Analytical Chemistry for Technicians, Essay Example

In the experiment a spectrometer will be applied in order to ascertain the amount of a colored substrate that is produced when the Fe (NO₃)₃(aqueous) reacts with the Phenol derivative. This hypothesis will be examined by conducting an experiment with a collection of solutions in which the saturation of the Fe ⁽NO₃)₃ and 5- sulfosalicyclic acid will be varied. The intensity of the blue of the solution that results from the Fe (NO₃)₃ and the  5- sulfosalicyclic acid will be applied in order to ascertain the stoichiometric proportion of which of the reagents have been applied. The most deeply hued solutions should be distinguishable by eyesight. Notwithstanding, a spectrometer will be applied in order to determine the assessment of the intensity of the colors. Nineteen trials will be conducted. The information that includes the volume of the solution and the number of moles being applied of the Fe (NO₃₎)₃ and the 5- sulfosalicyclic acid will be of 5- sulfosalicyclic acid documented. This data will be used in order to ascertain the molar faction of each of the reagents.

In order to calculate the molar fraction of Fe (NO₃)₃, the amount of iron (III) nitrate must be viewed. It can be seen that the amount of Fe ⁽NO₃)₃  is 1.69 X 10^-3 M/ liter. The amount of solution is 6.61 ml. We would multiple 1.69 X 10^-3 M/ l. x 0.00651 l. = 1.10019 X 10 ^‘5 Moles of Fe ⁽NO₃)₃ The amount of 5- sulfosalicyclic acid is 1.71 X 10 ^‘3 Moles/l. The volume of solution is 3.5 ml. The 3.5 ml must be converted into liters . This infers, 1.71 X 10^’3 Moles/ l x the volume in liters (0.00350 l) = 5.985 X 10 ^‘6 moles of sulfocsalicyclic acid.

In order to aciculate the absorbance of solutions with the following value for (%T), the mathematical relations hip for the formula of absorbance must be applied.  The formula is:

A= 2- log₁₀ (%T)

The data was derived from tube #10. The molecular weight for a Mole of Fe (NO₃)₃, is 179.857 g/ mole. The percentage composition of iroin (III) in a mole of Fe (NO₃)₃, is   (55.845 g/ 179.845 g) = 0.31049 % in Fe (NO₃)₃.  In order to find the number of moles of Fe³⁺ in Fe (NO₃)₃, the percentage composition of the Fe (0.3149%) must be multiplied by the amount of Fe (NO₃)₃ found in tube 10. The amount of Fe (NO₃)₃, was assessed at 8.5 x 10^-6 Moles/l. The volume of solution is 5 ml. (0.005 l). The number of moles of Fe (NO₃)₃ as assessed at 4.25009133 M. The amount of Fe³⁺

The absorbance is 2- log₁₀ (0.35) = 2- log ₁₀-0.44855 = 0.44855 = A

The graph shows the ideal amount of Fe (NO₃)₃ and 5- sulfosalicyclic acid required in order to react. The table and graph is shown with values in moles.

The reagent in the reaction between Fe (NO₃)₃ and 5- sulfosalicyclic acid is Fe³⁺. This is due to the attribute of the Iron (III) nitrate being consumed until there is no longer a reaction.  The chemical ratio of the  proportion of nitric acid to the iron (III) s 6: 2.

2Fe³⁺ + 6 HNO₃ ? 2Fe (NO₃)₃ + 3H₂

Transmittance in chemistry is the quality of the sample that enables the passage of light. This is demon stated in chemistry as percentage transmittance (Kenkel 193). The absorbance is the amount the light absorption quality of the sample is defined by the following mathematical relationship A = log₁₀ (%T). . The absorbance is the assessment of the light absorption quality of a sample (Kenkel 194). These qualities are defined under the Beer – Lambert law (Kenkel 194).

The ratio of Fe (NO₃)₃ and 5- sulfosalicyclic acid must be 1: 1 in or4drer to achieve a reaction.

The evidence of the inert salicylic acid in the sample of manufactured aspirin can be found by conducting an iron (III) chloride examination. Add approximately 1 ml of deionized water into several testing tubes. Apply a sterile stirring rod and position a 5- sulfosalicylic acid crystal into the initial tests tube. In the following tube,  position ,a crystal of the manufactured aspirin.   In the final tube, position a crystal granule of the commercial variety of aspirin. Add one drop of iron (III) chloride to the test tubes with the manufactured aspirin. Agitate the tube and review the hues that are produced. The hues can also be analyzed by ,means of a spectrometer. Document your observation. Assess the melting point of the manufactured aspirin with theMeltemp device and contrast it with the melting point of commercial aspirin at 138°- 140°, ( LA Technical College, 1).

Works Cited

Kenkel, John. Analytical chemistry for technicians, (third edition). Boca Raton, FL: CRC Press, 2002. Print.

LA Technical College. “Chemistry 104: Synthesis of aspirin.”LA Technical College, 2014. Web. 20 October 2014.   http://www.chem.latech.edu/ºdeddy/chem104/104Aspirin.htm