Determining the Concentration of Calcium Carbonate in an Unknown Substance through the Methods of Titration Aim Essay

trammel the absorption of the unfathomable ethanoic point root word by titrating with a known concent dimensionn of atomic number 11 hydrated oxideEquipment and Materials* Unknown ethanoic acetous* 50cm3 buret* 250cm3 Erlenmeyer flask* 100cm3 beaker (for CH3COOH)* cccm3 beaker (for NaOH)* 100cm3 beaker (for waste)* Standardized atomic number 11 hydrated oxide response* Burette clinch* Retort stand* Phenolphthalein indicator* 50cm3 gradational cylinder* Distilled wet supply (to rinse the flask) partTo begin with, obtain approximately 200 cm3 of sodium hydrated oxide solution. Then, set up the retort stand and buret squeeze as indicated in the diagram below. use twain 10 cm3 aliquots of the NaOH solution, rinse the buret twice. Next, fill to above the 0.00cm3 mark and drain land to below the 0.00cm3 mark in graze to remove any atmosphere bubbles. After that, transfer 50 cm3 of the unknown point into the 250cm3 flask. Into the same flask, place 2 drops of the p henolphthalein indicator. Fin tout ensembley, tote up sodium hydroxide from the burette until you reach the termination.Procedural NotesTo accommodate for the sodium hydroxide that splashes to the sides of the flask, distilled water was used. Using the distilled water on the sides of the flask was rinsed sight to summate the sodium hydroxide to the rest of the solution in the flask. Also, when dropping a half-drop into the flask, the quest procedure was used First, a half-drop was do at the tip of the burette. Then, using the flask, the half-drop was dispassionate to the flasks side. Finally, using the distilled water, the half-drop was rinsed down to the rest of the solution.To make it easier to recognize the endpoint of the reaction, a white paper was plant under the flask. This way, it was easier to recognize when the solution changed color. card (selective information Collection)Quantitative DataMeasurements Recorded During the essayTrial123*4*Initial Burette discipli ne (ml?0.02ml)0.200.420.100.23Final Burette Reading (ml?0.02ml)45.7045.9345.3945.30 deal of Ethanoic Acid Used (ml?0.04ml)50.0050.0050.0050.00*To gain the results, audition 3 and 4 was taken from another(prenominal) group to live on more data, thereby increasing the accuracy of the data.Qualitative DataDescriptions of the Substances Used and ProducedSodium Hydroxide take solution, low viscosity, slipperyEthanoic venereal disease gain solution, acidic,Phenolphthalein indicatorClear solution, comes in bottle, add as dropsSolution Produced (NaCH3COO(aq) + H2O)Clear/ intercept throughout, trail 4 was the closely victorious as it was closest to straighten than all other trails. Volume of political campaign 1 was greatest as a covey of water was used in order to wash down the sodium hydroxide stuck to the side of the flask.Data AnalysisThe neutralisation reaction reaction between sodium hydroxide and ethanoic acid isSodium Hydroxide + Ethanoic acid Sodium Ehthanoate + WaterThe refore, the molar ratio is 1 mole of sodium hydroxide to 1 mole of ethanoic acid. Sodium hydroxide is known to have a parsimony of 1.003 mol dm-30.004 mol dm-3.Consequently, the following represents the calculations to restrict the immersion of ethanoic acid in exertion 1Using similar calculations, the concentration of ethanoic acid for trials 2,3, and 4 were calculated as well. The following table represents the results.Results for the calculations of the concentration of ethanoic acid used in each trialTrialConcentration of CH3COOH / mol dm-3 CH3COOHUncertainties / %10.9131.320.9131.330.9091.340.9041.3 bonny0.9101.3ConclusionIn conclusion, the result of this testing ground indicates that the concentration of CH3COOH is 0.910 mol dm-3. Using this re appreciate, and the veridical measure out of ethnoic acid, 0.9190 mol dm-3 0.0004 mol dm-3, pct flaw was calculated as followsWith this, we see that the portion of uncertainties is greater than the portion wrongful conduct. The percent of uncertainties represents the random errors, in which the measured value can either be bigger or smaller than the accepted value, collectible to an imprecise measurement. To meliorate these random errors, it is requisite to use more precise equipment and/or repeat measurements. One example of this would be to use a pipette preferably of a gradational cylinder, especially because ?0.4 cm3 is a relatively large uncertainty. Consequently, the use of such equipment led to the percent of uncertainties being greater than the percent error. This means that the random errors overcome for the errors in this research science lab. However, there are a couple potential self-opinionated errors that should be appointed in this lab. The biggest maven would be that it is hard to get to the endpoint, where the solution is merely pink. In all trials, the solution became candid pink.However, it was only in trial 4 that the solution was truly ambiguous to whether it was pass ably pink. The worry of getting to this ambiguous clear pink is definitely a organized error as it endlessly leads to a larger ledger of sodium hydroxide used to react. One way to amend this whitethorn be to perform the lab in a longer date span. When I performed the lab, I felt pressured to get a sufficient measure of trials do within the class period. By reach the season span of the lab, it may be possible to take more time and get better quality results. A more realistic reformment may be to record measurements more ofttimes when approaching the endpoint. This would give us two measurements that the endpoint lies within, religious serviceing us reckon where the endpoint actually is.However, improving this error would lead to a smaller volume of sodium hydroxide, a smaller value for the concentration of ethanoic acid, which would make the observed value further from the true value. Another systematic error in this lab is the sodium hydroxide splashing to the sides of the flask. Although using water to rinse the sodium hydroxide down was aimed to cover this, another way to improve this may be to use equipment with a wider mouth, such as a beaker, kinda of a flask. Once again, improving this error would lead to a greater percent error for the same reasons as the difficulty of getting an ambiguous pink color.Next, although it most likely did not affect the results in this lab, there is a question to whether launder the burette two times is sufficient. To improve this, it may be suggested that rinsing the burette 4 times is more sensible, evening though it is time consuming. A last(a) systematic error comes when transferring the ethanoic acid from the graduated cylinder. When this happens, some of the ethanoic acid may be retained in the graduated cylinder. This is a systematic error as this always leads to a smaller volume of ethanoic acid than measured. To improve this error, one may pour out a tiny bit more than 50 ml of ethanoic acid, and m easure that as 50 ml of ethanoic acid. Improving this error leads to a larger volume of ethanoic acid, a lower concentration of ethanoic acid, and once again, an increase in percent error.All in all, it is very interesting how knowing the amount of one substance can help determine the amount of another substance, although it is a topic that appears frequently in chemistry. In this case, knowing the number of moles of sodium hydroxide enabled us to know the concentration of the ethanoic acid. Furthermore, this lab helps one enhance their knowledge on the difficulty of setting up a lab. By reviewing and understanding the errors to a lab, one can relate the improvements to future labs. In a nutshell, this lab exemplified the process of titration, and how effective it can be.