solutions should be mixed with ethanol and stored for 14 days at standard conditions of temperature and pressure (Hayes p. 7). 2.2.5 Preparing Standard Stock Solutions of Florfenicol A stock solution of 1.0 mg/mL florfenicol should be used to develop calibration standards (at least 4) for the samples to be examined (Hayes p. 8). The standard solutions of florfenicol should be tightly stoppered for 14 days at r.t.p. Table 1 illustrates the typical serial dilutions. Table 1: Sample Dilution Scheme (Courtesy:
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solution‚ and mixing well. A single beam Agilent technologies CARY60-UV-Vis Spectrophotometer was then employed to determine the optimum wavelength in the visible spectrum of the ionic Iron and FerroZine® complex. 1.2: Calibration Curve of ionic Iron and FerroZine® complex
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Solution 1. Prepare 250m1 0.1 M HCl solution from the 6 M stock solution provided. Calculation: (6 M) (?ml) = (0.1 M) (250 ml) 2. Prepare the solution by adding approximately l00ml distilled water to the 250 ml volumetric flask‚ pipetting the calculated volume of stock 6 M HC1 solution into the flask‚ and diluting to the mark with distilled water. Apply parafilm to the flask top and invert and shake to assure mixing. Part B - Standardization of HC1 Solution
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half-equivalence point where pH=pKa. In addition to the pH‚ Ka is an indication of an acids strength; pKa = - log Ka. B. The potential sources for errors in this experiment are the inconsistent and miscounting of drops of NaOH in the titration. The pipet must be held upright dispensing the exact size drops to have an accurate measurement. C. If your experimental Ka is 5.3 and the actual Ka of your unknown acid is 4.7‚ what is your %
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spectrophotometric analysis. Acidified solutions (using 0.1 M HCl) of FeCl3 and KSCN were prepared for the calibration of the UV-Vis spectrophotometer (using standard solutions) and the determination of Keq of the Fe(SCN)2+ formation (solutions with unknown concentrations). Absorbance readings of the standard and unknown solutions were obtained through the spectrophotometer. The equation of the trend line of the calibration curve (obtained through the plot of the absorbance readings vs. thiocyanatoiron (III) ion
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Calibrated glassware and balances were used to make sure all measurements were very accurate. We shook the prepared solution to ensure that they were homogeneous. To obtain concordant results we repeated the titrations. The results that we recorded were calibrated to three decimal places to ensure accuracy. We ensured that all washing was transferred to volumetric flasks. When using the potassium manganate we took readings from the top
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absolute zero - a theoretical condition concerning a system at zero Kelvin where asystem does not emit or absorb energy (all atoms are at rest) accuracy - how close a value is to the actual or true value; also see precision acid - a compound that‚ when dissolved in water‚ gives a pH of less than 7.0 or a compound that donates a hydrogen ion acid anhydride - a compound with two acyl groups bound to a single oxygen atom acid dissociation constant - an equilibrium constant for the dissociation of
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Quantitative and Qualitative analysis Ensuring accuracy in both quantitative and qualitative methods. Accurate data collection is essential in maintaining the integrity of research. Working accurately greatly decreases the possibility of an error occurring in an experiment‚ provides a greater chance of producing expected results and provides knowledge gained only from proven results. Quantitative methods generate numerical data or data that can be transformed into useable statistics. It is used
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B and G. Each of the concentrated pigments was dabbed onto their respective rows on each of the three TLC plates using a plastic pipet tip. 3 TLC chambers were prepared using 7mL of each different mobile phase (9:1‚ 8:2 and 7:3 pet ether: acetone solution). The TLC’s were performed and Rf values were measured. All materials were disposed of properly and all glassware was cleaned following correct laboratory
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Solubility and Stoichiometry I. Introduction The first purpose of this experiment is to apply solubility rules to choose two of eight given reactants to do a precipitation reaction. The second purpose is to use stoichiometry to calculate how much of a reactant will be used in a precipitation reaction‚ assuming that the amount of product is given‚ and to figure out the actual yield vs. the theoretical yield and to calculate the percent yield. The other purpose of this experiment is to practice the
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