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Alenkinab [10]
3 years ago
7

3. A Beer's law plot for Cu2+ was experimentally obtained. The slope of the Beer's law plot was 435 L/mol (with a y-intercept =

0.001). A Cu2+ solution of unknown concentration had an absorbance of 0.75. What is the molar concentration of Cu2+ in the unknown solution?
Chemistry
1 answer:
ozzi3 years ago
7 0

Answer:

0.00172 M

Explanation:

According to the Lambert's Beer law:-

A=\epsilon l c

Where, A is the absorbance

l is the path length

\epsilon is the molar absorptivity

c is the concentration.

If a graph is plotted between the concentration and absorbance, then the slope is:- \epsilon l. So,

c=\frac{A}{slope}=\frac{0.75}{435}\ M=0.00172\ M

<u>0.00172 is the molar concentration of Cu^{2+} in the unknown solution.</u>

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Determine the mass of 5.20 moles of C6H12 (gram-formula mass = 84.2 grams/mole).
muminat

Hello!

Determine the mass of 5.20 moles of C6H12 (gram-formula mass = 84.2 grams/mole).

We have the following data:

m (mass) = ? 

n (number of moles) = 5.20 moles

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Now, let's find the mass, knowing that:

n = \dfrac{m}{MM}

5.20\:\:\diagup\!\!\!\!\!\!\!mol = \dfrac{m}{84.2\:g/\diagup\!\!\!\!\!\!\!mol}

m = 5.20*84.2

\boxed{\boxed{m = 437.84\:g}}\end{array}}\qquad\checkmark

_______________________

I Hope this helps, greetings ... Dexteright02! =)

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