Erlenmeyer flask

Get a hot plate, two 50 ml Erlenmeyer flask, and a magnetic bar. Set up the hot plate under neither the fume hood and put on low heat. Using the pipettes provided, gather .4 ml of salicylaldehyde and place it in one of the 50 ml erlenmeyer flask. With the other 50 ml erlenmeyer flask add .2 ml of ethylenediamine and the magnetic stir bar. Add 10 ml of methanol to each flask, make sure that this step is completed underneath the fume hood, and swirl the mixtures thoroughly. Once completed carefully

Pestle Vitamin C tablet 2 Erlenmeyer flasks 250 mL Balance 50 mL buret Buret clamp Support stand 250 mL beaker Short -stem funnel Sodium hydroxide(NaOH) 150 mL dry beaker Stirring rod Phenolphthalein solution Procedure: 1.Two 250 mL erlenmeyer flasks was labeled 1 and 2 and weighted 2.Vitamin C tablet was crushed into powder and transferred roughly equal into the labeled erlenmeyer flasks. 3.The mass of erlenmeyer flasks that contained the powder of vitamin c was measured

to boil, a 125-mL Erlenmeyer flask was obtained. P-aminophenol (1.5g) was weighed and then placed inside the Erlenmeyer flask. Deionized water (25 mL) was added to the flask followed by 35 drops of concentrated phosphoric acid. An additional 15 drops were added to the solution, since the initial 20 drops of concentrated phosphoric acid was not dissolving the p-aminophenol. Phosphoric acid was added to the reaction mixture because it acted as a catalyst for the reaction. The flask was then swirled

This experiment is designed to demonstrate how to use volumetric tools and how to calculate the molarity of an unknown based on the usage of these tools. Volumetric tools include burets, pipets, and volumetric flasks and can be used to react an unknown substance with a substance of known concentration to find the molarity of an unknown. This specific experiment sought to find the concentration of an HCl solution by reacting it with a standard NaOH solution. An indicator was added to show when this

g (2.87 mmol) of 2-methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2-methylphenol, 0.957 mL (0.00287 mmol) NaOH was calculated and collected in a syringe. The NaOH was then added to the 2-methylphenol solution and allowed to mix completely. In another 10 mL Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated

experiment, we placed a boiling stone into a 25 mL Erlenmeyer flask. Using a small piece of aluminum foil and a rubber band we sealed the mouth of the flask. We pinched a small hole in the center of the aluminum foil, and we measured the mass of the dry flask, boiling stone, and foil cap to the nearest 0.001 g. We obtained about 25mL of an unknown volatile liquid using a 10 mL graduated cylinder. We meticulously took

Introduction For this experiment, we are going to determine the effect of temperature on solubility, to be done in a chemical by dissolving a solute in a definite amount of solution which is saturated. Specifically, the goal of this experiment is to prepare a saturated solution of Na2C2O4 in water at different temperatures, determine the effect of temperature in solubility, and to apply Le Chatelier's Principle. We can do all this by simply titrating a certain amount of standard KMnO4, and measuring

The purposes of this experiment were to model a bimolecular nucleophilic substitution reaction between potassium hydroxide (KOH) with 1-bromopropane and determine whether it follows a second-order rate law mechanism. A rate constant of 0.0684 M-1 min-1 was obtained for this reaction at 45.1°C, which was determined through equilibrating the reaction and performing titrations of 0.390 M KOH with 0.1000 M hydrochloric acid (HCl). The activation energy calculated from class data was 50.188 kJ/mol, which

EXPERIMENT 4A: Synthesis of an Iron(III)-Oxalate Complex: To begin, a filtering crucible was washed, labeled, and dried in an oven for one hour. While the experiment was performed, the filtering crucible was set-aside in a desiccator to cool and stay dry. After this was done, a mass of about 1.2 g (±0.2 g) of iron(II) ammonium sulfate hydrated salt (Fe(NH4)2(SO4)2 ∙ 6H2O) was measured and recorded. It was then placed in a 50-mL beaker with 3 mL of deionized water and 1-3 drops of 6M sulfuric acid

MATERIALS • Erlenmeyer flask (125 mL) • Agarose (0.75g) • Scoopula • Weigh boat • Digital scale • Graduated cylinder (50 mL) • Pieces of aluminum foil • Vials of DNA samples (14): o lambda Hind III/ Eco RI (4) o mutated (2) o wild type (2) o child #2 (2) o child #1 (2) o No DNA (2) • Masking tape • Stirring rod • Mitton-like gloves • Hot plate • Well-forming comb • 1×TAE Buffer (50mL) • Power Supply (150V) • Gel Electrophoresis Chamber • Gel Tray • Pipets (6) • Latex gloves • Permanent marker