A $2.3$ x $10^-4$ $M$ solution has trasmittance of $0.508$ when placed in a cell of path length $1$ $cm$ at wavelength $525$ $nm$ . Calculate the absorbance if concentration is doubled?

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A $2.3$ x $10^-4$ $M$ solution has trasmittance of $0.508$ when placed in a cell of path length $1$ $cm$ at wavelength $525$ $nm$ . Calculate the absorbance if concentration is doubled?

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Answer 1 · 2016-10-12T15:49:21

The absorbance should be $1.160$ , or thereabouts.

Explanation:

The $"Beer Lambert Law"$ , holds that $A=epsilonbC$ , where $epsilon="molar absorptivity"$ ; $b="cell path length"; and c="concentration in mol L"^-1$ .

So if we double the concentration, (or double the path length), we should in principle, double the absorbance. In practice, it is never this easy to do and deviations are common. The $"Beer Lambert Law"$ only approximately holds at low concentrations, $~=0.1*mol*L^-1$ or lower.

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A $2.3$ x $10^-4$ $M$ solution has trasmittance of $0.508$ when placed in a cell of path length $1$ $cm$ at wavelength $525$ $nm$ . Calculate the absorbance if concentration is doubled?

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Explanation:

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A 2.32.3 x 10^-410^-4 MM solution has trasmittance of 0.5080.508 when placed in a cell of path length 11 cmcm at wavelength 525525 nmnm. Calculate the absorbance if concentration is doubled?

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A $2.3$ x $10^-4$ $M$ solution has trasmittance of $0.508$ when placed in a cell of path length $1$ $cm$ at wavelength $525$ $nm$ . Calculate the absorbance if concentration is doubled?