1. By the Arrhenius definition, a base
a. produces
an H+ ion in water.
b. reacts
with a metal to produce H2.
c. Feels
slippery on skin.
d. produces
an OH‑ ion in water.
2. An
H+ ion in water is more accurately described as a (an)
a. hydroxide
ion. c. hydronium ion.
b. oxy
acid. d. binary acid.
3. A
Bronsted-Lowry acid is defined as a substance that
a. accepts
a proton. c. accepts an electron
b. donates
a proton. d.
donates an electron.
4.
Which
of the following is an acid - base pair in the reaction?
a. F - and H2CO3 c. HF and F-
b. HF and HCO3 - d. HF and H2CO3
5. Which of these
is not a true statement?
a.
All Lewis bases are also Bronsted-Lowry bases.
b.
All Lewis acids contain hydrogen.
c.
All Bronsted-Lowry acids contain hydrogen.
d. According to the Bronsted-Lowry theory, water
is both an acid and a base.
6. Which statement is true?
a. BF3(g) + NH3(g) à BF3NH3(s) is
an example of a Brønsted-Lowry reaction.
b. H3O+(aq) + OH-(aq) à 2H2O(l) is
an example of a Brønsted-Lowry reaction.
c. The
Brønsted-Lowry Theory states that an acid and a base react through electron
transfer.
d. The hydroxide ion is
normally a Brønsted-Lowry acid.
7. Water can act as either an acid or a base.
Which equation represents water reacting as an acid?
a. H2O(l) +
NH3(g)
à OH–(aq) +
NH4+(aq)
b. H2O(l) + HCl(aq) à H3O+ + Cl–(aq)
c.
H2O(l) à H2(g) + ½O2(g)
d.
H2O(l) +
C(s) à
CO(g) + H2(g)
8. What does the
strength of an acid depend upon?
a. concentration
of the acid
b. time
it takes the acid to neutralize a base
c.
extent to which the acid ionizes
d.
volume of the acid
9. According to the
Arrhenius theory, what causes the characteristic properties of bases?
a. aqueous
hydrogen ions
b. lone
pairs of electrons in the base molecule
c.
aqueous hydroxide ions
d.
proton donors in the base molecule
10. Which substance can
be called an Arrhenius base?
a. CH3OH c. HBr
b. KOH d.
NaCl
11.
A solution in which [H+] = [OH-] is said to be
a.
acidic. c. neutral.
b.
basic. d. salt.
12. A solution in which [OH-] exceeds
[H+] is said to be
a.
acidic. c. neutral.
b.
basic. d. salt.
13. What is the conjugate acid of HSO4-?
a.
H2SO4 c. SO4-
b.
H3SO4 d. SO4-2
14. What is the conjugate base of H3PO4?
a.
H2PO4 c. PO4-3
b.
H2PO4- d. HPO4-2
15. Household ammonia has a [H+] of
1x10-12. How do you classify
household ammonia?
a.
acid c. salt
b.
base d. neutral
16. Which concentration below is neutral?
a.
[H+]
= 4 x 10-9 c. [OH-] = 7 x 10-13
b.
[OH-]
= 1 x 10-7 d. [H+] = 3 x 10-9
17. What is the Kw of water at 25oC?
a.
1.0
x 1014 c.
1.0 x 10-14
b.
1.0
x 10-7 d. 1.0 x 107
18. The interaction of proton with one water
molecule forms the
a.
hydroxide
ion, OH- c. hydronium ion, H3O+
b.
Hydrogen
ion, H+ d. water, H2O
19. The more readily a base accepts protons, the
less its conjugate acid
a.
gains
electrons. c. exchanges electrons.
b.
gives
up electrons. d. no transfer occurs.
20. An acid is a substance that can donate a
proton to another substance while a base is a substance that can accept a
proton. This is the definition of acid
and base according to
a.
Arrhenius c. Lowry
b.
Bronsted d. Bronsted and Lowry
21. What is the concentration of OH-(aq)
in a solution in which [H+] = 2 x 10-6 M?
a.
1.0
x 10-7 M c. 1.0 x 10-8 M
b.
5.0
x 10-9 M d. 1.8 x 10-9 M
22. What is the concentration of H+(aq)
in a solution in which [OH-] is 0.010 M?
a.
1.0
x 10-11 c. 1.0 x 10-13
b.
1.0
x 10-12 d. 1.0 x 10-14
23. It is the negative logarithm in base of 10 of
[H+].
a.
pH c. [H+]
b.
pOH d. [OH-]
24. Rain has a pH of 6.0, what is it value in pOH?
a.
6.0 c. 8.0
answer key ?
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