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Mid­Unit Test, Part 2
Answer the following questions. You may use the periodic table in the Chemistry: Problems and Solutions book for this test. When you have finished, submit this assignment to your teacher by the due date for full credit.
(5 points)

Score

1.

For an experiment, a biology student makes 1 liter of a solution containing the following substances, which are shown in the table below. Using the given information, fill in the missing parts of the table for each substance by
(a) providing the formula weight and (b) calculating either the mass the student needs to weigh out or the number of moles that the student has, based on the amount weighed out. For each calculation, show your work.
Be sure to include the formula mass of water for CaCl2 ( 2H2O and NaH2PO4 ( H2O.

Substance

Formula
Weight (g/mol)

Number of
Moles

Mass (g)

NaCl

58.4
74
180.2
84
147.01
246.47
120.4

0.14

58.5
74.55
1.01

KCl
C6H12O6
NaHCO3
CaCl2 ( 2H2O
MgSO4
NaH2PO4 ( H2O

0.005

.75
0.0262

.01173
0.0008
.0033

84.01
0.15
120.336
0.14

(5 points)

Score

2. Acetaminophen (C8H9NO2) is the active ingredient in many nonprescription pain relievers. Each tablet contains
500 mg of acetaminophen, and a typical adult dose is two tablets every eight hours.
● Determine the molar mass of acetaminophen (show your work).
● Calculate the number of moles of acetaminophen in a single tablet (show your work).

Calculate the number of moles of acetaminophen that an adult would have taken if she took three doses of acetaminophen in one day (show your work).

Answer: 8x12 plus 1x9 plus 1x14 plus 2x16 plus = 151 for molar mass of acetaminophen

molacetaminophen is 500 mg/ by the mass of acetaminophen which equals 3.311 molacetaminophen plus 500 mg x 3 doses/ by the molar mass acetaminophen equals 9.933

___ of 10

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