Neutralization Titration using a Strong Acid and Weak Base Essay

What mass of sodium carbonate is needed to make 250cm3 of a 0.0500 breakwater dm-3 response? What is the submerging of the Hydrochloric back breaker of 0.108 mols? This examine involves the making of a standard sodium carbonate solution and using the exact concentration of this solution to find the sinless concentration of an approximately 0.1mol Hydrochloric deadly solution using an indicator (Methyl Orange). We give be using the same amount of indicator and atomic number 11 Hydroxide solution for this experiment each time it is repeated to minimize any misunderstandings that may occur. It is expected that through this experiment we leave alone observe a coloring material change of the indicator from the Alkaline yellow, to a strong orange colored solution. We result be measuring the amount of Hydrochloric acid that is required each time this experiment is repeated to determine the concentration of the Hydrochloric acid.VariablesDependent variable1. The dependent variab le would be the Hydrochloric acid as the amount used will depend on the experimenters actionsIndependent variable1. the control variable is the experimenters eye and judgmentControl Variables1. the volume of atomic number 11 Carbonate in each titration2. the mole of the Hydrochloric acid used3. the mole of the Sodium carbonate solution used4. the indicator used (Methyl Orange)Materials and EquipmentPart A1. Anhydrous Sodium Carbonate (NaCO3)2. Deionized urine3. 100 cm3 Beaker4. 250 cm3 Volumetric Flask with stopper5. Small FunnelPart B1. Volumetric flask of 250 cm3 NaCO3 from part A2. 20.00 cm3 pipette3. Methyl orange indicator4. 50 cm3 Burette5. Small Beaker6. Hydrochloric Acid (HCl)7. 100 cm3 Conical flask(s)DiagramMethodPart A1. An amount of about 1.325g of anhydrous sodium carbonate was weighed and its mass recorded2. 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 do three times.4. Additional deionized water was added to a third of the volumetric flask and the stopped was applied and the flask was shaken to dissolve any remaining anhydrous sodium hydroxide solution.5. An additional 100 cm3 of deionized water was added and was mixed thoroughly6. 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 knowledge was recorded to the nearest 0.02 cm35. Hydrochloric acid was titrated against the indicated sodium carbonate solu tion until a color change from yellow to orange occurs. The final examination 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 reduce exposure to any chemical splashesData CollectionConcentration of HCl solution = 0.108 moldm3Uncertainties1. Burette 0.022. Pipette 0.063. plate 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 slowly changed from yellow to an apricot-like orange3. When access Hydrochloric acid was ad ded, the solution turned pinData ProcessingThe total amount of HCl used was 159.74 cm3 0.32cm3The average volume of Hydrochloric acid used is calculated as0.32cm3 payable to the observance of a wide spread area of results, I take selected three close results to be more accurate in my calculations. I puddle selected the spunkylighted pieces of data from figure 1The revised average is0.12 cm3To convert this to dm3 we divide by 1000, = 0.01846 dm3To calculate the moles I will use the formula=0.0125 molsI will find the concentration of sodium carbonate=0.05 mol dm-3Knowing that this equation is a one to one ratio I can assume that 0.05 mol of sodium carbonate will react 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 molecules. This will give me the moles of HClTo find the concentration I will use the formulaThe contribution difference is ca lculated asThe total hesitation in the whole of Part A and B isScale x1selected pipette x3Titre x3The percentage uncertainty of each piece of equipment isScalePipetteTitreTotal 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 works on the theory that when the correct amount of acid is added to a base to neutralize it, the pH will be equal to 7, and a color change will occur with an indicator. The percentage difference between my results and the expected results (given by the teacher) is 0.00%.EvaluationIn order to decrease any possible error, we have repeated the experiment 8 times in total. Through calculations, we have found that it was the scale that gave us the highest error percentage, thus causing a high overall unce rtainty. Any error that may have been caused when we were transferring the sodium carbonate to the conical flask, as a too much or too wee 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 example reading above the meniscus instead of below it. Parallax error is also a possibility this would cause the calculations and results to fluctuate. Systematic errors such as not zeroing the scale correctly 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 further improved my using a more accurate and reliable sort to measure the volume of the HCl that was released by using possibly an electronic measuring device that would be more accurate in readin g the scale. The random error can be minimized by performing the experiment a larger amount of times and selecting the best results to average. Another way to improve the experiment, would be to use an electronic magnetic stirrer to stir the substance whilst the titration is occurring to gain a more accurate time for stopping as the reaction will occur much faster due 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.