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- Discuss thoroughly two (2) spectroscopic techniques used in analytical chemistry.
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- Which area of Analytical Chemistry do you think is the most applicable in your future profession which is Registered Medical Technologist?The use of statistics in analytical chemistry has become important and essentials in recent years. With specific examples, discuss four practical applications and/or utility of statistics in analytical chemistry.(a) Derive linear density expressions for BCC [110] and [111] directions in terms of the atomic radius R and (b) compute linear density values for these same two directions for tungsten. (a) [110]: i [111]: i (b) [110]: i [111]: i atom/R atom/R 1/m 1/m
- Assume for the following situations that Beer’s law remains linear. For (a) and (b), indicate whether the extinction coefficient ε, path length b, or concentration C is changing, and how it will change the absorbance of the solution. (a) A sample is moved from a test tube that is 1.0cm wide to a test tube that is 1.5cm wide. (b) A sample is diluted by adding enough solvent to double its volume. (c) A solution of iron (III) chloride appears brown when in high enough concentrations. In a 1.0 cm cuvet, the absorbance of 334 nm light by a 5.4 × 10−4 M solution of FeCl3 is measured to be 1.05. What is the extinction coefficient of the FeCl3 complex at this wavelength? (d) A sample containing an unknown concentration of FeCl3 is measured to have an ab- sorbance of 0.43 at 334 nm in a 1.0 cm cuvet. What is the molar concentration of the solution?Please thoroughly justify this answer in lower Chemistry terms.IAH and IGH are not the answer.
- 2. ] You make 150.0 mL of a copper(II) sulfate solution but forget to cover it before leaving for the day. The next class, you measure the volume and find that you only have 132.0 mL remaining. You didn’t record the initial concentration, but you measure the absorbance of the remaining solution at 620 nm and find that it is 0.386. You also construct the following calibration curve for CuSO4: Standard solution Abs620 0.50 M 0.424 0.40 M 0.336 0.30 M 0.247 0.20 M 0.159 (refer to image) a. What is the value for k (in Beer’s Law)? Provide a calculation or graph to support your answer. b. What is the concentration of the (remaining) solution? c. What was the concentration of the original solution from the first class? d. If you removed 7.5 mL from the 132.0 mL solution in the process of measuring the absorbance, how much water should you add to obtain the original concentration that you solved for in part (c)?Laser light scattering technique is an innovation for the determination of particle size. Briefly define this method, then state two each for its (2) advantages and disadvantages.Assume for the following situations that Beer’s law remains linear. For (a) and (b), indicate whether the extinction coefficient ε, path length b, or concentration C is changing, and how it will change the absorbance of the solution. (a) A sample is moved from a test tube that is 1.0 cm wide to a test tube that is 1.5 cm wide. 4 (b) A sample is diluted by adding enough solvent to double its volume. (c) A solution of iron (III) chloride appears brown when in high enough concentrations. In a 1.0 cm cuvet, the absorbance of 334 nm light by a 5.4 × 10−4 M solution of FeCl3 is measured to be 1.05. What is the extinction coefficient of the FeCl3 complex at this wavelength?
- 9. (a) What are the objectives of computational chemistry? Explain the differences intro between molecular mechanics and ab- initio methods.Be sure to answer all parts. Covalent bonds in a molecule absorb radiation in the IR region and vibrate at characteristic frequencies. (a) A molecular vibration absorbs radiation of wavelength 28.3 um. What frequency (in s) corresponds to that wavelength? Enter your answer in scientific notation. x 10 (b) A molecular vibration has a frequency of vibration of 7.574 x 10" Hz. What wavelength (in um) corresponds to that frequency? umPlasma emission spectroscopy can be used to determine the concentration of elements such as iron or zinc in pharmaceutical preparations. with the aid of suitable diagrams, outline the principles behind this technique and explain how it can be used to provide qualitative and quantitative information about these elements.
