Directions:For Questions 63–65, use the
following information:

25.0 mL of a sample of vinegar (a solution

of HC 2 H 3 O 2 , MW = 60.00 g ⋅mole–1) is

neutralized by 50.0 mL of a 0.50 N NaOH
solution.

63.What is the normality of the acid?

A. 0.25 N

B. 0.50 N

C. 0.75 N

D. 1.0 N

E. 2.0 N

64.Calculate the number of grams of acetic

acid per liter of the vinegar.

A. 5.0 grams

B. 25.0 grams

C. 30.0 grams

D. 50.0 grams

E. 60.0 grams

65.Calculate the weight percentage of

acetic acid in the vinegar. The vinegar

has a density of 1.0 g/mL.

A. 1.0%

B. 1.5%

C. 2.5%

D. 6.0%

E. 6.5%

66. When a solid melts, which of the
    following is true?

A. ∆H> 0, ∆S> 0

B. ∆H< 0, ∆S < 0

C. ∆H> 0, ∆S< 0

D. ∆H< 0, ∆S> 0

E. More information is required

before we can specify the signs of

∆Hand ∆S.

67. For the following reaction

Zn(s) + 2 Ag+(aq) →Zn2+(aq) + 2 Ag(s)

the standard voltage Ecell% has been

calculated to be 1.56 volts. To decrease

the voltage from the cell to 1.00 volt,

one could

A. increase the size of the zinc

electrode

B. reduce the coefficients of the

reactions so that it reads

1/2 Zn(s) + Ag+(aq) →

1/2 Zn2+(aq) + Ag(s)

C. decrease the concentration of the

silver ion in solution

D. increase the concentration of the

silver ion in solution

E. decrease the concentration of the

zinc ion in solution

Practice Test

Section

I

Multiple-Choice Questions

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