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How does the molar absorptivity depend upon the concentration mole per L of the dissolved solute?
Molar absorptivity is completely independent of concentration of a substance as Molar absorptivity is represented by epsilon and is a constant. Absorbance of light is what is dependent upon concentration and will go down as concentration goes down and increase as concentration increases.
The absorbance of a solution of NiCl2 of unknown concentration is found to be 0.388 what is the concentration of this soultion?
The concentration of the NiCl2 solution can be determined by using Beer's Law, which states that absorbance is directly proportional to concentration. You would need to know the molar absorptivity of NiCl2 at that specific wavelength in order to calculate the concentration. Plugging in the values of absorbance and molar absorptivity into Beer's Law equation would give you the concentration of the NiCl2 solution.
How do you determine molar absorptivity of cobalt nitrate?
Utilizing the Beer-Lamber Law you have A=abc here A= is the absorbance at a set wavelength a= the molar absorbtivity b= the path length c= concentration in molar The best way to determine a is to make solutions of known concentrations of cobalt nitrate (3-5 would be best) and determine the absorbance of each solution. Next plot the Abs vs concentration of each solution using something like excel or R. Determine the line of best fit ( it's important to force fit this line through 0) the R-sqr value should be no less than .95 Since the equation of a line is : y=mx +b, this is equivalent to A=abc noting that b is assumed to be 1cm we habe A=ac, where m=a and x=c In short the slope of the line of best fit in the molar absorbtivity
What is the molar absorptivity of Cu2 plus at 620 nm given that the cuvettes used in lab had a pathlength of 1.00 cm with a concentration verse absorbtivity curve of y equals .727x plus .0557?
The molar absorptivity of Cu2+ at 620 nm can be calculated using Beer-Lambert law equation A = εlc, where A is the absorbance, ε is the molar absorptivity, l is the pathlength (1.00 cm), and c is the concentration. Using the concentration- absorbance curve given (y = 0.727x + 0.0557), at 620 nm, x = c = 1. Therefore, substituting these values into the Beer-Lambert equation will give you the molar absorptivity of Cu2+ at 620 nm.
How to calculate lambda max?
using uv-visible spectrophotometer concentration vs absorbance is plotted and the maximum absorbance of the drug is lambda max of the drug. then after it will decrease. still if needed clarification, refer beer lambert"s law
What is the molar absorptivity of red dye?
The molar absorptivity of a substance is a measure of how strongly it absorbs light at a particular wavelength. To determine the molar absorptivity of red dye, you would need to know the specific type of red dye as well as the wavelength of light at which its absorption is being measured. Molar absorptivity is typically provided in literature or can be experimentally determined.
What is the extinction coefficient (aka molar absorptivity) for CuSO4 at the wavelength you used?
The extinction coefficient, also known as molar absorptivity, for CuSO4 at the specific wavelength used is a measure of how strongly the compound absorbs light at that wavelength. It is a constant value that helps determine the concentration of the compound in a solution based on its absorbance.
What is the extinction coefficient (aka molar absorptivity) of CuSO4 at the wavelength you used?
The extinction coefficient, also known as molar absorptivity, of CuSO4 at the specific wavelength used is a measure of how strongly the compound absorbs light at that wavelength. It is a constant value that helps determine the concentration of the compound in a solution based on its absorbance.
How does the molar absorptivity depend upon the concentration mole per L of the dissolved solute?
Molar absorptivity is completely independent of concentration of a substance as Molar absorptivity is represented by epsilon and is a constant. Absorbance of light is what is dependent upon concentration and will go down as concentration goes down and increase as concentration increases.
What is the molar absorptivity of CuSO4 and how does it impact the measurement of its concentration in a solution?
The molar absorptivity of CuSO4 is a measure of how well it absorbs light at a specific wavelength. It impacts the measurement of its concentration in a solution by affecting the amount of light absorbed, which is used to determine the concentration through a calibration curve. A higher molar absorptivity means more light is absorbed, leading to a more accurate concentration measurement.
What is the molar absorptivity of copper and how does it impact the analysis of copper-containing compounds?
The molar absorptivity of copper is a measure of how well copper absorbs light at a specific wavelength. It impacts the analysis of copper-containing compounds by helping to determine the concentration of copper in a sample based on the amount of light absorbed. A higher molar absorptivity means that copper can be detected at lower concentrations, making the analysis more sensitive and accurate.
Why can you not measure the molar absorptivity of the food dyes?
You can.
What is the molar absorptivity of crystal violet?
The molar absorptivity of crystal violet can be determined using Beer's Law. Beer's Law is A=E*c*l where A is absorbance, E is the molar absorptivity, C is the concentration of the crystal violet, and l is the path length. Path length is how long the light has to travel through the solution. If you can find the absorbance of a certain concentration by using a spectrophotometer, where the path length is 1 cm, then you know all the variables and are able to solve for the molar absorptivity. For example, the measured absorbance of 2.5x10^-5 M CV (crystal violet) is 1.64 with a path length of 1 cm. This means 1.64=E*(2.5x10^-5)*1 E=1.64/(2.5x10^-5) E=65600 Happy Chemistry!
The absorbance of a solution of NiCl2 of unknown concentration is found to be 0.388 what is the concentration of this soultion?
The concentration of the NiCl2 solution can be determined by using Beer's Law, which states that absorbance is directly proportional to concentration. You would need to know the molar absorptivity of NiCl2 at that specific wavelength in order to calculate the concentration. Plugging in the values of absorbance and molar absorptivity into Beer's Law equation would give you the concentration of the NiCl2 solution.
How do you determine molar absorptivity of cobalt nitrate?
Utilizing the Beer-Lamber Law you have A=abc here A= is the absorbance at a set wavelength a= the molar absorbtivity b= the path length c= concentration in molar The best way to determine a is to make solutions of known concentrations of cobalt nitrate (3-5 would be best) and determine the absorbance of each solution. Next plot the Abs vs concentration of each solution using something like excel or R. Determine the line of best fit ( it's important to force fit this line through 0) the R-sqr value should be no less than .95 Since the equation of a line is : y=mx +b, this is equivalent to A=abc noting that b is assumed to be 1cm we habe A=ac, where m=a and x=c In short the slope of the line of best fit in the molar absorbtivity
What is the molar absorptivity of Cu2 plus at 620 nm given that the cuvettes used in lab had a pathlength of 1.00 cm with a concentration verse absorbtivity curve of y equals .727x plus .0557?
The molar absorptivity of Cu2+ at 620 nm can be calculated using Beer-Lambert law equation A = εlc, where A is the absorbance, ε is the molar absorptivity, l is the pathlength (1.00 cm), and c is the concentration. Using the concentration- absorbance curve given (y = 0.727x + 0.0557), at 620 nm, x = c = 1. Therefore, substituting these values into the Beer-Lambert equation will give you the molar absorptivity of Cu2+ at 620 nm.
What is the extinction coefficient of crystal violet?
The extinction coefficient of crystal violet is approximately 89,000 M^(-1)cm^(-1) at a wavelength of 590 nm. This value indicates the molar absorptivity of crystal violet at this specific wavelength, which is commonly used for measuring the concentration of crystal violet in solution using spectrophotometry.
