Quantitative Determination of Sulphate By Gravimetric Analysis Essay Sample
Quantitative Determination of Sulphate By Gravimetric Analysis Essay Sample

Quantitative Determination of Sulphate By Gravimetric Analysis Essay Sample

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  • Pages: 6 (1433 words)
  • Published: August 26, 2018
  • Type: Experiment
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The purpose of this study is to quantify the sum of sulfate through hydrometric analysis, which involves determining BaSO4 as the total amount of sulfate.

The percentage of sulfate was determined by conducting a hydrometric analysis experiment. To carry out this experiment, a diluted solution of Ba chloride was added to a hot, acidified unknown sulfate solution containing concentrated HCl. The resulting precipitate was then filtered using suction filtration, washed with water, and dried at 150 degrees Celsius for approximately 30 minutes in an oven. The dried precipitate was subsequently cooled in the desiccator and weighed as Ba sulfate. The percentage of sulfate present was calculated based on the weight of the resulting Ba sulfate.

The concentration of sulfate was found to be 0.004269 M and 0.4098 g/L. Meanwhile, the weight of Ba sulfate estimated at 0.0249g.

In the experiment, there were n


o hiccups encountered. The aim was to determine the amount of sulfate using hydrometric analysis. Additionally, students could learn about Gravimetric Analysis techniques through this experiment. Gravimetric analysis is considered to be one of the most precise analytical methods available. Typically, hydrometric analysis involves preparing a solution with a known weight, followed by subsequent steps. (1)

The most common methods for isolating desired substances from a solution are precipitation and filtration, which utilize reagents to form insoluble compounds with the desired components without precipitating other elements. The process involves three steps: (2) isolation of desired elements, (3) weighing them, and (4) calculating their sum by taking into account the weight of stray substances. For instance, in a sulfate experiment, 25mL of a given sulfate solution was utilized to determine the amount of sulfate tha

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would be obtained at the end in relation to the amount used initially.

It is important to use a fume hood when adding concentrated HCL to H2O because of the potential danger of boiling water and splattering acid caused by the heat generated. Furthermore, inhaling the toxic vapor released by concentrated HCL should be avoided.

A thicker glass covered the beaker during heating to enable condensation and prevent solution loss via vaporization. Ba chloride beads were then introduced to observe mixture homogeneity. If these beads do not dissolve in the clear solution, it suggests incomplete mixing.

When there is complete precipitation, the next step is to use suction filtration to filter the Ba sulfate precipitate. To do this, a filter flask is used because it can withstand pressure without breaking and helps speed up the filtration process.

It is important to ensure that the filter paper covers the entire base of the crucible to prevent dissolved materials from leaking during suction, which could result in loss of material or even breakage of the flask due to internal pressure. Additionally, using a rubber policeman can effectively transfer all particles from the beaker to the crucible, and it is more effective than a glass rod because it can cover a larger surface area, thus speeding up the process of dislodging particles.

It is important to remove the tubing from the filter flask before turning off the pump to avoid sudden pressure changes that could cause the filter paper to rupture. To dry and concentrate Ba sulfate, the crucible containing the precipitate was dried in an oven to evaporate any remaining moisture, leaving only the dried sample behind. Cooling the precipitate in

a desiccator helps prevent moisture in the surrounding air from being absorbed, as the desiccator regulates its humidity level while the precipitate cools. Finally, the crucible was weighed for its measurement.

The precipitation of barium sulfate from a given sulfate solution was carried out in a closed balance to measure an accurate weight of the gathered sulfate. The procedure involved pipetting 25mL of the given sulfate solution into a 250mL beaker, adding 50mL of H2O and 5 beads of concentrated HCl, heating and stirring the solution till boiling, and adding 10mL of 10% Ba chloride solution bead wise from a measuring cylinder.

After digesting for 20 minutes, the beaker was covered with a thicker glass. To test for complete precipitation, a few beads of Ba chloride were added to the clear supernatant liquid. The barium sulphate precipitate was washed and filtered by placing a filter paper over the entire base of the crucible. The decanted clear supernatant solution was then filtered into the pre-weighed crucible with filter paper. A "rubber-policeman" was used to remove any particles from the beaker, which was rinsed with warm deionised water. Finally, the contents were emptied into the crucible while using a vacuum pump.

The Ba sulfate precipitate underwent two rinses with deionized H2O under vacuum, and the filtrate was disposed of. The crucible housing the precipitate was subjected to a 150°C drying process for half an hour before being allowed to cool in a desiccator for ten minutes.

Experiment 4 involved determining the weight of Ba sulphate. This was achieved by subtracting the weight of a crucible with precipitate from the weight of a crucible with filter paper after it had

cooled down. The results were tabulated.

When 3337 grams is subtracted from 3088 grams, the result is 0.0249 grams of SO42-. The molarity of SO42- is 0.004268632 M. The concentration of SO42- in grams per liter is calculated by multiplying the molarity of SO42- by the molar weight of SO42- and is equal to 0.

According to the results, the weight of Ba sulfate was found to be 0.0249g and the concentration was 0.4098g/L. The precipitate of Ba sulfate was observed as white and powdery, as seen in online sources.

According to Texas A&M University, thoroughly rinsing the beaker and vacuum pump during filtration is essential to ensure that all the precipitate is collected and none is lost. This can significantly reduce the amount of impurities present, resulting in a higher yield of pure precipitate. Additionally, improper drying or insufficient drying time may result in moisture being present in the precipitate, which can also increase its weight.

It is possible that the precipitate still contains moisture, as our group has only completed one cycle of drying in the oven and chilling in the desiccators. To increase accuracy, we can repeat the drying process until a constant weight is achieved. Additionally, measurement inaccuracies may occur due to human error and environmental conditions, such as parallax errors when measuring the Ba chloride and sulphate solutions.

Reading the value at an incorrect angle can lead to incorrect concentration of the solution used. Furthermore, if the beaker was covered with a ticker glass during the digestion procedure and the final result was less than anticipated as explained in theory.

Possibleand unification:
If the final results are inaccurate and some sulfate has been

lost, it is probably due to incomplete dissolution of Ba chloride in the solution. Additionally, the precipitate loss may also result from inadequate rinsing into the crucible.

Not washing down any precipitate left in the beaker could result in the loss of precipitate, affecting the amount of sulfate obtained. Additionally, during the procedure involving heating and vigorous stirring, some of the solution may have accidentally spilled out.

This experiment familiarized my group with the hydrometric analysis method for determining the amount of a desired component present in a sample. Heating the H2O may cause some of the solution to evaporate, resulting in a loss of solution.

In order to determine the exact amount of a desired substance, a procedure is followed which involves precipitation, suction filtration, drying and weighing. The results of this process show that for Ba sulfate, the weight is 0.0249g and its concentration is 0.4098g/L.

The white and powdery precipitate is comparable to the origins of the online world, but it has a greater weight than some other products from different groups.

Insufficient or inadequate drying of the sample clip may have caused moisture to be present in the precipitate, which could have resulted in inaccurate recorded data. Nonetheless, despite this possible problem, the experiment was ultimately deemed successful. References: Dr.

The online resource by Nutts (2010) provides a definition of Gravimetric Analysis and includes information on the theory section. The source can be accessed via the hypertext transfer protocol link: http://www.chm.davidson.edu/ronutt/che115/viii_gravi.pdf. The text is presented in a HTML paragraph tag.The web page located at Dartmouth College's website, specifically the /~chemlab/techniques/vfiltration.html section, provides details about suction filtration relating to its theory. Additionally, the website at

laboratoryequipmentworld.com contains information regarding filtering flasks.

HTML - The implementation of a filtration flask (theory section) using Hypertext Transfer Protocol: //en.wikipedia.org/wiki/Gravimetric_analysis - comparing outcomes and methods with online sources (discussion section)

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