TABLES
S.No Substance Colour
&State Taste Solubility
1. Sodium
acid phosphate Colour less crystals Saline Freely
soluble in water
2. Sodium
bicarbonate White Saline Freely soluble in H20
3. Sodium
citrate Colourless crystals
Saline Very soluble in boiling H2O
4. Magnesium
sulphate Colourless Saline, Bitter Freely soluble in H2O
5. Sodium
potassium tartarate Colour less Salty Freely soluble in H2O
crystals
6. Sodium
sulphate (Na2So4) White crystalline Saline,
Bitter Freely soluble in water
7. Magnesium
chloride Colour less crystals Bitter Freely
soluble in water
8. Ferrous
sulphate Pale green or pale
Astringent, Freely soluble in water,
bluish green metallic taste Very soluble in boiling water
9. Ferrous
gluconate Yellowish grey Burnt sugar Freely soluble in water
10 Potassium
iodide Colourless Slight bitter, Very soluble in water
salty
11. Aluminium
sulphate White crystalline powder Slight sweet Freely
soluble in water
12. Ammonium
chloride Colour less Saline Freely soluble in water
13. Calamine Pink or reddish Taste less Insoluble in water, soluble
brown in mineral acids
14. Potassium
permanganate Dark purple with Sweet and Soluble in water
metallic luster astringent
15. Silver
nitrate Colourless
crystals Bitter, metallic Highly soluble in water
16. Iodine Bluish black with -- Freely
soluble in chloroform
metallic luster , Carbon tetra
chloride, CS2.
17. Povidone
iodine Yellowish brown -- Soluble
in water
powder
18. Precipitated
sulphur Pale greenish yellow Taste less Completely
soluble in CS2
19. Sublimated
sulphur Yellow colour -- Soluble only to the exact of
about 80% in CS2
20. Heavy
kaolin Whitish or
yellowish Earthy of clay Insoluble in water
white like
21. Light kaolin White
Taste less Insoluble in water & mineral
acid
22. Aluminium
hydroxide gel White Tasteless Soluble in dilute mineral
acids and in an excess of
caustic
alkali solution
23. Barium
sulphate White powder Tasteless Insoluble in water
24. Bentonite Pale buff colour Slightly earthy Insoluble in water but swells
in to a homogenous mass
25. Calcium
gluconate White Taste less Freely soluble in boiling
water
26. Calcium
hydroxide White powder Alkaline and Soluble in glycerin and in
slightly
bitter aqueous solution of sugars
27. Calcium
lactate White powder Slight or not Readily soluble in hot water
unpleasent
28. Dibasic
calcium White powder Tasteless Insoluble in water, Soluble
phosphate in
Dil.HCl, Dil.HNO3
29. Tribasic
calcium phosphate White powder Tasteless Insoluble in water, Soluble
in Dil.HCl, Dil.HNO3
30 Ferrous
fumarate Reddish
orange to Slightly Slightly soluble in water
reddish brown powder astringent
31. Magnesium
trisilicate White Tasteless Insoluble in water
32. Potassium
bromide Colourless crystals Saline and Soluble in water and glycerin
slightly
bitter
33. Potassium
citrate White granular
crystals Saline Very soluble in water
34. Potassium
chloride Colourless crystals Saline Freely
soluble in water
35. Sod.
Benzoate White Saline, Freely soluble in water
36. Sodium
chloride Colourless Saline Freely soluble in water
37. Sod
hydroxide White sticks -- Freely soluble in water &
alcohol
38. Sodium
lauryl sulphate White or pale yellow -- Soluble in water
crystals
39. Sodium
meta bisulphite Colourless Acid and saline Freely
soluble in water
40. Sodium
phosphate Colourless -- Freely soluble in water
41. Sodium
salicylate Colourless Sweetish, Freely soluble in water
Saline
42. Sodium
thiosulphate Colourless crystals Saline Very
soluble in water
43. Talc White Tasteless Insoluble in water
44.
Titanium dioxide White Tasteless Insoluble in water, slowly
soluble in hot H2SO4
45. Zinc
chloride White Tasteless Very soluble in water
46. Zinc
oxide White or
white Taste less Insoluble in water
yellowish powder
47. Zinc
sterate White Tasteless Insoluble in water
48. Zinc
sulphate Colourless Astringent Very soluble in water
49. Zinc
undecylenate White or pale -- Insoluble in water
yellowish white
Table II
List of synonyms of inorganic
medicinal compounds
S.No. INORGANIC COMPOUND SYNONYM
1. Potassium aluminium sulphate Alum
2. Ammoniated mercury Aminochloride
of mercury
3. Aluminium oxide Corundum
4. Aromatic spirit of ammonia Spirit
of Sal. volatile
5. Solid carbondioxide Dry
ice
6. Antimony sodium tartarate Tartar
emetic
7. Barium sulphate compound powder Barium meal, Shadow meal
8. Borax Sodium
tetra borate
9. Calamine Prepared
calamine
10. Calcium hydroxide Slaked
lime
11. Copper sulphate Blue
vitriol
12. Aqueous iodine solution Lugol’s
solution
13. Aromatic Sulphuric acid Elixir
of vitriol
14. Aluminumacetate solution Burrow’s
solution
15. Bentonite Soap
clay
16. Compound sod.chloride solution Ringer’s
injection
17. Chlorinated lime Bleaching
powder
18. Calcium carbonate Precipitated
chalk
19. Calcium oxide Quick
lime
20. Chlorinated lime & Boric acid sol. Eusol
21. Dried sodium phosphate Exsiccated
slamber’s salt (or)
Exsiccated
sodium sulphate
22. Dicalcium phosphate Dibasic
calcium phosphate
23. Heavy kaolin China
clay
24. Iron and ammonium citrate Ferric
ammonium citrate
25. Lead acetate Sugar
of lead
26. Magnesium sulphate Epsom
salt
27. Magnesium hydroxide mixture Milk
of magnesia
28. Mercury with chalk Grey
Powder
29. Mercurous Chloride Calomel
30. Potassium iodide Kalli
idodium
31. Nitrous oxide Laughing
gas
32. Plaster of Paris Gypsum
33. Potassium acid tartarate Potassium
hydrogen tartarate
34. Potassium nitrate Indian
salt petre
35. Potassium hydroxide Caustic
potash
36. Sodium bicarbonate Baking
soda
37. Sodium chloride injection Normal saline solution for injection
38. Sodium hydroxide Caustic
soda
39. Sodium nitrate Chile
40. Sodium potassium tartarate Rochelle
salt
41. Sodium sulphate Glauber’s
salt
42. Sodium thiosulphate Hypo
43. Sodium metaphosphate Madrell’s
salt [Graham’s salt ]
44. Silver nitrate Luhar
caustic
45. Weak solution of iodine Iodine
tincture
46. Zinc sulphate White
vitriol
47. Zinc
oxide compound paste Zinc
paste
48. Zinc gelatin Unna
49. Ferrous sulphate Green
vitriol
Table III
S: No Inorganic medicinal Chemical
formula Medicinal use
chemical
compound
1. Alum KAl(SO4)2. 12H2O Astringent, Styptic(Stops bleeding)
2. Aluminium
hydroxide Al(OH)3 Antacid
3. Ammoniated
mercury NH2HgCl Local anti-infective
4. Ammonium
chloride NH4Cl Expectorant, Diuretic & Systemic
Acidifier
5. Antimony
potassium C4H4O7Sbk. ½ H2O Emetic orally and treatment of Kala-
tartarate azar
by I.V
6. Barium
sulphate BaSO4 Radio-opaque contrast media for the
x-ray examination of GIT
7. Borax Na2B4O7. 10H2O Antibacterial
8. Boric acid H3BO3 Local anti-infective
9. Calcium carbonate CaCO3 Non-systemic antacid
10. Calcium chloride CaCl2 Electrolyte replenisher
11. Calcium gluconate C12H22O14Ca.H2O Calcium replenisher
12. Chlorinated lime CaOCl2 Electrolyte replenisher
13. Dicalcium phosphate CaHPO4. 2H2O Source of calcium, phosphorus and
diluent in tablets.
14. Ferrous sulphate FeSo4. 7H2O Haematinic
15. Hydrogen peroxide H2O2 Oxidising agent
16. Light kaolin Al2O3.2SiO2. 2H2O Adsorbent (GIT infections)
17. Magnesium hydroxide Mg (OH)2 Antacid and laxative
18. Magnesium oxide MgO Antacid
19. Magnesium sulphate MgSo4. 7H2O Saline cathartic and sedative by I.V/ I.M
20. Magnesium trisilicate 2MgO. 3SiO2. XH2O Antacid
21 Mercurous chloride HgCl Cathartic
22. Nitrous oxide N2O General anaesthetic
23. Phosphoric acid H3PO4 Pharmaceutical aid
24. Plaster of Paris CaSO4. ½ H2O For making bandages, surgical aid.
25. Potassium chloride Kcl Electrolyte replenisher
26. Potassium citrate C6H5K3O7. H2O Systemic alkaliser
27. Potassium iodide KI Expectorant
28. Potassium permanganate KMno4 Antiseptic, oxidising agent
29. Selenium sulphide SeS2 Antidandruff
30. Silver nitrate AgNO3 Antibacterial
31. Sodium acetate CH3COONa. 3H2O Preparation of peritoneal dialysis fluid
32. Sodium benzoate C6H5COONa preservative
33. Sodium bicarbonate NaHCO3 Systemic antacid
34. Sodium carbonate Na2CO3 Pharmaceutical aid
35. Sodium chloride NaCl Electrolyte replenisher
36. Sodium dihydrogen
phosphate C6H5Na3O7. 2H2O Urinary acidifier
37. Sodium fluoride. NaF To prevent dental caries
38. Sodium hydroxide NaOH Pharmaceutical aid
39. Sodium metabisulphite Na2S2O5 Antioxidant
40. Sodium nitrite NaNO2 Antidote in cyanide poisoning
41. Sodium potassium tartarate C4H4KNaO6. 4H2O Saline cathartic
42. Sodium thiosulphate Na2S2O3. 5H2O Antidote in cyanide poisoning
43. Stannous fluoride SnF2 Prevention dental caries
44. Strontium chloride SrCl2 Desensitizing
agent in tooth preparations.
45. Talc 3MgO.4SiO2.H2O Glidant in tablets, filter medium and
used in dusting powders.
46. Titanium dioxide TiO2 Topical protective, opacity agent
47. Yellow mercuric oxide HgO Local
antibacterial
48. Zinc chloride ZnCl2 Pharmaceutical aid
49. Zinc oxide ZnO Mild astringent
50. Zinc sterate (C17H35COO)2 Zn Lubricant
51. Zinc sulphate ZnSo4.7H2O Astringent & Anti septic
Table-IV
Solubilities
Descriptive phase Volume
of solvent dissolving in
part of solvent
Very
soluble Less than
one part
Freely
soluble 1 to 10
parts
Soluble 10 to 30 parts
Sparingly
soluble 30 to 100 parts
Slightly
soluble 100 to 1000
parts
Very
slightly soluble 1000 to
10,000 parts
Table V
Classification of solvents
S.No Solvent Definition Examples
1. Protophilic A
solvent that is capable of accepting protons Acetone,
Ether,
from
the solute Liquid
ammonia.
2. Protogenic A
solvent that is capable of donating protons. Formic
acid, Acetic acid,
Sulphuric
acid, Hydrochloric
acid
3. Amphiprotic A
solvent that is capable of donating as well Water,
Alcohol
as
accepting protons
4. Aprotic A
solvent that neither accept nor donate Hydrocarbons
protons
Table VI
S.No Limit test Principles
1. Limit test for chlorides It is based on the
formation of the opalescence due to inter
reaction of chlorides present
in the substance with silver
nitrate
in presence of nitric acid and it is compared with a
standard
opalescence produced by definite amount of
chlorides
(NaCl )
2. Limit test for sulphates It is based on the
formation of turbidity due to interaction of
sulphates present in substance
with barium chloride in
presence
of hydrochloric acid, and it is compared with a
standard
turbidity produced by definite amount of sulphates
(K2SO4)
3. Limit test for Iron It is based on the
formation of purple colour due to the
interaction
of thioglycollic acid with iron in the presence
of
citric acid and in ammonical alkaline medium. It is
compared
with standard purple colour produced by definite
amount
of iron.
4. Limit test for Lead It is based on the
violet colour produced in chloroform due
to the reaction between lead
impurity and dithizone which
results
in the formation of lead dithizonate. The intensity of
final
violet colour produced in the chloroform medium is
compared
with standard.
5. Limit test for Arsenic (Gutzeit
Test) It is based on the formation of
yellow stain on mercuric
chloride paper by arsine gas
which is produced by
reduction
of arsenic compound with zinc and HCl in the
presence
of potassium iodide. The yellow stain is compared
with
standard.
6. Limit test for heavy metals It is based on the reaction
between Hydrogen sulphide and
(Lead,
Antimony, Bismuth, Tin & Cobalt) heavy metals in an acidic
medium to produce the metal
sulphides
(Brown colour). It is compared with standard
containing
definite quantity of lead nitrate.
Table VII
S.No Limit
tests Reagent Use
1. Limit test for chlorides Nitric acid Prevent opalescence being caused due to
silver carbonates or CO2 or
alkaline
impurities
2. Limit test for sulphates Barium sulphate reagent:
a) Barium chloride To produce turbidity
b)
Potassium sulphate Increases
sensitivity of the test by giving
ionic
concentration in the reagents which
just
exceeds the solubility of BaSo4
3. Limit test for iron i) Thioglycollic acid Strong reducing agent which reduces
ferric to ferrous and produce
purple colour
ii) Citric acid Prevents precipitation of
iron with
ammonia
4. Limit test for arsenic Potassium iodide Helps in the reduction of
pentavalent
(Modified Gutziet Test) arsenic
acid into trivalent arsenic acid
Granulated
zinc Produces steady evaluation
nascent
hydrogen
Stannous
chloride Reducing agent
Table VIII Assays
S.No Chemical compound Method
(titration) Principle (By
titration with standard
solution)
1. Boric
acid Acid-base Sodium hydroxide
using phenolphthalein
as indicator. Glycerin is added
to convert
boric
acid into strong acid
2. Sodium
bicarbonate Acid-base Standard solution
of hydrochloric acid
using methyl orange solution as
an
indicator
3. Ammonium
chloride Acid-base Sodium hydroxide
using phenolphthalein
as an indicator
4. Calcium
gluconate Complexometric titration M/20
disodium edetate using mordant
black-II mixture as an
indicator
5. Calcium
lactate Complexometric
titration M/20 disodium edetate using
mordant
black-II mixture as an
indicator
6. Magnesium
sulphate Complexometric titration Disodium edetate using mordant black-II
mixture as an indicator
7. Zinc sulphate Complexometric titration Disodium edetate using Xylenol
orange
as an
indicator
8. Ferrous gluconate Oxidation-reduction Cerric ammonium sulphate
using ferroin
sulphate
solution as an indicator
9. Ferrous sulphate Oxidation-reduction Cerric ammonium sulphate
using ferroin
sulphate
solution as an indicator
10. Hydrogen peroxide Oxidation-reduction Potassium permanganate
solution in
presence of sulphuric
acid
11. Chlorinated lime Oxidation-reduction Sodium thiosulphate using
starch
(Iodometry) mucilage
as an indicator
12. Potassium permanganate Oxidation-reduction By using oxalic acid solution, which is
titrated with
pot. permanganate solution
which
is a self indicator.
13. Iodine Iodometry Sodium
thiosulphate using starch
mucilage as an
indicator
14. Copper sulphate Iodometry Sodium
thiosulphate using starch
mucilage as an
indicator
15. Sodium chloride Volhard’s method Ammonium
thiocyanate using ferric
ammonium
sulphate as an indicator.
16. Yellow mercuric oxide Thiocyanate method Ammonium thiocyanate using
ferric alum
as
an indicator
Table IX
S.No Method of titration Example
of compounds assayed
1. Acid-alkali
method Ammonium
chloride
2. Complexo
metric titration Calcium
gluconate, Magnesium sulphate and zinc
sulphate
3. Non-aqueous
titrations Sodium
citrate, Potassium citrate and sodium acetate
4. Gravimetric
method Barium
sulphate, Magnesium trisilicate and disodium
auro-thiomalate
5. Precipitation
titrations Silver
nitrate, Sodium chloride and potassium chloride
6. Oxidation-Reduction method
a) Permanganometry Potassium
permanganate and Hydrogen peroxide
b) Iodometry Iodine,
Copper sulphate, Chlorinated lime and sodium
thiosulphate
c) Cerimetry Ferrous
gluconate and ferrous sulphate
Table X Pharmaceutical
analytical techniques
S.No Method Description Examples
1. Spectral
method Based on the use of
light absorbtion Visible
spectroscopy,
(or) emission characteristics
of drugs Ultraviolet spectroscopy
Flourimetry, Nephlometry,
Infra red spectro metry,
NMR spectro scopes,
ESR spectroscopy,
Mass spectroscopy
2. Chromatographic
method Based on the use of
affinity(or)partition Thin layer
chromatography,
co-efficiant differences between
drugs Paper chromatography,
Gas chromatography,
Ion exchange chromatography,
Column
chromatography,
High
pressure liquid
chromatography
3. Electro analytical Based
on the use of electro chemical Potentiometry,
techniques property of drugs. Conductometry,
Polarography, Amperometry,
Paper electrophoresis etc.
4. Biological
and Based on the use of
either animals(or) Biological assay of
some Microbiological methods
micro-organisms for analysis. Vitamins
microbiological
assay
of antibiotics and
vitamins.
5. Radioactive
methods Based on the radio immuno
assay and
related techniques.
6. Physical
methods Based on the use of
measure some Differential Thermal
Analysis,
physical characteristics of drugs (DTA)
Differential Scanning
Calorimetry, (DSC)
Thermo Mechanical Analysis,
(TMA)
Thermo
Gravimetric Analysis.
(TGA)
(TGA)
7. Miscellaneous Like conventional titrimetric
methods,
techniques Polarimetric methods
Table XI Physical
properties used for analysis
S.No Physical property measured Instrumental
methods based on measurement of property
1. Absorbtion of radiation Spectrophotometry
(X-ray, U.V, visible I.R) Calorimetry,
Atomic absorbtion, Nuclear
magnetic resonance and
electron spin
resonance spectroscopy.
2. Emission
of radiation Emission
spectroscopy (X-ray,
U.V, visible)
Flame photometry,
Fluorescence (X-ray, U.V, visible), Radio chemical methods
3. Scattering
of radiation Turbidimetry,
Nephelometry, Raman spectroscopy,
4. Refraction of radiation Refractometry,
Interfero metry,
5. Diffraction
of radiation X-ray,
Electror defraction methods
6. Rotation
of radiation Polarimetry, Optical rotatory dispersion and
circular dichroism
7. Electrical
potential Potentio
metry, chrono potensiometry
8. Electrical
conductance Conductivity
9. Electrical
current Polargraphy,
Amperometric titrations
10. Quantity
of electricity Coulometry
11. Mass-to-charge
ratio Mass spectrometry
12. Thermal
properties Thermal
conductivity and enthalpy methods
Table XII Hardness
of water
S.No Type of water Due
to the presence of Removal
methods
1. Temporary
hardness of Bicarbonates of
calcium and 1. Boiling
water
(Carbonate hardness) magnesium 2.
Clarke’s process (milk of lime)
2. Permanent hardness of water Chlorides
and sulphates of calcium and 1.
Gan’s permutit process
(Non-carbonate hardness) magnesium (zeolytes)
2.
Calgon process (sodium
hexameta phosphate)
3.
Ion exchange method
PHARMACOPEIAS Editions
of I.P
1. I.P= Indian Pharmacopeia First
edition I.P= 1955
2. B.P=British Pharmacopeia Second
edition of I.P=1966
3. B.P.C= British pharmaceutical codex Third edition of I.P=1985
4. N.F=National formulary Fourth
edition of I.P=1996 (Latest edition)
5. U.S.P= United states Pharmacopeia
6. E.P=European Pharmacopeia
LIST OF PHARMACOPEIAS
1. Indian Pharmacopeia(I.P) 9.
Pharmaceutical codex
2. British Pharmacopeia(B.P) 10.
Merck index
3. British pharmaceutical
codex(B.P.C) 11. British
national formulary
4. National formulary(N.F) 12. United states
5. United
states United states
6. European Pharmacopeia(E.P) 14. Indian
pharmaceutical codex
7. International Pharmacopoeia 15.
Mrtindale extra Pharmacopoeia
8. Japanese Pharmacopoeia
Definitions:
Arhenious theory:
i) Acid: Generates [H+] ion in
solution
ii) Base: Generates [OH-
Eq: Acid+Base Salt+ Water
Eg: HCl+NaOH NaCl +H2O
Bronsted-Lowery theory:
i) Acid: Any thing that donates a H+
(Proton donar)
ii) Base: Any thing that accepts a H+.
(Proton acceptor)
Eq: Acid+Base Acid+Base 
Eg: HNO2+ H2O NO2+ H3O+
[Acid]
[Base]
Lewis theory:
Acid: Accepts an electron pair.
Base: Donates an electron pair
Strong acids: These acids completely ionize
in solution, so they are always represented in chemical equation in their
ionised form.
Eg: H2So4, Hno3, HClo3, HCl, Hbr, HF
Strength of few acids in decreasing order:
HClo4>HBr>H2So4>HCl>HNo3
Weak acids: These acids partially ionize in solution so they
are always represented in chemical equation in their ionized form.
Strong bases: These bases completely ionize
in solution and are always represented in their ionized form in chemical
equations.
Eg:
NaOH, LiOH, KOH, RbOH, Ca(OH)2, Sr(OH)2
pH: It
is defined as the negative logarithm of the concentration of hydrogen ion[H+]
or [H3o+]
in solution
pH=-log10
[H+] or log1/[H+]
·
If
hydrogen ion concentration is one molar the pH becomes “0”.
·
If
hydroxyl ion concentration is one molar the pH becomes 14.
·
The pH 0-7 is acidic and 7-14 is basic
pH=-log [H3O+]
pH+poH=
pKW (Where pKW=14)
pOH=pKW-pH
pH=pKa+log [base/acid]
Buffer: Solution which resists any change in its pH value
on dilution or on addition of small quantity of an acid or alkali.
Buffer action: The process by which added H+
and OH-
Acidic buffer solution: It consist of weak acid and its
salt with a strong base
Eg: CH3COOH+ CH3COONa
Basic buffer solution: It consists of a weak base and
its salt with a strong acid
Eg: NH4OH+ NH4Cl
Buffer capacity Ø: The buffer capacity of a buffer
solution is defined as the number of mole of a strong acid or a strong base
required to change the pH of one litre of a buffer by one unit.
Buffer
capacity (Ø) =
Number
of moles of acid/
Base added to the one litre of the solution
Change in pH
Hard water: Which doesn’t stable lather
readily
with soap solution is called hard water.
Soft water: Which gives stable lather readily with soap
solution is called soft water.
Radio activity: The emission of alpha, beta or
gamma particles due to nuclear decay is called radioactivity.
Bequerel(BQ): it is the unit for the rate of decay
BQ=1Decay/second
Isotopes: The nuclides of the same element having different
mass number are called isotopes.
Their chemical properties are
similar but differ in their physical and radio active properties
Radioactive isotopes: The isotopes which emit
radiations are called radioactive isotopes.
Iso bars: The nuclides of different elements with the same
mass numbers and different atomic numbers are called isobars.
Isobars will have different
physical as well as chemical and radioactive properties.
Curie(Ci): It is the unit representing the rate of decay and is equal
to 3.7X1010 disintegrations /sec
1Ci=3.7X1010
Bq
Rad: It
is the unit of absorbed dose
1Rad=10-2 JKg
-1
Roentgen(R): It is the unit of exposure
1R=2.58X10-4CKg -1
Red Equivalent Man:(REM) It is the unit of dose
equivalent
Dose in REM=Dose in Rads X Quality
factor
X Distribution factor
Half life of Radio Pharmaceuticals
i) Physical half life (Tp): The amount of time
necessary
for the radio active atoms to decay to one half their original number.
Biological half life (Tb): The amount of time required for
the body to metabolize or eliminate one of the administered dose of any
substance through biological process.
Effective half life (Te): The time required for an
administered radiopharmaceutical dose to be reduced by one of due to both
physical and biological decay mechanisms
Te=Tp+Tb
/
TpXTb
Where Te= Effective half life
Tp= Physical half life
Tb=Biological half life
Molarity(M): 1gm molecular weight of solute dissolves in
1000ml of solution.
Molality(m): 1gm molecular weight of solute dissolve in 1000gms
of solution.
Normality(N): 1gm of equivalent weight of
solute dissolves in 1000ml of solution.
Mole fraction(X): The ratio of the moles of one
constituent of a solution to the total moles of all constituents.
Oxidation: Loss of electrons (gain in positive charge)
Reduction: Gain of electrons (gain in negative charge)
Cations: Positively charged ions, attracted to the negative
electrode, cathode.
Anions: Negatively charged ions, attracted to the
positive electrode, anode.
