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Chapter 19 Acids And Bases
Test Description: Acid and base interactions
Instructions: Answer all questions to get your test result.
1) For a water solution to be acidic, what must be true?
A
[H3O+] < [OH-]
B
[H3O+] > [OH-]
C
none of these.
D
[H3O+] = [OH-]
2) A buffer keeps a solution's pH constant by
A
releasing or absorbing H+ ions
B
increasing the concentration of H2O molecules.
C
providing neutralizing ions.
D
changing the [H3O+].
3) A common example of a good buffer solution is
A
seawater.
B
herb tea.
C
blood.
D
coffee.
4) What determines a buffer's capacity to neutralize added base?
A
all of these are correct.
B
the amount of conjugate base
C
its temperature
D
the amount of weak acid
5) The amount of acid or base that a buffer can neutralizze is called
A
neutralizing capacity
B
buffer concentration.
C
the buffer capacity.
D
neutralizing concentration.
6) If hydronium ions or hydroxide ions are added beyond the buffer capacity, the added excess ions will
A
change the pH.
B
neutralize each other.
C
have no effect on the pH.
D
precipitate.
7) The carbonic acid-bicarbonate buffer sstem in blood has a 1:20 ratio of acid to conjugate base. Thie means it has a great capacity for neutralizing
A
excess base.
B
the conjugate base.
C
the conjugate acid.
D
excess acid.
8) How can you determine the concentration of a water solution of a weak acid?
A
perform an acid-base titration.
B
determine the extent of electrical conductivity.
C
Observet he color change of litmus paper.
D
Measure the pH with a pH meter.
9) To determine the concentration of an unknown acid, one of the requirements is
A
litmus paper.
B
universal pH paper.
C
a standard acid.
D
a standard base
10) To determine the concentration of an unknown acid or base in a titration, you need a(n)
A
acid-base indicator.
B
a standard salt solution.
C
standard base.
D
weak acid solution.
*select an answer for all questions
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