You weighed out 0.020 g of your crude aspirin product in order to determine the amount of salicylic acid impurity. Following the procedure outlined in the manual, you dissolved the solid and diluted the solution to a final volume of 10.0 mL. If the absorbance of your sample solution was 1.07, what was the percent salicylic acid in your product? a. 6.4%.
b. 10%.
c. 7.8%.
d. 92%.
e. none of the above.

7.8%

Explanation:

Given that:

The initial mass amount of aspirin = 0.020g

The standard molar mass of aspirin = 240 g/mol

Thus, the number of moles = mass/molar mass

= 0.020/240

= 0.0000833 moles

Now, the molarity of aspirin in the solution(diluted) =

= (provided the volume v = 0.01 L)

The absorbance of the sample solution A =1.07

The path length (b) = 1 cm

From the standard value of salicylic acid, the coefficient (e)= 139.322 /M/cm

Now; according to Beer's law, the concentration of aspirin is:

A = e×b×c

c = 0.00768 M

Finally, relating the concentration of the aspirin, the percentage of salicylic acid the product  

= 7.8%

the awnser is group 12

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.