The following results were obtained when each of a series of standard silver solutions was analyzed by flame-atomic absorption spectrometry: Concentration (ng-mL¹) Absorbance (r.u.) 0 5 10 15 20 25 30 40 0.003 0.127 0.251 0.390 0.498 0.625 0.763 0.771 Determine the slope and intercept of the calibration plot, along with their confidence limits (95%). Using the data from exercise 1 above, estimate the confidence limits for the silver concentration in: a) A sample giving an absorbance of 0.456 in a single determination. b) A sample giving absorbance values of 0.308, 0.317, 0.347, and 0.412 in four separate determinations.

Mass spectrometry is an extremely versatile detection system for GC. However, interfacing an HPLC system to a mass spectrometer is a much more difficult task. Describe the major reasons why it is more difficult to combine HPLC with mass spectrometry than it is to combine GC with mass spectrometry.

A solution is prepared by diluting 2.79 mL of the blue dye stock solution to 25.00 mL. The measured absorbance for the prepared solution is:   Blue dye stock solution = 0.293 M Absorbance at 630 nm = 0.00265 Calibration curve  y = 0.0833x   A.) What is the theoretical molar concentration? B.) What is the experimental molar concentration? C.) What is the percent error?

0.1040 g of a solid sample containing copper was dissolved by acid and transferred to a 250.00 mL volumetric flask and volume was made up with distilled water. The solution was then diluted by a factor of 20. The final solution was analyzed by atomic absorption spectrophotometry and the concentration was found be 3.109 ppm, What is the weight percentage of copper in the original solid sample? Keep four significant figures in your final answer. Do not try to include the "%" in your answer. e.g. if your final answer is 10.01%, only write 10.01 in the box.