Calculate the concentration of grams of sodium stearate per milliliter of diluted solution. To do this, multiply the concentration of sodium stearate in the dishwashing liquid by the dilution of the solution (1.50 mL dishwashing liquid per 100 mL solution). Answer = 1.5 *10^-4 g/mL 4. Calculate the number of moles of sodium stearate in a single layer. 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.
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.
APPARATUS: Burette (50 cmᶾ), Pipette (25 cmᶾ), two conical flasks (250 cmᶾ), two beakers (250 cmᶾ), funnel, wash bottle, retort stand, boss and clamp, evaporating dish, pipette filler, hot-plate. MATERIALS: Approximately 2.0 mol dmˉ³ hydrochloric acid, 1.0 mol dmˉ³ sodium hydroxide, methyl orange indicator. METHOD: 1. Firstly, the burette was rinsed with a little hydrochloric acid and filled up to just above the zero mark. 2.
For step 3, the solution was heated with a hot plate. The solution was heated until a change in the reaction mix occurred. After that it was heated for another 5 minutes before cooling. For step 4, the liquid was decanted. Then 10 ml distilled water was added.
Record the combined weight 4. Determine the weight of the water by subtracting the empty beaker weight (step 1) from the weight of the beaker plus 50 ml of sea water (step 3) 5. Place beaker on hot plate and evaporate most of the water. Record the time and temperature at which the seawater begins to boil. As the water is being evaporated, record the temperature every 2 minutes.
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.
Abstract The focus of this experiment was to analyze the kinetics of a nucleophilic substitution. A mixture of 0.3622-M 1-bromopropane and 0.3622-M potassium hydroxide in an 90:10 ethanol/water solvent provided the reactants for a SN2 reaction to occur in a temperature controlled bath at 50.0˚C. The disappearing reactant was found by titrating timed aliquots during the reaction and then measuring the concentration of hydroxide. The k-value was found to be 0.0202 M-1Min-1. Using the linear form of the Arrhenius equation the activation energy was calculated to be 19.9 kcal/mol.
* 5ml of distilled water was poured down the sides of the beaker, swirled and poured into the funnel. * The filter paper containing the precipitate was allowed to dry and then weighed. 1.7g/1.4g * The weight of the filter paper was subtracted (1.1g/0.7g) to give the actual yield of calcium carbonate (0.6g/0.7g). Observations: * When CaCl2 and Na2CO3 were mixed, a white precipitate was noted immediately. * Residual precipitate was observed on the beaker when filtering.
The system was heated for 4-5 hr under vacuum at 200°C and then cooled down to the temperature (50°C) where we want to perform the adsorption study. Small doses of test gases consecutively introduced to the system and gradually increased up to 50 Torr until an equilibrium pressure was reached. Then the obtained differential heats of the test gases adsorption were recorded as a function of its coverage. Further, the manifold degassed under vacuum for almost 30 minutes; adsorption was conducted in the same manner. Finally, the number and strength of active surface are obtained from the difference between the adsorbed gases from the first and second
Fill the conical flask with 50 cm3 of 0.2 M hydrochloric acid. 4. Weight up 0.2 g of magnesium strips. 5. Put that magnesium strips into the conical flask which contains 50 cm3 of 0.2 M hydrochloric acid.