Diprotic Titration: Multi-Step Chemical Reactions 012-10738 r1.04.
Acid-Base Equilibria. Arrhenius acids increase [H + ] when dissolved in water acids can be...
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Transcript of Acid-Base Equilibria. Arrhenius acids increase [H + ] when dissolved in water acids can be...
Acid-Base Equilibria
Arrhenius
• acids increase [H+] when dissolved in water• acids can be classified as monoprotic, diprotic
or triprotic• bases increase [OH-] when dissolved in water• bases can be classified as monobasic, dibasic,
or tribasic
A-B Strength
• strong acids & bases ionize completely and are strong electrolytes
• 7 acids & 8 bases (memorize them!!!)• diprotic acids & dibasic bases do NOT ionize
completely, only their first H+ or OH- ionizes completely.
• Strong acid + strong base = neutral salt• strong A-B are not equilibrium expressions, but
all other A-B are reversible
Bronsted-Lowry A-B
• restricts definition to H+
– acids donate H+
– bases accept H+
• allows the classification of less traditional A-B• conjugate A-B pairs = 2 formulas in an
equation whose formulas differ by a H+
What is the acid, base, and the conjugates?
HClO +H2O H3O+ + ClO-
CO32- + H2O OH- + HCO3
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Wait, water can go both ways?
• amphoteric substances can behave as either an acid or base depending on what they react with.
• water and anions with protons (H+) attached are most common amphoterics
Weak A-B• only partially ionize in water and are weak
electrolytes• can be written as equilibrium expressions with a
Ka or Kb value• K value indicates how much the acid or base will
ionize (high K = higher ionization)• larger K values indicate a stronger acid or base• For di- and tri- protic/basic, there will be 2 K
values (one for the first ionization and one for the second)
Autoionization of Water
H2O + H2O OH- + H3O+
• reversible equilibrium where water can donate a proton to itself
• Kw = 1.0 x 10-14 at room temp.
• For any conjugate A-B pair, Kw = Ka x Kb
• What is the Ka value for NH4+?
Example
Is an aqueous solution of Na2HPO4 acidic or basic?
pH scale
pH = -log[H+]• works for pH ranges from 2-12 and
approximates pH outside that window• The exponent on the [H+] is an indicator of
approximate pH.
Strong A-B
• no equilibrium b/c all acid/base ionizes• use original acid concentration to calculate pH• Calculate the [H+] and pH in a solution of
0.37M hydrochloric acid.• Calculate the [OH-] and pH in a 0.58M solution
of NaOH
Weak Acids
• use RICE to find equilibrium concentrations:R HA + H2O H3O+ + A-
I I 0 0C -x +x +xE I-x x x
• b/c Ka for most weak acids is less than 10-3, I-x is about equal to I, so Ka = x2/I
Example
What is the pH of a 0.20M solution of acetic acid (CH3COOH)?
Weak Bases
• similar calculations as acids (replace H3O+ with OH-)R B + H2O OH- + HB+
I I 0 0C -y +y +yE I-y y y
• b/c Kb for most weak bases is less than 10-3, I-y is about equal to I, so Kb = y2/I
Example
What is the pH of a 0.68M solution of aqueous ammonia?
Classify the following as weak/strong acids/bases:
• chloric acid• ammonium chloride• calcium hydroxide• ethyl amine• sodium cyanide
Example
Measurements show that the pH of a 0.10M solution of acetic acid is 2.87. What is the Kb of potassium acetate?
A-B properties of salt solutions• for the most part anions are slightly basic (because they
attract protons) and cations are slightly acidic (because they can donate protons)
• ions from strong A-B are the only neutral ions• To determine if a salt is acidic or basic, look at the ions it
forms:– ignore any neutral ions– if anion is left, salt is basic– if cation is left, salt is acidic– if both cation & anion are neutral, salt is neutral– if both cation & anion are not neutral, the A-B-ness can’t be
determined from the formula
Classify the following salts as acidic, basic, or neutral:
• NaNO2
• CH3NH3Cl
• NaCl• MgSO4
• Al2(SO3)3
A-B-ness & chemical structure
3 factors affect attraction of electrons (acidity increases with stronger attraction of electrons)1. ionic charge – when comparing similar atoms, more
positive ions are stronger acids2. oxidation # on central atom – when comparing
similar formulas with the same central atom, the higher the ox#, the stronger the acid
3. electronegativity – when comparing similar formulas with different central atoms, the higher the EN, the stronger the acid
Common Base Reactions• Strong bases also include hydrides (H-), nitrides
(N3-), and carbides (C22-)
– NaH + H2O H2 + Na+ + OH-
– Mg3N2 + 6H2O 2NH3 + 3Mg2+ + 6OH-
– Ca2C2 + 2H2O C2H2 + Ca2+ + 2OH-
• strong bases also include oxides of groups 1&2 metals– Li2O + H2O 2Li+ + 2OH-
– CaO + H2O Ca2+ + 2OH-
Common Acid Reactions
• nonmetal oxides (aka. acid anhydrides) turn into acids when placed in water– SO2 + H2O H2SO3
– CO2 + H2O H2CO3
– Cl2O7 + H2O 2H+ + 2ClO4-