* The above procedures were modified from the "Background on Making Soap and Detergent" on Lab Achieves.
In week 2's experiment for HCl standardization 0.2 g of Na2CO3 was weighed and dissolved into an Erlenmeyer flask filled with 50 mL distilled water. 4 drops of Phenolphthalein were added to the solution and the color was recorded. The solution was titrated with HCl until just before the endpoint (when the solution is very light pink). Solution was cooled to room temperature and the sides of the flask were washed with small amounts of distilled water to get all of the sample back into the solution. The titration was finished (took very little HCl, proceeded slowly). Color of the solution and volume of HCl was recorded. The concentration of HCl was calculated. ( CALCULATIONS) The equipment used for the procedure is as followed: scale, graduated cylinder, beakers, Erlenmeyer flask, hot plate and titration pipette. The chemicals used in the procedure are as followed: pure Na2CO3, distilled water, phenolphthalein concentrated 1% in 50% ETOH/50% H2O, and 0.02 M concentrated HCl.
__ g 〖Na〗_2 〖CO〗_3 × ((1 mol 〖Na〗_2 〖CO〗_3)/(105.99 g 〖Na〗_2 〖CO〗_3 ))= ___ mols 〖Na〗_2 〖CO〗_3
___ mols 〖Na〗_2 〖CO〗_3 × ((2 mol HCl)/(1 mol 〖Na〗_2 〖CO〗_3 ))= ____ mols HCl
((___ mols HCl)/(___ L HCl))= ___ M (mol/L) HCl
* The above procedure
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It was a white, thick and oily substance. When the 6M Sodium Hydroxide was added to the Crisco drop by drop, the solution became a light pink color while it appeared to have a smooth surface. During mixing, the Crisco was clumped together, however it seemed to be more fluid than the original Crisco texture. Once heated to a boil, the paste turned a yellowish color and hardened when removed from the heat. The soap was then filtered using suction filtration which turned the soap into a solid 3D structure of multiple different yellowish
Marwah Alabbad Post lab 10/21/15 Question 1: 1. Experiment 1: Number of trails NaOH concentration (M) Volume of HCl solution (mL) Initial volume of NaOH(mL) final volume of NaOH(mL) The volume of NaOH to titrate HCl (mL) Concentration of HCl (M) 1st 0.1023 25.0 10.05 36.12 26.07 0.085 2nd 0.1023 25.0 5.74 31.40 25.66 0.105 3rd 0.1023 25.0 9.84 35.52 25.68 0.105 First trail calculation: 0.02607L× (0.1023mole NaOH/1L)×(1 mol of HCL/1 mol of NaOH)×(1/0.025)= 0.085M of HCl
2. Add 8cm³ of sodium carbonate to each tube using a measuring cylinder. 3. Measure out the strontium nitrate for each boiling tube and add it (boiling tube 1 contains 1cm³, test tube 2 contains 2cm³ and so on). 4.
Next, about 10 mL of both solutions, Red 40 and Blue 1, were added to a small beaker. The concentration of the stock solution were recorded, 52.1 ppm for Red 40 and 16.6 ppm for Blue 1. Then, using the volumetric pipette, 5 mL of each solution was transferred into a 10 mL volumetric flask, labelled either R1 or B1. Deionized water was added into the flask using a pipette until the solution level reached a line which indicated 10 mL. A cap for the flask was inserted and the flask was invented a few times to completely mix the solution. Then, the volumetric pipette was rinsed with fresh deionized water and
Lab report Experiment 6 The synthesis of Alum Lingrui Ge Oct 18th 2015 Purpose: discover the synthesis of alum. Materials: two 250 mL beakers, 400 mL beaker, 25 mL or 50 Ml GRADUATED cylinder, Buchner funnel and filter flask, watch glass, glass stirring rod, lab burner, ring stand, ring, wire gauze, hot plate, wash acetone, Aluminum foil, 3 M sulfuric acid solution, KOH, 50% enamel solution, ice bath, balance, boiling chips, gloves, pipe cleaner. Process: get and wear goggles, set up a Buchner funnel and flask and measure its mass.
A two-hundred and fifty milliliter(ml) flask was zeroed out on the scale. Fifty milliliters of HCl was put into the flask and weighed. The unknown mixture was poured into the HCl while
The setup for the cation exchange chromatography is shown in Figure 3. This was done by plugging the bottom of a burette with a small amount of glass wool. The wool was lightly packed using a thermometer. Approximately 5 mL of Dowex 50 cation exchange resin was obtained in a small beaker, and the resin was mixed with 5 mL of pH 3 citrate buffer. This mixture was poured into the burette with the stopcock closed.
The first calculation we used was to calculate the number of moles NaOH added to each of the antacid samples. We used the average amount of NaOH added to solve this equation. The equation for the Tums is: .0013 L X .2m = .00026 mol NaOH.
Conclusion: Every compound has a uniquely identifying molar mass as well as individual properties. In this lab, the purpose was to use the properties that three unknown alkali metal carbonate powers have, to identify the molar mass. For the three unknown substances, they all were white powders of about the same texture, and they all reacted when added to hydrochloric acid. Based on these properties, it is impossible to distinguish which one is which due to the similarities, so it is necessary to solve for the molar mass since that is unique to every element and compound.
I. Title: Mass and Mole Relationships in a Chemical Reaction II. Background: Percent yield is the ratio of actual yield to theoretical yield. Amount in percent of one product formed in chemical reaction. Actual yield is the information found is experiments or is given.
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
Titration is the basis of the Titration Lab because the goal of the lab was to titrate. Titration is determining the concentration of a solution by neutralizing it with another known concentration. We titrated the NaOH in the HCl. The titration caused a
Each buffer was measured in a 100 mL graduated cylinder and contained in a 40 mL beaker. Once the reading of the buffer was stabilized, the program entered into reading 1. The probe was cleaned with distilled water and dried before being placed into the second buffer for reading 2. Once the second calibration was completed the pH probe was cleaned again. Next the probe was placed into the unknown solution.
Stoichiometry of a Precipitation Reaction University Student Name Abstract The purpose of this experiment is to calculate the actual yield of Calcium carbonate from the reaction of Calcium Chloride with Sodium carbonate. We have to then compare the actual results with the theoretical value of Calcium carbonate and find out the error. When we mix 1.0 grams of Calcium Chloride and 0.80 g of sodium carbonate, it produces around 0.60 g calcium carbonate in the actual experiment.
Commercial vinegar, Yamaha brand 0.1 mol/dm3, NaOH soloution Phenolpthalein indicator soloution (50.00 ± 0.5 cm3 ) cm3 burrete (250.00 ± 0.5 cm3) volumetric flask a (250 cm3± 0.5 cm3)
The solution with the pigments was spotted 15 times on both region A and region B and then allowed to dry. When the plate was dry it was placed into the tank for at least 20