Neutralization Titration using a Strong Acid and Weak Base Essay

What circumstances of atomic number 11 change is needed to practise 250cm3 of a 0.0500 gram bulwarkecule dm-3 outcome? What is the absorption of the Hydrochloric sour of 0.108 mols? This prove involves the making of a standard sodium change solvent and using the exact concent balancen of this solvent to find the spotless concentration of an virtually 0.1mol Hydrochloric superman response using an power (Methyl Orange). We exit be using the very(prenominal) tax of index and Sodium hydrated oxide resolvent for this essay to each one clip it is repeat to minimize any illusions that whitethorn occur. It is expected that done this test we allow for observe a food coloring tack of the indicator from the Alkaline yellowish, to a grueling orangeness colored solution. We leave alone be measuring the issue forth of Hydrochloric blistering that is infallible each cadence this experiment is repeat to determine the concentration of the Hydrochloric acid .VariablesDependent variant1. The dependent variable would be the Hydrochloric acid as the amount employ exit depend on the experimenters actions breakaway variable1. the control variable is the experimenters eye and judgmentControl Variables1. the bulk of Sodium change in each titration2. the seawall of the Hydrochloric acid employ3. the mole of the Sodium carbonate solution employ4. the indicator used (Methyl Orange)Materials and Equipment musical composition A1. Anhydrous Sodium Carbonate (NaCO3)2. Deionized pee system3. 100 cm3 Beaker4. 250 cm3 Volumetric Flask with nag5. Small Funnel dissolve B1. Volumetric flaskfulful of 250 cm3 NaCO3 from part A2. 20.00 cm3 pipet3. Methyl orange indicator4. 50 cm3 buret5. Small Beaker6. Hydrochloric panelling (HCl)7. 100 cm3 Conical flask(s)Diagram systemPart A1. An amount of virtually 1.325g of anhydrous sodium carbonate was weighed and its battalion record2. The anhydrous sodium carbonate was then dissolved in a small amount of deionized water and was transferred to a 250 cm3 volumetric flask using a small funnel.3. Using small amounts of deionized water, any residual sodium carbonate solution was washed into the flask. This was done three generation.4. spare deionized water was added to a third of the volumetric flask and the stopped was applied and the flask was shaken to dissolve any rest anhydrous sodium hydroxide solution.5. An special 100 cm3 of deionized water was added and was mixed good6. The flask was then filled with deionized water up to the 250 cm3 markPart B1. The 20 cm3 pipette was rinsed with sodium carbonate solution from part A. then 20.00 cm3 of sodium carbonate solution was transferred through the pipette into a 100 cm3 conic flask2. 2 drops of methyl orange indicator was added to the conical flask3. The 50 cm3 Burette was rinsed with approximately 0.1 mol hydrochloric solution then was filled with hydrochloric acid4. The initial burette nurture was recorded to the nearest 0.02 cm35. Hydrochloric acid was titrated a sort outst the indicated sodium carbonate solution until a color change from yellow to orange occurs. The final burette reading was recorded to the nearest 0.02 cm36. This experiment was identically repeated until three concordant results were obtainedSafety1. A lab coat must be worn when performing this experiment to compress exposure to any chemical splashes info CollectionConcentration of HCl solution = 0.108 moldm3Uncertainties1. Burette 0.022. Pipette 0.063. Scale 0.0014. titre 0.04Amount of Anhydrous Sodium Carbonate weighed = 1.325 0.001Amount of Sodium Carbonate solution used = 20 cm3Physical observationsPart A1. When the anhydrous sodium carbonate was mixed with the deionized water, we saw no color change in the water and the sodium carbonate dissolved completelyPart B1. The sodium carbonate solution was clear, when the indicator was added it became a strong yellow color2. When the hydrochloric acid was added the color behind change d from yellow to an apricot-like orange3. When access Hydrochloric acid was added, the solution turned pin entropy ProcessingThe total amount of HCl used was 159.74 cm3 0.32cm3The average volume of Hydrochloric acid used is noted as0.32cm3Due to the service of a wide spread domain of a function of results, I wee selected three cosy results to be more accurate in my calculations. I discombobulate selected the steeplighted switchs of info from anatomy 1The revised average is0.12 cm3To replace this to dm3 we divide by 1000, = 0.01846 dm3To calculate the moles I pull up stakes use the formula=0.0125 molsI leave alone find the concentration of sodium carbonate=0.05 mol dm-3Knowing that this equating is a one to one ratio I can assume that 0.05 mol of sodium carbonate will play off with the same number of mols of HCl.The HCl titre of NaCO3 will be calculated usingdm3I will multiply this by 2 as for every sodium carbonate molecule reacted, I will have 2 Hydrochloric acid mo lecules. This will get around me the moles of HClTo find the concentration I will use the formulaThe share diversion is calculated asThe total doubtfulness in the whole of Part A and B isScale x1selected pipette x3 titer x3The percentage uncertainty of each piece of equipment isScalePipetteTitre be percentage uncertainty isThe absolute uncertainty for the concentration is-3ConclusionThe aim of the experiment is to calculate the unknown concentration of HCl through titration using a strong-acid and a weak-base. The calculated result for the concentration of the HCl is 0.149 0.010 mols dm-3. This experiment deeds on the theory that when the correct amount of acid is added to a base to rot it, the pH will be relate to 7, and a color change will occur with an indicator. The percentage difference amongst my results and the expected results (given by the teacher) is 0.00%.EvaluationIn order to decrease any possible erroneous belief, we have repeated the experiment 8 times in to tal. Through calculations, we have found that it was the scale that gave us the highest fracture percentage, thus do a high overall uncertainty. Any error that whitethorn have been caused when we were transferring the sodium carbonate to the conical flask, as a too often or too little amount may have been taken causing the results to fluctuate. Another reason that there may have been an inaccuracy could have been because of human error in reading the scale wrong, for utilization reading above the meniscus alternatively of below it. Parallax error is also a possibility this would cause the calculations and results to fluctuate. Systematic errors much(prenominal) as not zeroing the scale decently could lead to significant fluctuations in the measurements, or slight inaccuracies to a more accurate reading. However, in this case, there was no percentage error in the results.Improving the experimentAlthough the results had 0% error, the experiment could be boost repaird my using a more accurate and reliable way to measure the volume of the HCl that was released by using by chance an electronic measuring device that would be more accurate in reading the scale. The random error can be minimized by performing the experiment a larger amount of times and selecting the outgo results to average. Another way to improve the experiment, would be to use an electronic charismatic stirrer to stir the substance whilst the titration is occurring to polish off a more accurate time for stopping as the reaction will occur much faster payable to the continuous constant motion of the stirrer.The best way to fix this type of error is to obtain more accurate scales to measure the substances. Or to have a data logger, with a pH probe to gain accurate readings for the neutralization.