Essay On Titration Of Carbonate And Bicarbonate

1. The first experiment is Preparation of a Cobalt Amine Bromide Product ; Synthesis #3 was used to create the compound. Added 5 grams of cobalt carbonate to 20 mL of hrdrobromic acid in a beaker. Noticied a slight color change to dark purple. Solution frothed after it settled I mixed in 15mL water and

2. Write a statement to explain the molecular composition of the unknown solution based on the results obtained during testing with the Biuret solution and each sample solution.

2. To titrate a hydrochloric acid solution of “known” 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.

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

Write a balanced chemical equation for the reaction of carbon dioxide with limewater. The formula for the active substance in limewater is on the pipet, and the products of the reaction are calcium carbonate and water.

* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube

The manufacturer results shows that Alka-Seltzer has 1.9 grams per tablet. In the experiment the results are too small compared to the number that is given by the label. In the first run only .0588 grams reacted to the acid. That suggest that the tablet only contains 0.588 grams of sodium bicarbonate which is very different from the manufacturers. The second run gave an even smaller number of gram. In terms of moles only .0007 reacted in the first and third run and only .0006 in the second run. There are many factor that could had alter the amount of moles that reacted to the acid which affected the result in showing that there is a smaller composition of sodium bicarbonate in the tablet than that of the manufacturer’s.

The problem that was trying to be solved in this study deals with analyzing unknown solutions. In this particular case, a chemical company has several unknown solutions and to correctly dispose of them they need to know their properties. To figure out the properties several qualitative tests were performed throughout the study (Cooper 2012).

The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O.

Next, add concentrated HCl drop wise until the litmus paper indicates that it is acidic. During this procedure, I added to much HCl because many CO2 gas bubbles evolved. This error in the experiment will cause the recovery % to be lower.

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

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

The amount of soda ash needed for the experiment was calculated using the following equation: sample weight of unknown=0.1103M (18ml×150.99)/(10×2× %〖Na〗_2 〖CO〗_3 ) An analytical balance was used to weight the calculated amount of soda ash. A piece of weighing paper instead of a weighing boat was used. The mass was recorded. The weighed soda ash was transferred into a 250 mL beaker, then the sample was dissolved in approximately 70 mL of water. The pH meter and electrode was obtained, rinsed with DI water, and calibrated using pH 7 and pH 4 buffer. A burette was obtained, mounted on a ring stand, and filled with the standardized HCl solution, that was prepared in Experiment 2. Since magnetic stirring bars and stirring plates were not available, the students

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.