An analysis was performed using a UV-Vis spectrophotometer. The measured absorbance of a solution of X with a path length of 1.00 cm is 0.600. The molar absorptivity of X is 379 Lmol?¹cm?¹. Calculate the concentration of the solution of X.
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Step 1: Calculate the concentration using Beer's Law formula: \[ \text{Concentration} = \frac{\text{Absorbance}}{\text{Molar Absorptivity} \times \text{Path Length}} \] Show more…
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A substance, X, has a molar absorptivity of 1250 L mol-1 cm-1 at 325 nm. A sample of X gives an absorbance of 0.8 when measured in a UV-visible spectrophotometer at 325 nm with a path length of 1 cm. What is the concentration of the sample of X? A. 1000 mol L-1 B. 6.4 × 10-4 mol L-1 C. 1563 mol L-1 D. 1 mol L-1 E. 1.56 mol L-1
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The absorbance of a solution is found to be 1.1. The path length is 1.0 cm and the extinction coefficient (also known as the molar absorptivity coefficient) is 9.0 M-1cm-1. What is the concentration of the solution?
Spectrometry. The absorbance $A$ of a solution is defined as $$A=\log _{10}\left(I_{0} / I\right)$$ in which $I_{0}$ is the incident-light intensity and $I$ is the transmitted-light intensity. The absorbance is related to the molar absorption coefficient (extinction coefficient) $\varepsilon$ (in $\mathrm{M}^{-1}$ $\mathrm{cm}^{-1}$ ), concentration $c(\text { in } \mathrm{M}),$ and path length $l(\text { in } \mathrm{cm}$ ) by $$A=\varepsilon l c$$ The absorption coefficient of myoglobin at $580 \mathrm{nm}$ is $15,000 \mathrm{M}^{-1} \mathrm{cm}^{-1} .$ What is the absorbance of a $1 \mathrm{mg} \mathrm{ml}^{-1}$ solution across a $1-\mathrm{cm}$ path? What percentage of the incident light is transmitted by this solution?
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