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What does the Ionic Equilibria revision sheet cover?

Strong vs Weak Electrolytes, Strong electrolyte, Weak electrolyte, Degree of Dissociation, fraction of total moles that dissociates at equilibrium, percent dissociation, equilibrium concentration of either ion for a 1:1 electrolyte, initial concentration c, Acids, Bases and pH, Arrhenius, Bronsted-Lowry, Lewis, Amphoteric Nature of Water.

Is this for Class 12 Maharashtra HSC Chemistry?

Yes, it is written for the Maharashtra HSC Chemistry syllabus.

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Ionic Equilibria — Class 12 Maharashtra HSC Chemistry revision notes

A 5-page visual revision sheet for Ionic Equilibria, written for Class 12 Maharashtra HSC Chemistry. Formulas, diagrams and the traps that cost marks, laid out to be read the night before rather than the term before. Free, and it opens inside CapCompass.

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Ionic Equilibria in one look

how far an electrolyte splits, and what that split does to pH

Strong vs Weak Electrolytes

Strong electrolyte

ionises completely, or almost completely
strong acids, strong bases and salts
e.g. HCl, HNO_3, H_2SO_4, NaOH, KOH

Weak electrolyte

ionises only partially, an equilibrium survives between ions and unionised molecules
weak acids and weak bases
e.g. CH_3COOH, HCOOH, HF, H_2S, NH_4OH

Degree of Dissociation

fraction of total moles that dissociates at equilibrium α=fracmoles dissociatedtotal moles
percent dissociation \% dissociation=α×100
equilibrium concentration of either ion for a 1:1 electrolyte, initial concentration c [ion]=α c

Acids, Bases and pH

Arrhenius: acid: gives H^+ in water; base: gives OH^-. Limited to water, and fails for NH_3, Na_2CO_3 (no OH group)
Bronsted-Lowry: acid donates a proton, base accepts one; conjugate pairs differ by one proton (HCl/Cl^-, H_2O/H_3O^+)
Lewis: acid accepts an electron pair, base donates one; broadest, covers species with no proton

Amphoteric Nature of Water

water acts as a base toward HCl: it accepts a proton, forming H_3O^+ and Cl^-
water acts as an acid toward NH_3: it donates a proton, forming OH^- and NH_4^+
this dual role, acid toward one substance and base toward another, is called amphoteric behaviour

Ionisation Constants

acid dissociation constant, HA to H+ and A- K_a=[H^+][A^-]/[HA]
base dissociation constant, BOH to B+ and OH- K_b=[B^+][OH^-]/[BOH]

Page 1 of 5. The full sheet, all 5 pages, opens free in the app.

What this Ionic Equilibria sheet covers

Strong vs Weak Electrolytes
Strong electrolyte
Weak electrolyte
Degree of Dissociation
fraction of total moles that dissociates at equilibrium
percent dissociation
equilibrium concentration of either ion for a 1:1 electrolyte, initial concentration c
Acids, Bases and pH
Arrhenius
Bronsted-Lowry
Lewis
Amphoteric Nature of Water
Ionisation Constants
acid dissociation constant, HA to H+ and A-
base dissociation constant, BOH to B+ and OH-
Ostwald's Dilution Law
exact form, weak acid, initial concentration c
for a weak acid α is small, so 1-α ≈ 1
degree of dissociation follows
the same relations hold for a weak base, with K_b
pH: which formula applies
pH of a weak acid from Ka
Autoionization of Water and Kw
self ionisation of water
ionic product of water
at 298 K
pH and pOH
pH
pOH
relationship, from K_w at 298 K
Acidity, Basicity and Neutrality
Hydrolysis of Salts
Types of Salt Hydrolysis
Strong acid, strong base
Strong acid, weak base
Weak acid, strong base
Weak acid, weak base
Buffer Solutions
Henderson-Hasselbalch Equation
pH of an acidic buffer
pOH of a basic buffer
the p-scale definitions used above
Buffer Action, Properties and Applications
Strong acid-strong base titration
Solubility Product
general sparingly soluble salt
in terms of molar solubility S
Condition of Precipitation
Common Ion Effect
Traps that cost marks
Tricks that save time

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