A solution of concentration $5$ x $10^-5$ $M$ has absorbance of $0.75$ in a cell of $1$ $cm$ length. Calculate molar absorptivity and transmittance of the cell?

Question

10245 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-02-14T17:49:12

$(a)$

$1.5xx10^(4)"L/mol/cm"$ .

$(b)$

$17.8%$

$(a)$

The Beer - Lambert Law gives us:

$A=epsilon_(@)cl$

$:.epsilon_(@)=(A)/(cl)$

$:.epsilon_(@)=(0.75)/(5xx10^(-5)xx1)$

$epsilon_(@)=1.5xx10^(4)"L/mol/cm"$

$(b)$

$log(I_0/I)=0.75$

Since $I_0=100rArr$

$2-logI=0.75$

$I=17.8%$ which is the transmittance.

A solution of concentration 55 x 10^-510^-5 MM has absorbance of 0.750.75 in a cell of 11 cmcm length. Calculate molar absorptivity and transmittance of the cell?