Faculty of Pharmacy
Analytical Chemistry Department
Assignment Topic: Calcium Acetate
Course Title: Analytical Chemistry 2
Course Code: PC223
Lab Group: F3
Submitted To: Dr. Souha Hosam
Prepared By: Manar Mohamed Abd El Aziz - 170339
Due Date: 23-10-2017 Introduction:
There is more than one method to be used in the quantitative analysis. One of these methods is titration method which used in the titrimetric analysis. Titrimetric analysis is the quantitative chemical method which determines the accurate concentration of sample to react with another known volume and concentration substance. Titrimetric analysis was been called volumetric analysis as it expresses the analysis method better than volumetric analysis. The standard in titrimetric
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It has slightly acetic acid odour and melting point at 160C. Calcium acetate is highly soluble in water, partially soluble in alcohol, and insoluble in benzene and acetone. Its stability is very hygroscopic. It produces acrid smoke and fumes in decomposition at 160C and has 6-9 pH.
Assay of Calcium Acetate:
European Pharmacopeia: Add 0.150 g of calcium acetate to 100 mL of distilled water, dissolve, and carry out the complexometric titration of calcium (2.5.11). 1 mL of 0.1 M sodium edetate is equivalent to 15.82 mg of C4H6CaO.
The assay method is complexometric titration.
British Pharmacopeia:
Add 0.150 g of calcium acetate to 15 ml of distilled water, dissolve, and add 5 ml of diethylamine. Titrate with 0.1 M sodium edetate and determine the end-point using methylthymol blue mixture.
The assay method is titration.
American Pharmacopeia:
Add about 300 mg of Calcium Acetate to 150 mL of water containing 2 mL of 3 N hydrochloric acid. While stirring, preferably with a magnetic stirrer, add about 30 mL of 0.05 M edetate disodium VS from a 50 mL buret. Add 15 mL of 1 N sodium hydroxide and 300 mg of hydroxy naphthol blue, and continue the titration to a blue endpoint. Each mL of 0.05 M edetate disodium is equivalent to 7.909 mg of C4H6CaO4.
The assay method is
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Cool, transfer to a 250-ml volumetric flask, dilute to volume with water, and mix. Transfer 50 ml of the solution to a 400ml beaker, add 100 ml of water, 25 ml of sodium hydroxide TS, 40 mg of murexide indicator preparation (an alternative indicator is hydroxynaphtol blue, of which 0.25 g is used - in this case the naphthol green TS is omitted), and 3 ml of naphthol green TS. Titrate with 0.05 M disodium ethylenediamine-tetraacetate until the solution is deep blue in colour. Each ml of 0.05 M disodium ethylenediaminetetraacetate is equivalent to 7.909 mg of
All standardizations are performed in triplicate. Weigh out .1000-.1200 gram KIO3. Add 70-80 mL of deionized water. Swirl and dissolve. Add 3 mL of 6M HCl. Swirl and mix. Quickly titrated the brow-red solution with 0.1M Na2S2O3 until it is light yellow. Then add 3.5 mL of starch indicator. Titrate again until the dark color first disappears.
1. To titrate a hydrochloric acid solution of “unknown” concentration with standardized 0.5M sodium hydroxide.
As a group, we obtained our salt mixture of calcium chloride and potassium oxalate, and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution, leaving the precipitate. Once the precipitate was dried overnight, it was weighed and the mass was measured. Then we calculated the moles of the precipitate.
Step 4: Place the test tubes into separate coffee cups to maintain the upward position. Add 2 mls of the catalase solution to each of the test tubes and then place tubes1, 2, and 3 in the conditions described above. For test tube 4, fill the coffee mug half full of boiling
The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)
= = == Calcium Carbonate + Hydrochloric Acid Calcium Chloride + Water + Carbon Dioxide Equipment ---------
Add to this 5 drops of pH 4 buffer solution * Measure out 2 cm³ starch solution * Start stopclock and leave for 1 minute * Measure out 1 cm³ amylase and place in second corvette * Add to this 2 cm³ distilled water *
But the result met the expectation because the color of the solution was reached the end point by changing from red to blue. The primary errors may occur because of misreading the buret while measuring the volume of EDTA. Another error can affect the result of the experiment was that letting the volume of EDTA excess the ending point; so that the volume of EDTA was overapply that lead error. The last source of error was that our unknown sample had high percentage in mass of Mg2+, so that we need more than 50 ml of EDTA( which was the capability of the buret) to reach the end point. We had to refill the buret while measuring; and also the large volume of solution made the color harder to recognize the end point. That also led to error.
7. Using the slider on the right hand side, add NaOH to the HCl in the Erlenmeyer flask (This action is known as titrate). Add the indicator until the color of the indicator turns a light shade of pink.
Again, label 7 1.5ml tubes 0 thru 6. Place 15μl of each serially diluted extract into its corresponding labeled tube. Next add 465μl of media into each tube. Then 60μl of Alamar blue in each tube. Finally add an additional 60μl of cells (adjusted to 10,000 cells/20 μl). Vortex each tube for 5 seconds. Now, take 3 different samples 190μl samples of concentration 0 and put it in Wells A2, B2, and C2. Repeat this step again by taking 3 more different 190μl samples of concentration 1 and putting it in wells A3, B3, C3. It should be noted that it is important to vortex each 1.5μl tube again be-fore putting it into the 96 well plate. Contin-ue this same procedure consecutively for the re-maining concentrations.
then we know Ca2+ is involved in the solution. Next we add OH into the
ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is
Place 100 ml of distilled water in a 250-ml (or 400-ml) beaker. Add 1.26g of oxalic acid dihydrate (H2C2O4.2H2O) and 1 ml of concentrated ammonia. Stir the mixture until the solid has dissolved completely.
In this experiment, the Ksp for calcium sulfate dihydrate, CaSO4·2H2O, by titrating 4 times a calcium sulfate dihydrate solution with diprotic EDTA, H2(EDTA)2-. For each trial we found the Ksp by means of molarities and activities. The results for the Ksp using only molarities was very different than the Ksp using activities. The average Ksp using molarity only was 2.26 x 10-4 and the average Ksp using activity turned out to be 2.31 x 10-5. The actual Ksp however, is 3.14 x 10-5. A percent error of 26.6 % was calculated.
Sodium hydrogen carbonate was added to the solution until it becomes neutral. Ph paper was used for this test to determine its ph value.