)|Description of Products| 1|Zn|Solid, small chunky bits, Silvery-grey, dull|As the Zinc and Sulfur heated up it expanded in the test tube and shot out Zinc Sulfide.-light and heat are produced|White powder was created and the leftovers of the reactions was a black powder.| |S|Solid, resembles powder, Off-yellowOpaque||| 2|KI|-dull yellow liquid-transparent|Instantaneously changed colour to a bright yellow.|-Bright yellow liquid-Opaque| |Pb(NO3)2|-liquid, transparent, very clear-bubbly||| 3|H2O2|-liquid-clear-transparent|A dark grey bubbling liquid was created. It got hotter as it reacted.gas test observations:The splint relit. Oxygen was present.|Oxygen gas was created and a dark grey opaque liquid was left behind in the test tube. | |MnO2|-solid-powder-black||| 4|AgNO3|A clear, transparent liquid.|As the copper reacted with the Silver Nitrate, the ball of Copper changed colour to grey and subsequently developed a ‘furry-like’ characteristic on its coating.|-Clear liquid-Copper changes to a grey colour, ‘furry-like’.| |Cu|-brown/red-solid-stringy||| 5|HCl|A clear, transparent liquid.|When the Magnesium was inserted the HCl liquid started to bubble and fizz releasing Hydrogen. The Magnesium strip dissolved in the process and the test tube got hotter.