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Question 3After creating a Beer's Law plot using standard solutions of Q, you determined the slope of Beer's Law to be 0.515 M-1. Your unknown solution of Q tested in Part B of the experiment had an absorbance of 0.145. Determine the concentration (in molarity) of the unknown solution Q from Part B.Question 4Refer to the procedure stated in the manual pages for Part A to answer the following question.Using the equation editor embedded in this question, show a sample calculation determining the original concentration of the provided unknown Q in Part A from the diluted concentration calculated in question 3 above.Lab ManualYou have been provided with a solution of unknown Q, the actual molar concentration is listed as the unknown number. Dilute 15.00 mL of the provided solution to a final volume of 50.00 mL. You may only use the equipment and reagents listed above. Be sure to record your unknown number in your notebook. After making your dilution, calculate the concentration of your diluted solution.

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Answer:

3. Concentration of the unknown solution = 2.81 *10^-1 M

4. The concentration of diluted solution (Q)  = 0.9385 M

Explanation:

3. Calculating the concentration of the unknown solution Q using the formula, we have;

A = E*e*C

Where;

E = slope = 0.515 M^-1

e =1 cm

A = absorbance = 0.145

C = Concentration of the unknown solution

Substituting into the formula, we have;

A = E*e*C

C = A/E *e

   = 0.145/0.515*1

  = 2.81 *10^-1 M

Therefore, the concentration of unknown solution  = 2.81 *10^-1 M

4. Calculating the concentration of diluted solution, we have;

Let concentration of initial Q = Mi

So, Mi*Vi = Mdiluted * Vdiluted

Mi * 15.00mL = 2.81 *10^-1* 50.00mL

Mi = (2.81 *10^-1* 50.00)/ 15.00

   = 0.9385 M

Therefore, the concentration of diluted solution (Q)  = 0.9385 M

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