LESSON 2
PRACTICE EXERCISE
The following items will test your knowledge of the material covered in this lesson. There is only one correct
answer for each item. When you complete the exercise, check your answers with the answer key that follows. If
you answer any items incorrectly, go back to the part of the lesson that contains the information involved and
study again.
1. When verifying the preparation of chemical solutions, what can indicators be used for?
A. Standardizing an acid or base.
B. Air-drying glassware.
C. Determining the amount of solid solute needed.
D. In volumetric analysis to mark the end of titration.
2. When determining the amount of solid solute needed in the preparation of a chemical solution, what does N
represent in the equation?
A. Desired normality of solution to be prepared.
B. Volume solution to be prepared.
C. Weight of solute needed.
D. Milli-equivalent weight of solute.
3. When determining the volume of liquid needed in the preparation of a chemical solution, what does DFP
represent in the equation?
A. Decimal fractional purity of primary standard.
B. Decimal fractional purity of solute.
C. Volume of solute needed.
D. Volume of solution to be prepared.
4. When reviewing standardization procedures, what should be done before titration?
A. Swirl the flask.
B. Zero burettes.
C. Record the volume of solution used to reach the end point.
D. Calculate normality to four decimal places.
5. How many times should the titration procedure be repeated?
A. No more than two additional times.
B. At least once.
C. At least two additional times.
D. No more than once.
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QM 5181
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