The tip of the inner blue flame is the hottest portion. 4. How will you know in this experiment when the hydrate BaCl2*2H20 has been completely dehydrated? It will be completely dehydrated when the difference in successive weights of the crucible, cover, and residue (after cooled to room temp.) is 0.0020 g or less.
Gracen Seiler April 7th, 2015 Section- 109 Investigating Stoichiometry with Sodium Salts of Carbonic Acid Introduction- This experiment is intended to help find a better understanding of chemical stoichiometry through titrations of NaHCO3 and NA2CO3 with HCl. A chemical reaction is a process that involves rearrangement of the molecular or ionic structure of a substance, as opposed to a change in physical form in a nuclear reaction. Titration is when a measured amount of solution of unknown volume is added to a known volume of a second solution until the reaction between them is complete. The objective of this experiment is reacting sodium bicarbonate (NaHCO3) and sodium carbonate (NaCO3) with hydrochloric acid (HCl) to produce sodium chloride (NaCl), water (H20) and carbon dioxide (CO2). -Use the titrations of the following chemical reactions: NaHCO3 + HCl (aq) NaCl (aq) + H2O (l) + CO2 (g) 2HCl (aq) + Na2CO3 (s) 2NaCl (aq) + H2O (l) + CO2 (g) Experimental procedure- Two Erlenmeyer flask must be labeled “unknown 1 and unknown 2”.
Fill the burette with 0.005mol dm-3 potassium manganate(VII) solution. 6. Pour some of the thyme extract solution into a 250cm3 plastic beaker. 7. Using a measuring cylinder, add 50cm3 of 1.0mol dm-3 sulphuric(VI) acid to the thyme extract in the conical flask.
Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight. By using the information above in our experiment, we were then able to determine that one of these ionic compounds are not soluble in Water and in turn, produced a resulting precipitate which is the evidence that a reaction has occurred. We then identified the anion and cation for these ionic compounds. The Potassium Chromate-
Discussion & Conclusion In this experiment we learned how to synthesize the cyclohexene by dehydration of cyclohexanol. We procedure the first step where we have to mix the components. Then we heat the R.B.F with a fractionating column, distilled water. Then we obtained the layers, and we transferred the organic layer to a small, dry Erlenmeyer flask. We added anhydrous Sodium Sulfate as a drying agent.
The carbonate anion test mixes 1 mL of test solution and drops of 6M HCl. The formation of bubbles shows the presence of carbonate (CO32-). The acetate anion test heats 2 mL of the test solution, 1 drop of 18M H2SO4, and 1 mL (100%) ethanol. A fruity smell, using the wafting technique, shows the presence of acetate
The Loss and then Retrieval of Copper through Multiple Reactions Lab Partners: Justin Dunn and Alexis Almaguer Experiment #2 Section: 506 Intro: All science occurs within rules. One very important rule is that matter can neither be created nor destroyed and this rule will be expressed and proven in this lab by removing copper and then regaining it through multiple reactions, heating, and stirring. This experiment allows the students to learn the different types of reactions as well as learn new techniques within the laboratory such as vacuum filtration and handling hot glassware, but most importantly proves the law of conservation of mass. Materials and Methods: to begin the experiment a 50 ml beaker, hot plate, plastic funnel, aspirator,
Heats of Solution and Reaction Name: Cindy Hernandez Purpose: The purpose of this experiment is to decided if the chemical reactions are exothermic and endothermic. By finding the differences between each temperature. Overview: For this lab, we had three different chemicals involved NH4Cl, H2SO4, and NaOH. What we did with these chemicals was that we added water, except NaOH we added HCl, was that we combined both mixtures to determine if there was a temperature change. The reason why we're determining if their was a chemical reaction is to identify if it is exothermic or endothermic.
The chemical reaction for this experiment is: 3NaHCO3(aq) + C3H4OH(COOH)3(aq) C3H4OH(COONa)3(aq) + 3H2O(l) + 3CO2(g) sodium bicarbonate + citric acid sodium citrate + water + carbon dioxide Purpose: The purpose of this lab is to show visual evidence of the law of conservation of mass during a chemical reaction. Materials: 1) Plastic beaker 2) Paper towel 3) Effervescent tablet (Alka Seltzer) 4) Access to water 5) Balance 6) Safety goggles 7) Plastic bottle (500mL) with air-tight screw cap Variables: - Dependent Variables: - Independent Variables: Procedure: 1) Pour about 50 mL of water into the beaker. If you get the outside of the beaker wet, dry it using a paper towel. 2) Break the tablet in half. Shake or blow any loose grains off the tablet.
Microliter syringe is used for the introduction of samples into the column of gas chromatography (GC). The sample injection port, column and detector are heated about 50°C higher than the boiling point of the least volatile component of the sample (SHU, 2014). The temperature of the injection port and detector are usually slightly higher than the column. This is to increase the rate of vaporization of the injected sample and prevent the sample from condensed in the detector.