Data Collection Essay

* The Rough was excluded during the calculation of the mean as the raw was a running game to indicate the general where nighs of the end point, which is in accurate of the bring end point.Table 2. Observations collected during the look into. Table contains observations which were recorded during each trial of the experiment.TrialsObservationsBefore trials* When pissing was added to the crystals of oxalic loony toons, it dissolve almost instantly with a crystalize stirring of the beaker.Rough* When two con engrafts phenolphthalein was added to the solvent of atomic number 11 supplyd oxide, the get outant turned pinko.* afterwards adding about 20.8dm3 of oxalic pane into the sodium hydrated oxide firmness of purpose, while swirling the c iodin-shaped flaskful, the source turned wholly clear the oxalic acid was filled up to 21dm3 to swallow a rounded rough end point to flirt with.1* When two drops of phenolphthalein was added to the sodium hydroxide solution, the solution turned pink.* after(prenominal) adding about 20dm3 of oxalic acid solution, while swirling the conical flask gently, each drop of oxalic acid solution began to turn the pink solution reasonably clear.* After about 20.6dm3 oxalic acid solution was added, the pink solution turned completely clear.2* Two drops of phenolphthalein was added to sodium hydroxide solution, producing a pink dismal solution.* After about 20dm3 of oxalic acid solution was added, each drop began tour the pink solution fairly clear.* After adding around 20.4dm3 of oxalic acid solution, the pink solution turned completely clear.3* Two drops of phenolphthalein was added to the sodium hydroxide solution, turning the solution in the conical flask pink.* After adding about 20dm3 of oxalic acid solution, each drop began turning the pink solution slightly clear.* When about 20.3dm3 of the acid was added, the pink solution turned completely clear. info Processing1. Write an equivalence for the recept ion.(COOH)2 + 2NaOH 2NaCO3 + 2H2O2. What amount (in seawalles) of NaOH is present in 20.0 cm3 of 0.097 mol dm-3 sodium hydroxide solution?c = n/vc = 0.097mol dm-3 0.001= 0.097mols (0.001/0.097 x light speed%)= 0.097mols dm-3 1.03%v = 20.0cm3 0.04= (20.0/1000) (0.04/20.0 x 100%)= 0.020dm3 0.2%n = ?n = c x vn = 0.097 1.03% x 0.020 0.2%n = 0.00194 (1.03 + 0.2)%? n = 0.00194 mols 1.23%3. What amount of oxalic acid was present in the average volume mandatory to react exactly with the sodium hydroxide solution?Using the grinder ratio of 12 for acid base respectively0.00194 1.23% / 2 = 0.00097 mols? amount of oxalic acid present = 0.00097 mols 1.23%4. What amount of oxalic acid was present in your 250 cm3 volumetric flask?Concentration of acid in 250mL is the same as the assiduity of acid in 1L. on that pointfore the concentration of acid in 1 dm-3 of acid solution is the same as concentration of acid in 250mLc = n/vc = 0.01192.03% / 0.25 (0.15/250 x 100%)c = 0.0476 (2.03+0.06)%? c = 0.05 mols dm-3 2.09% (concentration of acid)c = n/v0.052.09% = n / 0.25 0.06%0.052.09% x 0.250.06% = n? n = 0.0125 (2.09 + 0.06)%? moles of oxalic acid in 250mL solution = 0.0125 mols 2.15%5. What is the softwood of hotshot mole of oxalic acid?n = m/MMMM = m/nMM = 1.5g 0.02 / 0.0125mols 2.15%MM = 1.5 (0.02/1.5 x100%) / 0.01252.15%MM = long hundred (1.33+2.15)%MM = 120 3.48%m = n x MMm = 1 x 1203.48%? luck of one mole of oxalic acid = 120g 3.48%6. How many molecules of peeing of crystallizing are present in one mole?MM of (COOH)2 = 2(12.01 + 32 + 1) = 90.04MM of H2O = (2.02 + 16) = 18.02(COOH)2.xH2O = 120g 3.48%? 90.04 + 18.02x = 120g 3.48%? 18.02x = 120g 3.48% 90.04? 18.02x = 29.963.48% (/18.02)? x = 1.66263.48%? Molecules of water of crystallisation = 1.660.06 finding and EvaluationDiscussion1. Estimate the degree of hesitancy in your narrations utilise the balance, the volumetric flask, the pipette and the burette. How accurately can you quote your answer? sleep = 0.02gVolumetric flask = 0.15mLPipette = 0.04cm3Burette = 0.15cm3The equipments use were relatively accurate as the uncertainties compared to the collected honors are small.2. Compare your answer with the chasten answer and work out the percentage error.Percentage error = ( observational value actual value) / actual value x 100%= (1.6626 3.48% 2) / 2 x 100%= 16.87% 1.74%3. arouse any other reasons for possible error.Other reasons for possible error acknowledge the incredulity of equipments, human errors and mistakes, possibility of contaminated solutions, air bubbles and transfer of solution between equipments.This experiment was conducted to find the ratio of water in hydrate oxalic acid crystals. This included calculations of the theoretical and experimental values for the ratio of water in the hydrate oxalic acid crystals and the percentage errors of values compared.The equation for the reaction between the sodium hydroxide solution (NaOH) and the oxalic acid solution ((CO OH)2) was worked out, with the intersection being a salt (NaCO3) and water (H2O). As the oxalic acid solution is a dibasic acid solution, the reaction ratio with sodium hydroxide is 12. The amount of NaOH, in moles, was also calculated by mul conclusionlying the concentration of the sodium hydroxide solution and the volume of sodium hydroxide solution apply. The equation c = n/v was used to calculate this. The result was 0.00194 moles of NaOH in the sodium hydroxide solution with an uncertainty of 1.23%. The amount of oxalic acid presented in the average volume required to react exactly with the sodium hydroxide solution was also calculated by dividing the moles of NaOH (0.001941.23%) by 2, based on the 12 reaction ratio stated before. The result was 0.00097 moles with an uncertainty of 1.23%.The amount of oxalic acid present in 250cm3 was also calculated. The concentration of acid in 250mL is the same as the concentration of acid in 1L, therefore, the concentration of acid in 1dm- 3 of the oxalic acid solution is the same concentration as the acid in 250mL. With this understood, the equation c = n/v was used once again. The concentration was first calculated by dividing the moles of NaOH by 0.25dm3.The result (0.05mols dm-3 2.09), was used in further calculations to determine the moles of oxalic acid by mul power pointlying the antecedent calculated concentration (0.05mols dm-3 2.09) with 0.25dm3, resulting in the moles of oxalic acid in the 250mL solution as 0.0125mols 2.15%. This value was used in the calculation of the mass of one mole of oxalic acid. The equation n = m/MM was used in this calculation. The MM (molar mass) was first calculated, dividing the mass of oxalic acid crystals by the moles of oxalic acid (1.5 / 0.0125). The mass (m = n x MM) was calculated with the result of this (1 x 1203.48%), resulting in the mass of one mole of oxalic acid being 1203.48%.Finally, the molecules of water of crystallisation presented in one mole were calculated. This was make by using the mass of one mole of oxalic acid (1203.48%), subtracting the MM of (COOH)2 (90.04) from it and dividing the result by MM of H2O (18.02). The concluding result of the number of molecules of water in crystallisation equalled 1.66 with an uncertainty of 3.48% or 0.06. With this final result, the percentage error was calculated, being 16.87%1.74%.all(a) the uncertainties within the values used were calculated into percentage with dividing the uncertainty by the value and multiplying it by 100%. The uncertainties were converted into percentages before doing calculations were done.There were several limitations found during this experiment which would have got been the cause of an outside final result the variableness between the theoretical value of 2 and the experimental value of 1.660.06. These limitations include the uncertainties of the equipment, human errors and mistakes, possibility of contaminated solutions, air bubbles found in solutions and the transference of solution between equipments. The significance of these errors and the improvements are listed in the table below.LimitationsSignificanceImprovementsUncertainty of equipmentsUncertainties were obtained during the experiment through the use of equipments. The inaccurate recording of data would have affected the results in the end. Eg. The readings on the electronic scale werent fully stable and consistent at one value, it varied increasing and decreasing slightly.In the case of the electronic scale, it was suggested that the variation in weight value was referable to the air-conditioning blowing down on it. The air-conditioner could be turned off to adulterate the uncertainties and variations. Students could also prevent themselves from breathing severely down onto the scale while measuring, this could have contributed to the variation as well. pitying errors and mistakesMistakes could affect the outcome and accuracy of results. Eg. While adding water into the volu metric flask to dissolve the oxalic acid crystals, a student out of the blue added a shortsighted too much, over the 250cm3 that was intended. This would have over diluted the oxalic acid.This could have been avoided through patience while adding the water into the volumetric flask. This could also have been done slowly and carefully, probably using a pipette towards the end at the 250cm3 mark.Reading the mea surement of the pipette, burette and volumetric flask could have been inaccurate, make results to be inaccurate and in turn affecting the calculations.Inaccuracy could have been payable to improper way of reading the beat. Students should have bent down slightly with the measurement at eye level. Students heads should not be tilted but level with the equipment as well. The measurement should also be read at the parallax, not above or below it. casualty of contaminated solutionsThe experiment was conducted with the use of several different solutions. These solutions could have accidentally been mixed in with each other, causing the solution to be contaminated. The results obtained due to this could have been inaccurate, affecting the final results.Being careful with the solutions used would tending avoid this. Using clean equipments for each different solution, making sure the solutions that are not meant to be placed together do not get mixed with each other.After the use of some of the equipments, they were to be washed and reused for another solution. The equipments were not dried before being used again this could have diluted the solution and contaminated it.Drying the equipment each succession after it is washed/cleaned would prevent access water and dilution of solutions.Air bubblesWhen transferring the dissolved oxalic acid into the burette, there were some tiny air bubbles. This would have because the measurement to be inaccurate as the air bubbles would have caused the reading of the solution to be great than it actually is. Over time wh en the bubbles removed itself from the solution which would have caused a decrease in solution. The inaccurate measurement reading would have affected the final results of the experiment.The burette could have been left alone for awhile to allow the bubbles to float to the top. Whatever the amount the bubbles made up for, fill the burette up again with the use of a pipette. carry-over of solution between equipmentsWhen transferring solutions between two or more differing equipments would have caused an increase of decrease in measurement. An inaccurate amount of solution would have affected the results or recorded data.When using a funnel shape during the transference of solution into the burette, it caused some increase in the in demand(p) amount. This is due to the tip of the funnel having some drops of solution left in it and when the funnel was removed, the relocation could have caused those drops to drop into the burette, causing an increase in amount of solution. This could be prevented by either slowly removing the funnel or using the funnel up to a certain mark, remove it and fill up to the desired amount with the use of a small pipette drop by drop.When using the 20mL pipette to transfer the sodium hydroxide into the conical flask, the tip of the nozzle had a drop that was tempted to drop out of the pipette. Avoid pitiful the sides and move the pipette over the flask slowly would reduce the chances of it fall out and altering the volume of solution.A small amount of the solution was also stuck at the tip of the nozzle after being emptied. By touching the tip to the side of the flask would help that tiny second of solution flow out. If possible have the nozzle flat on the side of the flask, this would allow it to flow out smoothly.To avoid or reduce these significant errors, these solutions and improvements should be taken into consideration during future repetition of this experiment.The experiment overall was invalid. Though the values in data collection may have been to a 0.10cm3 difference, the final calculation of the percentage error, 16.87%1.74%, was much greater than the desired 1% causing the experiment to be invalid.