Transcript Acids and Bases

Acids and Bases
ICS Madrid
1
Revision
When
an acid reacts with a base,
which compound(s) are formed?
What is the name of H2SO4?
What is the formula for
phosphoric acid?
Give four properties of acids.
Give four properties of bases.
2
Acids and bases: revision
What
is the charge on the
hydroxonium ion?
If the hydrogen ion concentration
is 10-10 M, is the solution acidic,
alkaline, or neutral?
If the [H+] in a solution is 1 x 10-1
mol/dm3, what is the [OH-]?
3
pH and concentration of strong acids and bases
If
the hydrogen ion concentration
is 10-7 M, what is the pH of the
solution?
If the hydroxide ion concentration
is 10-10 M, what is the pH of the
solution?
If the pH is 9, what is the
concentration of the hydroxide
ion?
4
If
the pH is 6, what is the
concentration of the hydrogen
ion?
How many free hydrogen ions
are there in one litre of water?
A litre of impure water has 10-4
mol of hydroxide ions. What is
the concentration of hydrogen
ions in this sample of water?
5
What
is the concentration of
hydrogen ions in a neutral
solution?
What is value of the ion-product
constant for water?
For a solution to be classified as
acidic, the hydrogen-ion
concentration must be _____ than
the hydroxide-ion concentration.
6
questions
A solution
in which the hydroxide
ion concentration is 1 x 10-4 M is
______.
A solution in which the hydroxide
ion concentration is 1 x 10-8 M is
______.
The formula of the hydrogen ion
is often written as ______.
7
The
products of self-ionization of
water are _____.
is most basic: a) [OH1-] = 1
x 10-4 M, or b) [H1+] = 1 x 10-11 M?
 In a neutral solution, the [H1+] is
______.
What is pH?
Which
8
Which
type of solution is one with
a pH of 8?
An indicator is what type of
compound?
In the reaction of aluminum
bromide with ionised sodium
bromide, which compound is the
Lewis acid?
9
In
the reaction of water with
hydrogen ions, which compound
is the Lewis base?
What is an acid according to
Arrhenius?
What type of acid (mono-, di-, or
triprotic) is sulphuric acid?
Which hydrogens can ionise in a
compound?
10
Which
hydroxides can ionise in a
compound?
Which hydroxide compound
yields the lowest concentration of
hydroxide ions in aqueous
solution: a) magnesium
hydroxide, or b) potassium
hydroxide?
11
Which
acid is monoprotic:
a) H2SO4, or b) CH3COOH?
Which acid is dibasic
a) H2SO4, or b) CH3COOH?
12
Which
is an Arrhenius base:
a) LiOH, or b) CH3COOH?
What is an acid, according to
Bronsted?
Which of the following is a
Bronsted-Lowry base, but not an
Arrhenius base: a) sodium
hydroxide, or b) ammonia?
13
Which
compound can act as both
a Bronsted-Lowry acid and a
Bronsted-Lowry base: a) water,
or b) sodium chloride?
What type of acid or base is the
ammonium ion?
What is a conjugate acid made
from?
14
What
is transferred between a
conjugate acid-base pair?
What is the term used to
describe a substance that can be
both an acid and a base?
the reaction: NH4+ + H2O 
NH3 + H3O+, water is acting as
a(n) ______.
In
15
the reaction: CO3- + H2O 
HCO3- + OH-, the carbonate ion
is acting as a(n) _____.
In
What
does amphoteric mean?
Identify
the Bronsted-Lowry
bases in this reaction: H2S + H2O
 H3O+ + HS-.
16
Which
of the following represents
a Bronsted-Lowry conjugate
acid-base pair: a) NH41+ and
NH3 or b) SO32- and SO2?
According to the Bronsted-Lowry
theory, water acts as a base
when it ______.
17
What
are the acids in the
following equilibrium reaction:
CN- + H2O  HCN + OHWhat is an “acid”, according to
Lewis?
Which acid is only a Lewis acid,
and not any other kind: a) water,
or b) boron trifluoride?
18
A hydrogen
ion is what type of
acid?
A Lewis acid is a substance that
can _____.
What is the acid dissociation
constant of a weak acid, if a
concentration of 0.3 M gives a
hydrogen ion concentration of
0.001 M?
19
What
is the hydrogen ion
concentration, if the acid
dissociation constant is 1 x 10-6 M
and the acid concentration is 0.01
M?
What characterizes a “strong”
acid or base?
20
The
acid dissociation constant
for an acid dissolved in water is
equal to the ______.
What is another name for the
acid dissociation constant?
What is the value of the acid
dissociation constant for a weak
acid?
21
How
many ionization constants
are associated with sulphuric
acid?
Which ionization constant is the
largest for phosphoric acid?
22
Which
of the following acids can
be concentrated, but is always
weak:
a) ethanoic acid
b) nitric acid?
for HF = 6.7 x 10-4. If we have
a 0.1 M solution, then [HF] is
_______ than [H+] x [F-].
Ka
23
A 0.12
M solution of an acid that
ionises only slightly in solution
would be termed ___ and ___.
Which of the following pairs
consists of a weak acid and a
strong base: a) sulphuric acid
and sodium hydroxide, or b)
acetic acid and sodium
hydroxide?
24
What
does “strong” mean when
referring to acids and bases?
Ethanoic acid ionizes in water as:
1%
CH3COOH + H2O  CH3COO- + H3O+
@ 99%
The ethanoate ion (CH3COO-) is
therefore a good _______
25
A 12.0
M solution of an acid that
ionises completely in solution
would be termed ___ and ____.
26