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

Determine the parsimoniousness of the unknown ethanoic acid solution by titrating with a known concentration of atomic number 11 hydrated oxideEquipment and Materials* Unknown ethanoic acid* 50cm3 burette* 250cm3 Erlenmeyer flask* 100cm3 beaker (for CH3COOH)* 200cm3 beaker (for NaOH)* 100cm3 beaker (for waste)* Standardized atomic number 11 hydroxide solution* Burette hug* Retort stand* Phenolphthalein indicator* 50cm3 receive cylinder* Distilled pissing (to moisten the flask)ProcedureTo begin with, obtain approximately 200 cm3 of sodium hydroxide solution. Then, set up the retort stand and burette clamp as indicated in the diagram be suffering. Using two 10 cm3 aliquots of the NaOH solution, rinse the burette twice. Next, fill to above the 0.00cm3 visage and drain vote out to below the 0.00cm3 mark in order to remove any air bubbles. After that, channel 50 cm3 of the unknown acid into the 250cm3 flask. Into the same flask, place 2 drops of the phenolphthalein indicator. Fi nally, make sense sodium hydroxide from the burette until you reach the depot.Procedural NotesTo accommodate for the sodium hydroxide that splashes to the sides of the flask, distilled water was employ. Using the distilled water on the sides of the flask was rinsed raft to bring the sodium hydroxide to the rest of the solution in the flask. Also, when falling a half-drop into the flask, the following procedure was procedure of goods and servicesd First, a half-drop was made at the tip of the burette. Then, using the flask, the half-drop was collected to the flasks side. Finally, using the distilled water, the half-drop was rinsed big m angiotensin converting enzymey to the rest of the solution.To make it easier to recognize the endpoint of the reaction, a white make-up was put under the flask. This way, it was easier to see when the solution changed color.Observation ( entropy Collection)Quantitative DataMeasurements Recorded During the ExperimentTrial123*4*Initial Burette Reading (ml?0.02ml)0.200.420.100.23Final Burette Reading (ml?0.02ml)45.7045.9345.3945.30 intensity level of Ethanoic Acid Used (ml?0.04ml)50.0050.0050.0050.00*To increase the issues, trial 3 and 4 was taken from another group to get much data, on that pointby increasing the the legitimate of the data.Qualitative DataDescriptions of the Substances Used and ProducedSodium HydroxideClear solution, low viscosity, slipperyEthanoic acidClear solution, acidic,Phenolphthalein indicatorClear solution, comes in bottle, play as dropsSolution Produced (NaCH3COO(aq) + H2O)Clear/pink throughout, trail 4 was the close to successful as it was closest to clear than all other trails. mess of trial 1 was greatest as a lot of water was used in order to wash down the sodium hydroxide stuck to the side of the flask.Data AnalysisThe neutralization reaction between sodium hydroxide and ethanoic acid isSodium Hydroxide + Ethanoic acid Sodium Ehthanoate + pissingTherefore, the gram moleculear ra tio is 1 mole of sodium hydroxide to 1 mole of ethanoic acid. Sodium hydroxide is known to have a concentration of 1.003 mol dm-30.004 mol dm-3.Consequently, the following represents the calculations to determine the concentration of ethanoic acid in trial 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 / %10.9131.320.9131.330.9091.340.9041.3Average0.9101.3ConclusionIn conclusion, the result of this lab indicates that the concentration of CH3COOH is 0.910 mol dm-3. Using this apprize, and the actual value of ethnoic acid, 0.9190 mol dm-3 0.0004 mol dm-3, pct misunderstanding was calculated as followsWith this, we see that the portion of uncertainties is greater than the percent defect. The percent of uncertainties represents the r andom fallacys, in which the measured value can either be bigger or little than the accept value, due to an imprecise measurement. To improve these random errors, it is necessary to use more precise equipment and/or repeat measurements. One example of this would be to use a pipette instead of a calibrated cylinder, especially because ?0.4 cm3 is a relatively large uncertainty. Consequently, the use of such equipment led to the percent of uncertainties beingness greater than the percent error. This means that the random errors cover for the errors in this lab. However, there are a couple potential systematic errors that should be prescribed in this lab. The biggest one would be that it is hard to get to the endpoint, where the solution is yet pink. In all trials, the solution became clear pink.However, it was only in trial 4 that the solution was truly ambiguous to whether it was slightly pink. The difficulty of acquiring to this ambiguous clear pink is definitely a systematic error as it always leads to a larger pot of sodium hydroxide used to react. One way to improve this may be to action the lab in a longer time span. When I performed the lab, I felt pressured to get a sufficient amount of trials done in spite of appearance the class period. By stretching the time span of the lab, it may be possible to take more time and get better persona results. A more realistic improvement may be to bear witness measurements more frequently when approaching the endpoint. This would give us two measurements that the endpoint lies within, helping us estimate where the endpoint actually is.However, improving this error would lead to a littler 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 thi s, another way to improve this may be to use equipment with a wider mouth, such as a beaker, instead of a flask. erstwhile 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 principal to whether rinsing the burette two times is sufficient. To improve this, it may be suggested that rinsing the burette 4 times is more sensible, even though it is time consuming. A final 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 a tiny bit more than 50 ml of ethanoic acid, and measure that as 50 ml of ethanoic acid. Improving this error leads to a larger volume of ethan oic 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 arouse 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 useful it can be.