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ap chem study guides

🌀  Unit 3 - Intermolecular Forces and Properties

👟  Unit 5 - Kinetics

🔥  Unit 6 - Thermodynamics

⚖️  Unit 7 - Equilibrium

  Unit 9 - Applications of Thermodynamics

🤺  AP Chemistry Essentials

3.13 The Beer-Lambert Law & Absorption

#beer'slaw

#absorption

⏱️  4 min read

written by

kanya shah

Dylan Black

dylan black

(editor)

Dalia Savy

dalia savy

(editor)


A Dive Into Spectrophotometry

In chemistry, many times we want to calculate how light reacts to a certain colored solution with solute in it. Well, spectrophotometry can do just that!

How Does a Spectrophotometer Work?

To get a better understanding of what spectrophotometry, let's take a look at a spectrophotometer itself:

https://firebasestorage.googleapis.com/v0/b/fiveable-92889.appspot.com/o/images%2FSketch-of-Conventional-Spectrophotometer-System-1.png?alt=media&token=d367fc01-0953-45be-bee3-f934f66e637f

Image Courtesy of ResearchGate

There are 3 main parts to this machine: the monochromator, the sample, and the detector.

The Monochromator

The monochromator has three main parts: the entrance slit, the dispersion device, and the exit slit. The entrance and exit slips are simple, they're where a beam of light enters and exits the monochromator. However, the dispersion device is the important part to the monochromator. Essentially, the dispersion device takes a beam of white light and splits it into the full spectrum of colors🌈. The exit slit is placed based on what wavelength of light the experimenter needs for the solution at hand, typically the opposite color (red solution --> green light, etc.)

The Sample

The sample is just that - the sample! It can be any colored solution you wish, from a solution of Copper (II) Sulfate, to red Gatorade, which we'll take a look at in a minute. Light from the monochromator is run through the sample and light is absorbed in the sample (That's why we want to use the opposite color, that's the most absorbed light!).

https://firebasestorage.googleapis.com/v0/b/fiveable-92889.appspot.com/o/images%2F-DEuXjnhdp8uq.png?alt=media&token=169c63bf-941c-4869-871f-3c9dfedf1dc1

Image Courtesy of Research Gate

On the right is the Incident Light (I0) and on the left is the transmitted light (I).

The Detector

Finally, after all of this has occurred, the remaining light is detected and the amount absorbed is spit out on a screen.

Applying the Spectrophotometer: Red Gatorade

Let's say a chemist is interested in calculating the molar concentration of red food dye🔴 in Gatorade. Well, this is a perfect time to talk about spectrophotometry in action! A chemist would fill a small test tube🧪 (though spectrophotometer test tubes are rectangular) with red gatorade and run it through a spectrophotometer with green light at around 560–520 nm. Then, he would get results as to the absorption, but how would he find the concentration? Well, luckily scientists have a formula for that:

The Beer-Lambert Law

The Formula Itself:

The formula for the Beer-Lambert Law is actually quite simple. The Beer-Lambert law (also known as Beer's law) is a linear relationship between the absorption of light and the concentration of the absorbing species.  

A = abc where: A = absorbance, a = molar absorptivity in L/[(mol)(cm)], b = path length in cm, and c is the concentration of the solution.

Once all written out, it may seem a little confusing, but the two variables a and b have are both quite simple to understand and are most often constant.

a = The molar absorptivity of a solute is a measurement of how strongly a chemical species reduces light (reduce here meaning absorbs, NOT takes electrons like in most other contexts) at a given wavelength.

b = The path length is simply the length of that rectangular test tube used by a chemist in a spectrophotometer. In fact, we often measure absorption on a linear scale by assuming a and b to be constant, leading to the equation A = mc, where m = ab:

https://lh6.googleusercontent.com/gLN7lC4Yhbp_XisnfXu4YIjg4yD2RTyXPZ_MgrYIw-PU2TAuot5spD6xVOBoLxickOPZUyY_I4r8noYsA96tFFrtaOlBmYH3g75af4PYcAPKEvPDJK_qzfm1xXSOjvo0acx1aYjC8hw

Gatorade Example

Back to our chemist friend. Let's say he looked up the molar absorptivity of his food dye, Red-40 and found it to be 2.13 * 10^4 L/(mol)(cm). He runs his solution through the spectrophotometer and finds an absorption of 0.500. Assuming a path length of 1cm, we can use Beer's law to calculate the molarity!

A = abc

0.5 = (2.13 * 10^4)(1)(c)

c = 0.5/2.13 * 10^4 = 2.3 * 10^-5 mol/L

And boom. We've found the concentration of red-40 in gatorade with an absorption of 0.5.

🎥 Watch: AP Chemistry - The Beer-Lambert Law

To enact the lab you would do for this key topic, you can use PhET simulations:

👉Engage: AP Chemistry - Beer's Law Lab

Practice AP Question for this Unit

In one of our previous guides, we went over part a of #5 on the 2019 AP Chemistry Exam. Let's go over part b since we now know the formulas🤓.

https://firebasestorage.googleapis.com/v0/b/fiveable-92889.appspot.com/o/images%2F-mwmJKN0ZjeBQ.JPG?alt=media&token=d437d1b0-88d0-415c-b2ed-546b277bbeda

To look over the in depth explanation of part a, read 1.6!

Part b is asking us for the wavelength of something. First things first, there are two equations that involve wavelength of light:

  • E=hv, where h = 6.626 x 10^-34

  • c=λv, where c = 2.998 x 10^8

That something is the energy needed to remove an electron from the valence shell, or the ionization energy/binding energy⚡. So let's solve for the wavelength of this energy!

The only piece of information they give us is the actual energy itself, but there are 6 different types of energy listed😕.

To recall, where the binding energy is the highest is where the nucleus is located. Thinking about valence electrons, we should be using the lowest binding energy. Now we know that E = 0.980 x 10^-18 and we can solve for frequency!

E = hv --> 0.980 x 10^-18 = (6.626 x 10^-34) (v)

v = 1.48 x 10^15

Now that we have frequency, we can solve for wavelength using c=λv.

2.998 x 10^8 = (λ) (1.48 x 10^15)

λ = 2.03 x 10^-7 m

This is an example of using both equations to solve an FRQ!🧠

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