Concocting Barium Sulfate Essay Example for Free

Concocting atomic number 56 sulfate EssayIntroductionBarium Sulfate is a white stub, liquid or solid, with the chemical formula being BaSO4. Barium sulfate is a radiopaque agent, which is purposed in order to serve x-rays be more visible due to the contrast between the barium sulfate and the x-rayed parts of the body. This substance is dangerous, but due to its poor solubility inlet will not result in the bodys absorption of the toxicity of it. Some of the dangers of ingesting Barium Sulfate however are bloating, constipation, cramping, diarrhea, nausea/vomiting, stomach/lower abdominal muscle pain, tightness in chest, troubled breathing, or wheezing. Barium Sulfate also reacts violently with Aluminum powders. Prolonged exposure to Barium Sulfate dust flush toilet result in baritosis, which is a form of benign pneumoconiosis. Barium Sulfate is insoluble in most substances, except for concentrated sulfuric acid.Research principalAn ample research question for this particu lar lab would be How can one create five chiliads of Barium Sulfate? This task explores the use of knowledge of different chemicals regarding their solubilities, concentrations and characteristics and the use of this knowledge in order to make a pre-determined five grams of Barium Sulfate. I intended to approach this problem by utilize my knowledge of chemicals stated above to come up with a simple, practical way of concocting five grams of Barium Sulfate.HypothesisIf Barium Nitrate and Sulfuric acidulent are combineed together appropriately, then we will be able to make five grams of Barium Sulfate, along with the other product. This hypothesis is clearly justifiable. If you meld 5.6 grams of Barium Nitrate with 2.1 grams of Sulfuric Acid, through the reaction types we can see that this is double replacement and should form HNO3 + BaSO4, and through some dilution calculations we can see that theoretically five grams of Barium Sulfate should be made.VariablesIndependent The am ounts of Barium Nitrate and Sulfuric acid. These variables are independent because they will channelize depending on what substances are use to make the Barium Nitrate and of what concentration.Dependent The amounts of Barium Sulfate and Nitric Acid produced. These variables are dependent because they depend on the independent variables, or the Barium Nitrate and Sulfuric Acid.Control The different materials use during the experiment are the materials used and the substances used to make the Barium Nitrate. These are controls because they do not change throughout the experiment.ProcedureMaterials 2 700mL beakers 50mL graduated cylinder 100mL graduated cylinder Stirring rod Digital Scale Coffee Filters Hot plate vacuity Flask 12.5 M H2SO4 Ba(NO3)2 FunnelSteps1. The true first step of this lab was to figure out how to make Barium Sulfate. In our case, we figured we would mix Barium Nitrate and Sulfuric Acid to do the trick. After subsequent calculations, we figured out that we would need 2.1g of Sulfuric Acid and 5.6g of Barium Nitrate.2. First we hardened 5.6 g of Ba(NO3)2 solid powder into the 700mL beaker3. We then proceeded to make it into a liquid by adding approximately 100mL of water, and to better dissolve these two substances we put the solution onto a hot plate and stirred until it was sufficiently dissolved4. Then we put 2.1g or 4mL of 12.5M H2SO4 into the 50mL graduated cylinder5. Then we diluted the 12.5M H2SO4 to 5M by adding in 6mL of water, in order to achieve 10mL of 5M H2SO46. We then poured the dissolved water and Ba(NO3)2 along with the 10mL of 5M H2SO4 together in the other 700mL beaker7. We then observed the reaction and recorded these observations. The solution was HNO3 and BaSO4, with the BaSO4 a white precipitate in the liquid HNO3.8. To isolate the BaSO4, it needs to be separateed. We weighed the coffee filter out with the digital scale, which came out to 0.5g and then placed the filter on the inside of the funnel.9. Place the funne l over the vacuum flask so that the HNO3 will go through the funnel into the vacuum flask and the remaining substance will isolated BaSO4 after the substance from the 700mL beaker is poured into the funnel very slowly10. Remove the coffee filter, and throw everything else out. Then let the BaSO4 on the coffee filter dry overnight11. Then we weighed the coffee filter with the dry BaSO4, which was 4.7g, and then subtracted the weight of the coffee filter to get the true weight of our BaSO4, which was 4.2 grams.Data mad DataAmounts of Reactants and Amount of BaSO4SubstanceAmount (+/- 0.5g)H2SO410mlBa(NO3)25.6g in 100mL of waterBaSO44.2 gramsCalculationsAmount to Use of Each Substance5g of BaSO4 x (1mol BaSO4/ 233.43g of BaSO4)0.02142 mols BaSO40.02142 mols BaSO4 x (1mol H2SO4/ 1mol BaSO4)0.02142 mols H2SO40.02142 mols BaSO4 x (1mol Ba(NO3)2/ 1mol BaSO4)0.02142 mols Ba(NO3)20.02142 mols H2SO4 x (98.078g H2SO4/ 1mol H2SO4)2.101g H2SO40.02142 mols Ba(NO3)2 x (261.336g Ba(NO3)2/1mol Ba(NO3 )25.597g Ba(NO3)2Dilutiono M1 V1=M2V2 (12.5M H2SO4)(Xml H2SO4) = (5M H2SO4)(10mL H2SO4) X = 4mL H2SO4 6mL of water needed for 4mL H2SO4Percent Yield(4.2g BaSO4/5g BaSO4) x 100 = 84%Percent Error(4.2g BaSO4 5g BaSO4)/ 5g BaS04 x 100 = 16%Diagrams all in all of our equipment laid outThe vacuum flask pulling the Nitric Acid out of the Barium SulfateThe finished, dried, Barium Sulfate on the coffee filterWeighing the Barium Sulfate on the coffee filterConclusionPrincipally, the lab was a success. We were able to come up with a perfectly ripe(p) method of creating Barium Sulfate. Technically, however the lab was slightly off. Instead of coming up with the ideal five grams of Barium Sulfate, we fell 8/10ths of a gram short, which came out to a sixteen percent error. This inaccuracy suggests that something in our lab went awry. When pumping the nitric acid out of the barium sulfate, we overflowed the filter on the vacuum flask, seeing as how we didnt take into account how thick the subst ance actually was. This mishap was most likely the largest contributor to our inaccuracy. Also, human error is always a factor. Inevitably, somewhere complicate the line we took a reading wrong or something of that nature, further skewing our results.This lab brought up a few questions for further investigation. After finishing the lab, the question occurred to me, if we had used an alternate method to make five grams of Barium Sulfate, could we have been more accurate, less(prenominal) accurate, or would our results have remained the same?To make a better lab, on that point are a couple things that could be done. First would be to take better care to observe the substances we work with much more carefully. By doing this, at that place is less likely of a chance of having something happen such as overflowing the funnel. Also, one could record observations better. This would make the analysis of the lab much easier, with less guesswork to do.