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Electrolysis in chemistry
Introduction about electrolysis in research
Introduction about electrolysis in research
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The purpose of the experiment was to determine the solubility of calcium sulfate. In Part A with the resin, The number of moles in the original CaSO4 sample was determined to be 3.69 x 10-4 moles, and the molarity of calcium in the saturated CaSO4 solution was determined to be 0.0148 M. The molarity of calcium in the saturated CaSO4 solution is equal to the solubility of CaSO4, so the solubility of CaSO4 was determined to be 0.0148 M at 18.9 °C. In Part B with the titration using EDTA, the moles of calcium in the original saturated calcium sulfate solution was determined to be 3.87 x 10-4 moles in Trial 1 and 3.74 x 10-4 moles in Trial 2, so the molarities of calcium in the saturated solution were determined to be 0.0155 M in Trial 1 and 0.0150
M in Trial 2. The molarity of calcium in the saturated solution of CaSO4 is equal to the molar solubility of calcium sulfate in water, so the average molar solubility in Part B was determined to be 0.0153 M at 18.9 °C. The average molar solubility of calcium sulfate was determined to be 0.0151 M at 18.9 °C. One possible source of error in this lab was possible incorrect amounts of solution mixed in the solutions. Because the pipet requires a finger to completely cover the top in order to keep the solution from dripping out, it is likely that some of the solution escaped between measuring 25 mL and adding it to the flask by way of finger movement over the top of the pipet. This would have caused smaller amounts of solution to be titrated than expected, so the molarity would be calculated to be higher than the actual molarity. Another potential source of error was the possibility of over-titration. It is likely that the NaOH added in Part A and the amount of Ca(CH3COO)2 in Part B were added slightly in excess of the actual equivalence point. This would cause the amount of moles calculated to be higher than the actual number of moles, which then would lead to a calculation of high molarities than the actual molarities.
The purpose for this experiment was to determine why it was not possible to obtain a high percent yield when Calcium Nitrate Ca(〖NO_3)〗_2 with a concentration of 0.101 M was mixed with Potassium Iodate KIO_3 with concentration of 0.100 M at varying volumes yielding Calcium Iodate precipitate and Potassium Nitrate. Filtration was used to filter the precipitates of the solutions. The percent yield for solution 1 was 87.7%, and the percent yield for solution 2 was 70.8%. It was not possible to obtain a high percent yield because Calcium Iodate is not completely soluble and some of the precipitates might have been rinsed back to the filtrates when ethanol was used to remove water molecules in the precipitate.
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
At this point the identity of the unknown compound was hypothesized to be calcium nitrate. In order to test this hypothesis, both the unknown compound and known compound were reacted with five different compounds and the results of those reactions were compared. It was important to compare the known and unknown compounds quantitatively as well to ensure that they were indeed the same compound. This was accomplished by reacting them both with a third compound which would produce an insoluble salt that could be filte...
The amount of hydrochloric acid. 3. The concentration of the hydrochloric acid. 4. The surface area of the calcium carbonate.
Investigating the Rate of Reaction Between Marble Chips and Hydrochloric Acid I am investigating the rate of reaction between marble chips (calcium
This will have taken the molar down to 0.2M so by repeating this process again the molar will be taken down to 0.02M, which is now ready for the titration. I performed the titration with the hydrochloric acid of 0.02 moldm-3 in a burette and 25cm3 calcium hydroxide in a conical flask. I considered the first reading as a rough reading and took another three readings, so that no anomalous result might occur.
Finding the Solubility of Ca(OH)2 Aim: ---- To determine the solubility of Ca(OH)2. To carry out the aim of this experiment an experiment needs to be planned and carried out. I am given the information that the solubility of the Ca(OH)2 is between 1 to 1.5g per dm3. Also I am given a standard solution of 1M hydrochloric acid (HCl) which may have to be diluted to suit the measuring needs of the experiment. Apparatus: [IMAGE] * 1g of Ca(OH)2.
Table of actual concentration of Each Ca2+ external calibration solution and experimental concentration measured by Atomic absorption spectrophotometer (AAS).
If the HCl needs to be twice as big as the alkali it needs to be
The Determination of the Solubility of Calcium Hydroxide I have to plan an experiment to find the solubility of calcium hydroxide, Ca(OH)2, in water. I have to make up a solution of calcium hydroxide and carry out a titration using hydrochloric acid solution of the chosen concentration. The equipment need is as below: · Solid calcium hydroxide · Methyl orange indicator · Volumetric flask (250cm3) · Clamp and boss · Clamp stand · Burette (50cm3) · Conical flask · Pipette (25cm3) · Pipette filler · Distilled water · White spotting tile · Hydrochloric acid of chosen concentration · Beaker x2 · Rubber bung · Funnel x2 · Electronic scale ‘The maximum mass of calcium hydroxide needed to produce 1dm3 of saturated solution at room temperature is 1.5g.’ I only want 250cm3 as I am using a 250cm3 volumetric flask. Therefore: 1dm3 / 4 = 250cm3 1.5g / 4 = 0.375g The number of moles in volumetric flask: 0.375 / 74 = 0.005 moles I need an excess of 0.5g to make sure that all the calcium hydroxide has been fully dissolved: 0.375g + 0.5g = 0.875g I have to now work out the concentration of hydrochloric acid I will be using. The molar mass of calcium hydroxide is: C = 40
To begin the experiment, approximately 0.01g of the known solid compound was obtained in a test tube. The relative quantity was then observed and about 1mL of water was added. The test tube was then agitated for approximately twenty seconds and the quantity of solid visible was observed and subsequently contrasted to the original volume. Next, it was determined if any solid appeared to have dissolved in the water. After having determined if the solid dissolved, additional crystals were introduced into the test tube in order to determine if the solid was slightly soluble, soluble or very soluble. If the solid dissolved, the pH of the water was tested using the pH strips and the existent color change or lack there-of was observed. This process
Determining the Concentration of Sulphuric Acid Risk assessment · CorrosiveAs sulphuric acid and sodium hydroxide are both corrosive, I will wear gloves, goggles and lab coat when performing the experiment · Eye protection must be wornIf any breakages occur I will carefully dispose of the glass in a suitable bin. · If any spillages occur during my experiments I will clean them promptly. Dilution of H2SO4 As the concentration of the sulphuric acid~10moldm-3, it is too concentrated for my experiments so I will dilute it to approx 0.05moldm-3.
This experiment conducted used the Gravimetric Analysis method to determine the concentration of an unknown sulfate solution. The unknown sulfate solution was pipetted into a smaller beaker, acidified, heated, decanted through filtration, dried, cooled and weighed. What was found at the end of the result was Barium Sulfate precipitate which weighed 0.1783 grams. The concentration of the unknown sulfate solution was found to be 2.9385 g/L and its molarity was 0.0306M.
15% sodium in the form of sodium carbonate (soda ash), 9% calcium in the form of limestone
After softening a large quantity of hard water the beads become saturated with calcium and magnesium ions. When this occurs, the exchange resin must be regenerated, or recharged. To regenerate, the ion exchange resin is flushed with a salt brine solution (Figure 1). The sodium ions in the salt brine solution are exchanged with the calcium and magnesium ions on the resin and excess calcium and magnesium is flushed out with wastewater.