ACIDS AND BASES for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet
Learning objectives Name and write formulae for common acids and bases Describe acids and bases according to Arrhenius and Brønsted definitions Identify conjugate acid-base pairs Distinguish between strength and concentration in acid-base terminology Calculate and estimate ph of acids and bases Describe basic principles of buffer solutions
ACIDS AND BASES The meaning of acid and base has changed over the years Arrhenius acid is one that generates protons when dissolved in water Arrhenius base is one that generates hydroxide ions when dissolved in water
Hydronium ion is the active ingredient of an acid Protons do not exist in solution CH 3 CO 2 H + H 2 O = H 3 O + + CH 3 CO 2 - Vinegar in water produces hydronium ions
Hydroxide ion is the active ingredient of a base NH 3 + H 2 O = NH 4+ + OH - Ammonia, a base, dissolves in water and produces hydroxide ions
Neutralization The mixing of an acid with a base: ACID + BASE = SALT + WATER The reaction of carbonic acid (CO 2 in H 2 O) to give limestone: H 2 CO 3 + Ca(OH) 2 = CaCO 3 + 2H 2 O ACID BASE SALT WATER
The essence of neutralization Elimination of the components of acid and base by combination to give H 2 O Reflection of strong O H bond H + + OH - H 2 O ACID BASE
Brønsted and Lowry A broader definition of acids and bases In the reaction NH 3 + HCl = NH 4 Cl has all the elements of acid-base neutralization but no H 2 O as would be required in the Arrhenius definition Brønsted acid donates a proton Brønsted base accepts a proton
Brønsted acid HCl + H 2 O = H 3 O + + Cl -
Brønsted base NH 3 + H 2 O = NH 4+ + OH - water NH 3 + HCl = NH 4+ Cl - No water
Substances can be both acids and bases depends on environment Note that in one instance H 2 O behaves like a base accepting protons, and in another, behaves like an acid donating protons HCl + H 2 O = H 3 O + + Cl - In presence of an acid H 2 O is a base NH 3 + H 2 O = NH 4+ + OH - In presence of a base H 2 O is an acid
The products are themselves acids and bases
Equilibrium: solution contains mixture of all components
Conjugate acids and bases Conjugate acid-base pair differs by H + Conjugate base base Conjugate acid acid HA + B A - + HB + Conjugate acid-base pair Conjugate acid-base pair
Identifying conjugate acid-base pairs: follow the protons
Salts Products of acid-base neutralization HCl + NaOH = NaCl + H 2 O HCl + KOH = KCl + H 2 O HNO 3 + KOH = KNO 3 + H 2 O 2HCl + Ca(OH) 2 = CaCl 2 + 2H 2 O HCN + NaOH = NaCN + H 2 O
Strength and concentration Not all acids completely donate the protons to water molecules in solution HA + H 2 O A - + H 3 O + The degree of ionization is described by strength The total number of moles per unit volume is described by concentration
HCl is completed converted to H 3 O + and Cl -
Acetic acid is only partly ionized
Graphical illustration of weak acid dissociation
Changing concentration does not change strength Strength refers to degree of ionization: Strong is completely ionized (100 %) Weak is partly ionized (1 % - 1:10 6 ) Concentration refers to number of moles per unit volume An acid (or base) can be strong and concentrated, weak and concentrated, strong and dilute, weak and dilute
Amphotericity A substance that behaves as an acid and a base is amphoteric. Water is a good example Acid Base
Ionization of water Even in pure water, a fraction of the molecules are ionized and the concentrations of OH - and H 3 O + are equal H 2 O + H 2 O = H 3 O + + OH - [H 3 O + ] = [OH - ] Concentration
In all aqueous solutions, product of concentrations is a constant [H 3 O + ][OH - ] = constant Increasing [H 3 O + ] decreases [OH - ] (acidic conditions) Increasing [OH - ] decreases [H 3 O + ] (basic conditions)
The ph scale reduces large range of numbers to small In water [H 3 O + ][OH - ] = 10-14 ph = - log 10 [H 3 O + ] Range of [H 3 O + ] 10 M 10-14 M Range of ph -1 to +14 Low ph = acid; high ph = basic ph = 7 = neutral
Relating ph to [H 3 O + ] For ph, take exponent of [H 3 O + ], change sign 10-1 M (0.1 M) HCl has ph = 1 Pure water has [H 3 O + ] = 10-7 M, ph = 7 Ammonia has [H 3 O + ] =10-11 M, ph = 11 Note: change of 1 unit in ph is factor of ten
ph scale and common substances
Estimating ph Estimating ph is often more useful than doing exact calculations Smaller ph value means larger H + concentration Estimating ph
Smaller ph value means larger H + concentration ph = - log 10 [H 3 O + ] [H 3 O + ] = 10-4 ph = - log 10 (10-4 ) = 4 [H 3 O + ] = 4 x 10-4 ph = - log 10 (4 x 10-4 ) = - log 10 4 - log 10 (10-4 ) = 4 log 10 4 =4 0.602 = 3.4 Calculating ph Concentration 1 x 10-4 M ph = 4 Concentration 4 x 10-4 M ph = 3.4
ph and poh In any aqueous solution, [H + ] x [OH - ] = 10-14 Obtain [H + ] given [OH - ] poh = -log 10 [OH - ] ph + poh = 14
Examples of ways to get [H + ] from [OH - ]
Relationships between [H + ], ph and [OH - ]
Buffer solutions control ph In biological systems it is often critical for stable function to maintain a specific ph environment. Buffer solutions perform this function they resist large changes in ph when either acids or alkalis are added
Buffer solution contains a combination of a weak acid and its salt
Mechanism follows Le Chatelier s principle Addition of H + converts CH 3 CO 2- to CH 3 CO 2 H CH 3 CO 2- + H + CH 3 CO 2 H Addition of OH - converts CH 3 CO 2 H to CH 3 CO 2 - CH 3 CO 2 H + OH - CH 3 CO 2- + H 2 O In general, Add OH - shifts equilibrium to right (HA A - ) HA + H 2 O A - + H 3 O + Add H + shifts equilibrium to left (A - HA)
Mechanism depends on equilibrium Addition of acid converts CH 3 CO 2- to CH 3 CO 2 H CH 3 CO 2- + H + CH 3 CO 2 H Addition of base converts CH 3 CO 2 H to CH 3 CO 2 - CH 3 CO 2 H + OH - CH 3 CO 2- + H 2 O