11.Repeat procedure again. Part Two 12.Use the thiosulfate to refill the 50 mL buret. 13.In a Erlenmeyer flask, add 1 mL of bleach. 14.Add this Erlenmeyer flask to 25 mL of distilled water. 15.Dissolve 2g of KI in the flask.
Objective The purpose of this experiment was to become familiar with the ability to reproduce an experiment several times. Experimental Materials 1 x Magnetic Stirring Bar (yellow) 2 x 100 mL Flask 8 x 50 mL Erlenmeyer flask Magnetic Hotplate Glass Stirring rod Distilled water Pipet (with Pump handle) Starch 0.20M Ammonium Persulfate (NH4)2S2O8 0.20M Ammonium Sulfate (NH4)2S2O4 0.20M Potassium Nitrate (KNO3) 0.20M Potassium Iodide (KI) 1.2 x 10-2M Sodium Thiosulfate (Na2S2O3) Experimental Method 1. All materials were obtained from the classroom. 2. The flasks were thoroughly cleaned with distilled water.
To do this, first take the number of drops used to achieve the monolayer (1 drop) and convert it to mL using the calibrated number of drops per mL. Then multiply the number of grams of sodium stearate per milliliter of solution. Finally, convert to moles through the molar mass of sodium stearate. HINT: The molar mass of sodium stearate is 296.5 g/mole. Answer = 1.06*10^7 moles/top layer 5.
In the first part, preparation of 5 x 10-3 m EDTA titrant was done by dissolving approximately 0.47 grams of EDTA in 250 ml distilled water. A pinch of MgCl2 • 6H2O was added. The solution served as the stock titrant. In the second part, preparation of diluted EDTA titrant was done. We took 10.00 ml aliquot of the prepared titrant and placed it in a 100.0 ml volumetric flask to dilute.
Eggshell was ground, and a mass of 0.1 gram was transferred to an Erlenmeyer flask. 150 drops of acid were added to the eggshell and agitated for about three minutes. The sides of the flask were washed down, then phenolphthalein indicator was added to the solution. Base was added from the base solution until a color change was noted in the indicator. The amount of base added was recorded when the color change was permanent.
Determination of Enthalpy Change Objective: to find the enthalpy change (∆H) in the decomposition of Sodium Hydrogen Carbonate. Materials: Calorimeter, 2.00 mol HCl, NaHCO3, Na2CO3, Lab Quest, Temperature Probe, Graduated cylinder, Balance scale. Procedure | Observations | 1. Obtain 50 mL of HCl in a beaker. | N/A | 2.
Experimental Section 2.1 The Catalytic Precursor Preparation A mixture of palladous chloride (0.0384 g, 0.216 mmol) and sodium chloride (0.0303 g, 0.518 mmol) in water (1.5 ml) was stirred and warmed to about 50ºC. The solution was allowed to cool down. A solution of triphenylphosphine (0.1280 g, 0.488 mmol) in ethanol (20 ml) was then prepared. The palladous chloride solution was added dropwise to the triphenylphosphine solution and stirred simultaneously. The resultant slurry was then warmed to about 50ºC over 30 minutes to coagulate the precipitate.
Method Part 1 1 Clean the surface of the 0.5cm piece of magnesium with a piece of steel wool 2 Place the magnesium into a test tube 3 Add three drops of detergent to the test tube 4 Add 2 cm of hydrochloric acid to the test tube. Set timer for 5 minutes and record your observations, including the height of the foam produced in a results table 5 Repeat the process for the
A 125mL Erlenmeyer Flask was used to combine (15mL) of concentrated aqueous ammonia and ammonium chloride (0.0467mol, 2.49g). The mixture was stirred till fully dissolved. Colbalt (II) chloride hexahydrate was ground (6.2g) and added in small amounts to the stirring solution (0.0210mol, 5.2g). As the mixture continued to stir (4mL) of 30% hydrogen peroxide was added drop wise to yield a dark warm slurry. After the effervescence, (15mL) of concentrated HCl was added drop wise to the solution.
Experiment 7: Ksp of Ca(OH)2 CHE 112 Abstract The primary objective in this experiment was to determine the solubility product constant of a calcium hydroxide that was very slightly soluble. At the conclusion of the experiment, the results determined that as the concentration of the medium increases, the solubility of the precipitate increases. Using the solubility product constant, it was determined that the solubility of calcium hydroxide precipitate decreased when dissolved in a medium possessing a common ion. Experiment and Observation For the first part of the experiment, 5 drops of 0.1 M calcium nitrate were placed in a 6-well row of a 24-well plate. 5 drops of distilled water were placed in wells 2 through 6.