Acid & Bases

The magnitude of Ka indicates the tendency of an acid to ionize in water. Since [H+] is found in the numerator of the equilibrium constant expression for the dissociation of an acid, a stronger acid will have a larger Ka val

Weak acids

Citric acid (C8H6O7) is a weak acid

Acetic acid is a weak acid

Common weak acids:

• HF

• HCN

• H2SO3

• CH3COOH (acetic acid)

• HXO2

• H2CO3

• HNO2

• HXO

• Organic acids —> carbon carbon

• X = Cl, Br, I

K = (Ka*Kb)/Kw

Big sized atom bonded to H leads to weaker and longer chemical bond, which results in a higher acidity due to the increased ability of the acid to donate protons.

In contrast, smaller atoms like fluorine form stronger bonds with hydrogen, resulting in lower acidity as they hold onto protons more tightly.

increasing ionic radius gives more volume to spread -1 charge over & minimize electron-electron repulsions

what does the ICE box stand for? Initial, Change, Equilibrium concentrations

% dissociation = [conjugate base equilibrium]/ [acid] initial * 100

pH decreases as [H3O+) increases

amphoteric = can act as both base & acid

water is amphoteric

Solution is neutral

• [H3O+]=[OH-]

Acidic

• [H3O+] > [OH-]

Basic

• [H3O+] < [OH-]

Why does water auto-ionization occur? because of entropy

Water autoionizlewation is endergonic. Reactants are favored

Lewis acid = accepts pair of electrons

Lewis base = donates pair of electrons

Bronsted dowry acid = donates proton

Bronsted dowry base = accepts proton