After performing the experiment, Spectrophotometric Analysis of Aspirin, a stude

Question

After performing the experiment, Spectrophotometric Analysis of Aspirin, a student wants to investigate the effect of heating on the degradation of acetylsalicylic acid in an aspirin tablet. With the approval of the instructor, the student heats an aspirin tablet containing 325 mg acetylsalicylic acid in a one-hundred degree oven for 4 hours to simulate the effects of an aspirin tablet sitting in a car for half a day on a hot day in July. The student then prepares the standards and the experimentally heated tablet in the same manner as performed in the lab. (Assume that a 2.0 mL sample of the aspirin unknown solution was diluted in a 50.00 mL volumetric flask just as you did in lab). The linear fit for the calibration of the standards produced y = 0.00341 x + 0.029. The absorbance of the experimentally heated
tablet was found to be 0.075.

What is the acetylsalicylic acid concentration in the diluted solution?

How many mg acetylsalicylic acid are in the diluted solution?

How many mg acetylsalicylic acid are in the tablet?

What % of the original 325 mg acetylsalicylic acid contained in the tablet is not degraded?

What % of the original 325 mg acetylsalicylic acid contained in the tablet is degraded?

Explanation / Answer

1) Always run [ ] = 0 to set zero point

2) the eqn is not correct: y2-y1 = slope (x2-x1);

slope from A & E-----> slope = 0.0037
_________B & D------> slope = 0.0053

linear line from eXcel: A = 0.0041 * [ ] + 0.0563 (not like yours!)

Actually for the expt, it is better for [ ] as y and A as x

[ ] = 216.51 * A - 4.1161

[F] = 47 mg/liter

X = mg in treated soln = 12 mg/liter
Y = mg dissolved that is "equivalent" to 325/?? liters

fraction left = X/Y

Plug and SOLVE

Basic mathematics is a prerequisite to chemistry

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