Unit 13 Question Preview (ID: 55832)
Acid/base.
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A Bronsted-Lowry acid is
a) an electron-pair acceptor
b) an electron-pair donor
c) a proton acceptor
d) a proton donor
In the reaction NH3 + H2O ⮀ NH4+ + OH−, H2O is a
a) Bronsted-Lowry acid
b) Lewis base
c) Bronsted-Lowry base
d) Arrhenius acid
A Lewis acid is
a) an electron-pair acceptor
b) an electron-pair donor
c) a proton acceptor
d) a proton donor
A conjugate base, according to the Bronsted-Lowry definition is anything that
a) remains after a base has given up a proton
b) is formed by the addition of a proton to a base
c) is formed by the addition of a proton to an acid
d) remains after an acid has given up a proton
In the reaction HF + H2O ⮀ H3O+ + F−, a conjugate acid is
a) F
b) HF
c) H3O+
d) H2O
According to the Arrhenius definition, a base is
a) a proton donor
b) a proton acceptor
c) an electron pair donor
d) a hydroxide donor
Name the following acid: H2SO4
a) hydrosulfuric acid
b) sulfuric acid
c) sulfurous acid
d) hydrosulfic acid
Which of the following is hydroxide ion?
a) H3O+
b) H2O
c) H+
d) OH−
pH + pOH = ?
a) 10
b) 8
c) 14
d) 7
If you have a substance that has a pH of 8... is it basic or acidic?
a) neither neutral
b) basic
c) acidic
d) cannot tell from that number
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