ACIDS & BASES
Arrhenius Theory 1. in aqueous solution 2. Acid: produces H + 3. Base: produces OH -
HA H 3 O + + A - Acid O H H HA + O H H H + + A -
HCl(g) + H 2 O H 3 O + (aq) + Cl - (aq) CH 3 COOH(l) + H 2 O = H 3 O + (aq) + CH 3 COO - (aq)
careless, but often seen HCl H + + Cl - CH 3 COOH H + + CH 3 COO -
Base NaOH (s) Na + (aq) + OH - (aq)
Arrhenius acid/base reaction acid + base H 2 O + a salt HA + MOH HOH + MA
Monoprotic acid: HCl HCl(aq) + NaOH(aq) H 2 O(l) + NaCl(aq) H + + Cl - + Na + + OH - H 2 O + Na + + Cl - H + + OH - H 2 O HCl
Diprotic acid: H 2 SO 4 H 2 SO 4 (aq) + 2NaOH (aq) 2H 2 O(l) + Na 2 SO 4 (aq) H + + OH - H 2 O H 2 SO 4
Triprotic acid: H 3 PO 4 Polyprotic H 3 PO 4 (aq) + 3NaOH (aq) 3H 2 O(l) + Na 3 PO 4 (aq) H 3 PO OH - 3 H 2 O + PO 4 3- H 3 PO 4
Bronsted-Lowry Theory 1. aqueous & nonaqueous solutions 2. Acid: species donating a proton HCl H + + Cl - H 2 SO 4 H + + HSO 4 - CH 3 COOH H + + CH 3 COO -
Bronsted-Lowry Theory 3. Base: species accepting a proton OH - + H + HOH H 2 O + H + H 3 O + NH 3 + H + NH 4 +
Conjugate acid-base pairs acid 1 + base 1 acid 2 + base 2 conjugate pairs HF + HOH
Conjugate acid-base pairs conjugate pairs HF + HOH H 3 O + + F - acid 1 + base 1 acid 2 + base 2
ALL Arrhenius reactions are Bronsted-Lowry reactions HCl + NaOH H 2 O + NaCl
NOT all Bronsted reactions are Arrhenius reactions CH 3 COOH + NH 3 NH CH 3 COO -
Amphiprotic = Amphoteric Can act as either an acid or a base HCl + HOH H 3 O + + Cl - NH 3 + HOH NH OH - NH 3 + OH - NH HOH HOH + HOH H 3 O + + OH -
ACID STRENGTH Relative ability of a compound to donate a proton Base strength is considered a result, not a cause
Strong acid 100% dissociation Weak acid <100% dissociation Notice this is NOT related to concentration REVIEW
Electronegativity is the most significant factor influencing the strength of acids & bases
HF > HCl > HBr > HI as acids in non- aqueous solvents, or as pure gases
Look at difference in electronegativities 2.1 H - F H - Cl H - Br H - I 2.5
Most “ionic” is the most acidic Nonpolar Polar Ionic E 0 E 1.7 E 4.0
However, as acids in aqueous solution HF < HCl = HBr = HI
2.1 H - O 3.5 competition! 2.1 H - F H - Cl H - Br H - I 2.5
Is methane acidic as a gas or in aqueous solution? 2.1 H - C 2.5
The strength of oxy-acids are also dependent on electronegativity.
Oxy-acids and bases have the same fundamental structure
NaOH: Na - O - H HClO: Cl - O - H
In water, the more “ionic” bond dissociates, forming the acid or base
NaOH: Na - O - H HClO: Cl - O - H
Are alcohols acids or bases? C - O - H
Acids in homologous series are of different strength
Acid Strength H 2 SO 4 > H 2 SO 3 HNO 3 > HNO 2 HClO 4 > HClO 3 > HClO 2 > HClO
Structurally H 2 SO 4 = O 2 S(OH) 2 H 2 SO 3 = OS(OH) 2
Need to examine formal charge of central atom.
Acid Strength CH 3 COOH> CH 3 CH 2 OH CF 3 COOH > CH 3 COOH
Need to examine inductive effect of neighboring atoms.
pH pK K a, K b, K w
2H 2 O H 3 O + + OH -
K eq [H 2 O] 2 = [H 3 O + ][OH - ] K w = [H 3 O + ][OH - ] where K w (25 o C ) = 1 x
in a neutral solution [H 3 O + ] = [OH - ] 1 x = [H 3 O + ] 2 = [OH - ] 2 [H 3 O + ] = [OH - ] = 1 x 10 -7
pX = -log X pK = -log K pH = -log [H 3 O + ] pOH = -log [OH - ]
leveling effect of H 2 O limits [H 3 O + ] & [OH - ] to that controlled by H 2 O
upper limit [H 3 O + ] = 1 lower limit [H 3 O + ] = 1 x
pH scale acid neutral base highest [H 3 O + ] on left lowest [H 3 O + ] on right
[H 3 O + ] and [OH - ] must be considered together
K w = [H 3 O + ][OH - ] -log K w = -log {[H 3 O + ][OH - ]} -log K w = {-log [H 3 O + ]} + {-log[OH - ]}
pK w = pH + pOH but K w = 1 x = pH + pOH
Relationship between conjugate acids & bases HA + H 2 O H 3 O + + A - A - + H 2 O HA + OH -
K a x K b = [H 3 O + ][OH - ] = K w
K a. K b = [H 3 O + ][OH - ] = K w K a. K b = K w
SUMMARY pH = -log [H 3 O + ] pOH = -log [OH - ] [H 3 O + ][OH - ] = 1 x pH + pOH = 14 K a. K b = K w
Applications of Acid-Base Concepts
for weak acids & bases, refer to Appendix H for K a & Appendix I for K b values in Kotz & Treichel
1. What is the pH of a solution that is M KOH?
2. What is the pH of a 0.20 M acetic acid solution?
mL of 0.10 M CH 3 COOH are mixed with 20.0 mL of 0.10 M NaOH. What is the pH of the solution?
4. Calculate the percent ionization of 0.10 M methylamine (CH 3 NH 2 ).
pH of Salts & Oxides
What effect does the addition of a salt to water have upon the pH of the water?
H 2 O equilibrium is the prime factor in the behavior of solutions.
pH of a salt solution is dependent upon the strength of the salt as an electrolyte.
Example 1 NaCl(s) + HOH NaOH(aq) + HCl(aq)
Example 1 NaCl(s) + HOH NaOH (aq) + HCl(aq) strong base strong acid Na + + OH - + H + + Cl - Na + + HOH + Cl -
thus, NaCl in water has NO effect on pH
Example 2 NaCN(s) + HOH NaOH(aq) + HCN(aq)
Example 2 NaCN(s) + HOH NaOH (aq) + HCN(aq) strong base weak acid Na + + OH - + HCN
CN - is the anion of the weak acid HCN CN - + HOH HCN + OH -
NaCN(s) + HOH Na + + OH - + HCN strong base weak acid
thus, NaCN in water produces a/n ?? solution
thus, NaCN in water produces a BASIC solution
5. What is the pH of a M sodium cyanide solution?
Example 3 NH 4 Cl(s) + HOH NH 4 OH (aq) + HCl(aq)
Example 3 NH 4 Cl(s) + HOH NH 4 OH (aq) + HCl(aq) weak base strong acid NH 4 OH + H + + Cl -
NH 4 + is the cation of the weak base NH 4 OH NH HOH NH 3 + H 3 O +
NH 4 Cl(s) + HOH -> NH 4 OH + H + + Cl - weak base strong acid
thus, NH 4 Cl in water produces a/n ?? solution
thus, NH 4 Cl in water produces an ACID solution
6. What is pH of a 0.10 M ammonium chloride solution?
Example 4 NH 4 CN(s) + HOH NH 4 OH (aq) + HCN(aq) weak base weak acid
NH 4 + is the cation of the weak base NH 4 OH NH HOH NH 3 + H 3 O +
CN - is the anion of the weak acid HCN CN - + HOH HCN + OH -
thus, NH 4 CN in water produces a/n ?? solution
The pH of a solution formed from the cation of a weak base and the anion of a weak acid is dependent on the relative strength of the weak acid and weak base.
K a (HCN) = 6.2 x [Text: Table 5.1] Appendix H A-23 K b (NH 4 OH) = 1.8 x [Text: Table 5.3] Appendix I A-25
thus, NH 4 CN in water produces a/n ?? solution
thus, NH 4 CN in water produces a BASIC solution, because the weak base is stronger (ionizes more) than the weak acid
Acidity of Oxides
SO 2 + HOH ??
SO 2 + HOH H 2 SO 3 [O 2 ] H 2 SO 4
SO 2 + HOH H 2 SO 3 [O 2 ] H 2 SO 4 Covalent oxides are acidic & are referred to as acid anhydrides
Na 2 O + HOH ??
Na 2 O + HOH 2NaOH (aq)
Ionic oxides are basic & are referred to as basic anhydrides
Lewis Acid-Base Theory
Acid substance capable of accepting an e - pair
Lewis acid must have an empty valence level orbital i.e. H + has an empty 1s orbital which can accept an e - pair
Thus, H + is an acid under all three theories Arrhenius Bronsted-Lowry Lewis
Lewis Acid-Base Theory Acid: substance capable of accepting an e - pair Base substance capable of donating an e - pair
Examples of Lewis bases OH -, NH 3, F - all have unbonded pairs of e - available for donation
Elements of Group 13 (3A) form compounds that make excellent Lewis acids
another “typical” Lewis acid-base reaction:
Reaction of a Lewis Acid and Lewis Base New bond formed using electron pair from the Lewis base. Coordinate covalent bond Notice geometry change on reaction.
Formation of hydronium ion is also an excellent example. Lewis Acids & Bases Electron pair of the new O-H bond originates on the Lewis base.
Lewis Acid/Base Reaction
H 3 BO 3 + H 2 O H 2 BO H 3 O + ? NO!
H 3 BO 3 + 2H 2 O B(OH) H 3 O +
is Al(OH) 3 an acid or base?
Amphoterism of Al(OH) 3
This explains AMPHOTERIC nature of some metal hydroxides. Al(OH) 3 (s) + 3 H + Al H 2 O Here Al(OH) 3 is a Brønsted base. Al(OH) 3 (s) + OH - Al(OH) 4 - Here Al(OH) 3 is a Lewis acid. Lewis Acids & Bases
Transition metal ions also very good Lewis Acids
Other good examples involve metal ions. Lewis Acids & Bases
Zn 2+ + HOH ?.. Zn 2+ => [Ar] 4s 0 3d 10 4p 0 Zn(H 2 O)
Reaction of NH 3 with Cu 2+ (aq)
Formation of complex ions is a Lewis acid-base reaction
Lewis Acid-Base Interactions in Biology The heme group in hemoglobin can interact with O 2 and CO. The Fe ion in hemoglobin is a Lewis acid O 2 and CO can act as Lewis bases Heme group
Lewis Bronstead Arrhenius Inclusiveness of the Acid/Base Definitions