Acids and Bases: Overview Common Uses of Acids and Bases ...
Acids and Bases Chapter 20 Lesson 2. Definitions Acids – produce H + Bases - produce OH - Acids...
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Transcript of Acids and Bases Chapter 20 Lesson 2. Definitions Acids – produce H + Bases - produce OH - Acids...
Definitions
• Acids – produce H+
• Bases - produce OH-
• Acids – donate H+
• Bases – accept H+
• Acids – accept e- pair• Bases – donate e- pair
Arrehenius
Bronsted-Lowry
Lewis
only in water
any solvent
used in organic chemistry,wider range of substances
HA
Let’s examine the behavior of an acid, HA, in aqueous solution.
What happens to the HA molecules in solution?
Ka (Dissociation Constant)
• A weak acid only ionizes to a small extent and
comes to a state of chemical equilibrium. • We can determine how much it ionizes by
calculating the equilibrium constant for this reaction, the ionization constant, Ka.
• The larger the Ka the more acid ions are found in solution and the stronger the acid because the more easily it donates a proton.
• The reverse is true for the smaller the Ka
HCOOH (aq) + H2O (l) < -- > H3O+ (aq) + HCOO- (aq)
• Ka = [H3O+][HCOO-][HCOOH]
• Notice how the Ka ignores the water since we are dealing with dilute solutions of acids, water is considered a constant, and when multiplied by both sides it is cancelled out.
Equilibrium In Solutions Of Weak Acids And Weak Bases
weak acid: HA + H2O H3O+ + A-
[H3O+][A-]
Ka =
[HA]
weak base: B + H2O HB+ + OH-
[HB+][OH-]Kb =
[B]You need to be able to write acid and base ionization equations!!!
Practice:
1. A solution of a weak acid, “HA”, is made up to be 0.15 M. Its pH was found to be 2.96. Calculate the value of Ka.
• Steps to follow:1. Write balanced equation2. Calculate [H+] using 10-pH
3. Set up chart for equilibrium (ICE or i Δ f)4. Solve using Ka expression
Answer
1. HA (aq) + H2O (l) < -- >H+ (aq) + A-(aq)
2. [H+]= 10 -2.96 = 0.0011 M3. Set up table:
HA H2O < -- > H+ A-
0.15 0 0
-.0011 +0.0011 +0.0011
0.139 0.0011 0.0011
i
Δ
f
Percent Dissociation
The fraction of acid molecules that dissociate compared with the initial concentration of the acid.
Percent Dissociation = [H+] x 100% [HA i]
For the previous question:Percent Dissociation = [0.0011] x 100% =0.73
% [0.15]
Practice:
• The ionization constant, Ka, for a hypothetical weak acid, HA, at 25°C is
2.2 x 10-4.a) Calculate the [H+] of a 0.20 M solution
of HA.b) Calculate the percent ionization of HA.c) Calculate the [A-].d) What initial concentration of HA is
needed to produce a [H+] of 5.0 x 10-3 M?
Answer
a) HA(aq) + H2O(l) < -- >H+(aq) + A-(aq)
Ka = [H+][A-] = 2.2 x 10-4
[HA]2.2 x 10-4 = (x)(x)
0.20 Mx2 = (2.2 x 10-4) (0.20 M)x = 0.0066 M
The [H+] is 0.0066 M.
Because it is a 1:1 ratio they are both the same concentration (x)
b) % ionization = 0.0066 M x 100% = 3.3%
0.20 Mc) From the stoichiometry of the
reaction,[H+] = [A-]Therefore, [A-] = 0.0066 M
Found d) from table set up
d) 2.2 x 10-4 = (5.0 x 10-3 M)(5.0 x 10-3 M)x – 5.0 x 10-3 M
• 2.2 x 10-4(x – 5.0 x 10-3M) = 2.5 x 10-5
• 2.2 x 10-4x – 1.1 x 10-6 = 2.5 x 10-5
• x = (2.5 x 10-5 + 1.1 x 10-6) / 2.2 x 10-4
• x= 0.12 M• The initial concentration of HA required
is 0.12 M.
Acid And Base Ionization Constants
weak acid: CH3COOH + H2O H3O+ + CH3COO-
[H3O+][CH3COO-]
Acid ionization constant: Ka =
[CH3COOH]
weak base: NH3 + H2O NH4+ + OH-
[NH4+][OH-]
Base ionization constant: Kb =
[NH3]
Acid and base ionization constants are the measure of the strengths of acids and bases.
Kb
• When using weak bases, the same rules apply as with weak acids, except you are solving for pOH and using [OH-]
Buffer Solutions
• A buffer solution is a solution that changes pH only slightly when small amounts of a strong acid or a strong base are added.
• A buffer contains a weak acid with its salt (conjugate base) or a weak base with its salt (conjugate acid) CH3COOH/CH3COONa
NH3/NH4Cl