You can analyze for a copper compound in water using an instrument called a spectrophotometer. [A spectrophotometer is a scientific instrument that measures the amount of light (of a given wavelength) that is absorbed by the solution] The amount of light absorbed at a given wavelength of light (A) depends directly on the mass of compound per liter of solution. To calibrate the spectrophotometer, you collect the following data: Plot the absorbance (A) against the mass of copper compound per liter (g/L), and find the slope ( m ) and intercept ( b ) (assuming that A is y and the amount in solution is x in the equation for a straight line, y = mx + b ). What is the mass of copper compound in the solution in g/L and mg/mL when the absorbance is 0.635?
You can analyze for a copper compound in water using an instrument called a spectrophotometer. [A spectrophotometer is a scientific instrument that measures the amount of light (of a given wavelength) that is absorbed by the solution] The amount of light absorbed at a given wavelength of light (A) depends directly on the mass of compound per liter of solution. To calibrate the spectrophotometer, you collect the following data: Plot the absorbance (A) against the mass of copper compound per liter (g/L), and find the slope ( m ) and intercept ( b ) (assuming that A is y and the amount in solution is x in the equation for a straight line, y = mx + b ). What is the mass of copper compound in the solution in g/L and mg/mL when the absorbance is 0.635?
Solution Summary: The author explains that the absorbance should be plotted against the mass of the copper and the slope, intercept, and mass in solution were determined.
You can analyze for a copper compound in water using an instrument called a spectrophotometer. [A spectrophotometer is a scientific instrument that measures the amount of light (of a given wavelength) that is absorbed by the solution] The amount of light absorbed at a given wavelength of light (A) depends directly on the mass of compound per liter of solution. To calibrate the spectrophotometer, you collect the following data:
Plot the absorbance (A) against the mass of copper compound per liter (g/L), and find the slope (m) and intercept (b) (assuming that A is y and the amount in solution is x in the equation for a straight line, y = mx + b). What is the mass of copper compound in the solution in g/L and mg/mL when the absorbance is 0.635?
In order to find the density of a solution of unknown density, 10 mL of solution was drawn into a clean and dry beaker three times with a pipette and weighed and the weighing results were found to be 65.1452 g, 64.9982 g, 65.1027 g. Calculate the density of the solution and the standard deviation of the measurements, since the empty weight of the beaker is 52.2461 g.
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The Creation of Chemistry - The Fundamental Laws: Crash Course Chemistry #3; Author: Crash Course;https://www.youtube.com/watch?v=QiiyvzZBKT8;License: Standard YouTube License, CC-BY