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## Chemistry library

### Unit 17: Lesson 4

Spectroscopy- Introduction to spectroscopy
- Electronic transitions and energy
- Worked example: Calculating the maximum wavelength capable of ionization
- Spectrophotometry and the Beer–Lambert Law
- Worked example: Calculating concentration using the Beer–Lambert law
- Spectroscopy and the electromagnetic spectrum
- Electronic transitions in spectroscopy
- Beer–Lambert law

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# Worked example: Calculating concentration using the Beer–Lambert law

AP.Chem:

SAP‑8 (EU)

, SAP‑8.C (LO)

, SAP‑8.C.1 (EK)

, SAP‑8.C.2 (EK)

The Beer–Lambert law relates the absorption of light by a solution to the properties of the solution according to the following equation:

*A*=*εbc*, where*ε*is the molar absorptivity of the absorbing species,*b*is the path length, and*c*is the concentration of the absorbing species. In this video, we'll use the Beer–Lambert law to calculate the concentration of KMnO₄ in an unknown solution. Created by Sal Khan.## Video transcript

- [Instructor] So I have a question here from the Kotz, Treichel,
and Townsend Chemistry and Chemical Reactivity book, and I got their permission to do this. And it says a solution
of potassium permanganate has an absorbance of 0.539 when measured at 540 nanometers in a one centimeter cell. What is the concentration of
the potassium permanganate? Prior to determining the
absorbance for the unknown solution the following calibration
data were collected for the spectrophotometer. So the way that we would tackle this is we know that there
is a linear relationship between absorbance and concentration. We could describe it something like this, that absorbance is going to be equal to sum slope times are concentration. And you could say sum y-intercept, if we're a purist about it, then the y intercept should be zero because at a zero concentration, you should have a zero absorbance. But the way that chemists
would typically do it, is that they would put
these points into a computer and then a computer do
a linear aggression. You could also do that by hand but that's a little bit out
of the scope of this video. And I did that, I went to Desmos and I typed in the numbers that they gave. And this is what I got, so I just typed in these numbers and then it fit a linear
regression line to it and it got these parameters,
m is equal to this and b is equal to this. Now we could say significant figures it seems like the small
significant figures here we have have our three, but we could just view the m and the b as intermediate numbers
in our calculations. What I'm going to do is
I'm gonna use m and b, and then my final I'll answer I'm going to round to
three significant figures. So what this tells us, is that absorbance is going to be 5.65333 times our concentration minus 0.0086. And now they've given us what A is. Let me get rid of all of this stuff here. They told us that our absorbance is 0.539, so we know that 0.539 is equal
to 5.65333C minus 0.0086. And then if you wanna solve for C, let's see, we could add
this to both sides first. So you get 0.539 plus
0.0086 is equal to 5.65333C, and then divide both sides by this, and you would get C is equal to, is going to be approximately
equal to, be a little careful all of these would really be approximate. C is gonna be equal to 0.539
plus 0.0086 divided by 5.65333. And of course we want to round
to three significant figures. All right, 0.539 plus
0.0086 is equal to that, divided by 5.65333 is equal to this, so if we go three significant figures this is going to be 0.0969. So I would write the concentration is approximately 0.0969 Molar.