PH Titrations Lab Report Example | Topics and Well Written Essays - 1000 words

PH Titrations - Lab Report ExampleIn the chemistry of vitriolics and bases, titration is used in determine the value of pH for different solutions (Verma, D. 2006). Whenever we carry out an acid-base titration, an indicator is normally used in copulation whether the solution is an acid or a base. In other cases an indicator whitethorn change its put one over a process that is described as a titration end point. In many cases, vividness changes may be observed in mixing ii solutions together in the proportions that are exact. Such a mixture may be defined as an equivalence point. In order to gain to a greater extent understanding on titrations, an experiment was set to investigate the pH values for different solutions. Hypothesis The speculation of the study was to determine the pH at the equivalence point and the un cognise concentration of the acids Aim The role of the study was to find out the pH at different points of the unknown acids concentration. Methodology. Apparatus. The instruments and the apparatus used in this study include Bulb Pipette, burette, conical flask, 3 substances HCl, NaOH, and CH3COOH, beaker, electrode, Magnetic, stirrer, and the pH thou. Procedure The burette was filled with 1,0 groin of sodium hydroxide dm-3 up to a zero mark. The conical flask was also filled. About 25cm3 of 0.1 moldm-3 of HCl was added victimisation a pipette. The flask was placed on a magnetic stirrer, and the stirrer dropped back into the flask. The stirrer was turned on in the medium to avoid movements of the bar to hit the glass. The titration was them started with a similar volume to that in the table. After each titration the pH for each solution was recorded. The process was repeated for vinegar and hydrochloric acid. The collected info was presented in table 1 and 2 in the results section. Table 1 pH values for HCl V of NaOH PH of HCl 0 1,86 1 1,91 2 1,98 2.5 2,03 3 2,09 3.5 2,22 4 2,43 4.2 2,53 4.4 2,74 4.5 2,96 4.6 3,29 4.7 5,10 5 10,85 5.5 11 ,44 6 11,64 7 11,46 CV=CV NaOH Acid HCl 4,7x0,514=25xC C of HCl=0,0966 Table 2 pH values of CH3COOH V of NaOH PH of CH3COOH 0 2,91 1 3,76 2 4,36 2.5 4,58 3 4,84 3.5 5,10 4 5,70 4.2 6,38 4.4 10,15 4.5 10,60 4.6 10,75 4.7 10,90 5 11,10 5.5 11,43 6 11,61 7 11,81 NaOH CH3COOH 4,3x0,514 = 25xC C of CH3COOH=0,0884 Graph 1 A graph of base versus strong acid Graph 2 A graph of a weak acid and a base. Discussion In this experiment the set up was used in calculating the quantity of the acid that is unknown inside the receiving flask through measuring the quantity of the autocrat or the base taken for the acid to be neutralized. In many cases, there are two categories of methods used to identify a neutralized solution. The first method involves using a pH meter inside the receiving flask and adding the base up to when the value of the pH reads 7. Another method uses an indicator (Matar, S. 2001). In this case, an indicator is a base or an acid having a conjugate base or acid with a color diffe rent from that of a compound that is original. There would be some changes in the color when the solution has a one to one ratio of the mixture of the different forms of colored indicators. From the equation of the Henderson-Hasselbatch, the pH of the solution would be equated to the pH of the indicator when the indicators end point is realized. At this point, the solutions pH and the titrands volume would be identified, and the amount of base needed for neutralization of the solution that is not known can easily be deduced. The obtained data was