This document discusses electrolyte replacement therapy and lists three common electrolyte compounds used: sodium chloride, potassium chloride, and calcium gluconate. Sodium chloride and potassium chloride are described in detail, including their molecular formulas, properties, preparation methods, assays, and uses. Calcium gluconate is also described briefly, noting its use as an electrolyte replenisher and to treat conditions caused by low calcium levels such as osteoporosis and rickets. The main purpose of electrolyte replacement therapy is to restore electrolyte and fluid balance in the body.

1. Electrolyte used for
the Replacement
therapy
Nidhi Sharma

2. The main purpose of electrolyte replacement therapy is to overcome the electrolyte
imbalance & to restore the composition of body fluid & body volume.
This electrolyte imbalance seen in different abnormal conditions like Diarrhoea, Vomiting,
Dehydration, Prolonged treatment without adding any source of Nutrients.
There are few electrolytes present in the body which are responsible for different actions
in the body like Sodium, Potassium, Phosphate, Bicarbonates, Sulphate, Calcium, Chloride &
Magnesium.
There are given example of three Compounds which can be used as the major source of
Electrolyte-
• Sodium Chloride
• Potassium Chloride
• Calcium Gluconate

3. Sodium Chloride
• Molecular Formula- NaCl
• Molecular weight- 58.44
• Synonyms- Rock salt, Table salt, Common salt etc.
• Method of Preparation-
• Sodium Chloride can be obtained from natural source as well as it can
also be prepared in laboratory.
• Naturally It can be obtained from Rock salt strata & Sea water. But
from these sources it can be obtained in impure form. The pure form
of salt can be obtained by the filtration process & finally the dried
form can be collected by evaporation process.
• It can also be prepared in laboratory in small scale by the acid- base
reaction. In which strong acid (HCl) reacts with strong base (NaOH) &
finally it gives Sodium Chloride.

4. Properties-
Physical properties-
• It is white, anhydrous crystalline solid.
• Odourless but having salty taste.
• It is soluble in water but insoluble in alcohol.
• Its 0.9% Solution is Isotonic (That means having same Osmotic
pressure) to blood.
Chemical properties-
• 1. It reacts with Silver nitrate and forms white precipitates of
Silvr chloride,
• 2. It can also reacts with sulphuric acid & gives Hydrochloric acid
(Gaseous form).

5. Assay-
• Its assay based on the Argentometric titration (It involve the
determination of chloride ion by action of silver ions).
• Weight 1 gm of sample & dissolve it in 50 ml of water in stoppered
conical flask. Now add 3 ml Nitric acid, 5 ml Nitrobenzene, 3 ml of
0.1 N AgNO3 solution, 2 ml of ferric ammonium sulphate
(Indicator). Now mix it & titrate the solution against 0.1N
Ammonium thiocyanate solution (Titrant).
Uses-
• It is used as electrolyte replenisher.
• Its 0.9% solution is isotonic (having same osmotic pressure) as
blood.
• It is also used as taste enhancer in the preparation of dishes.
• It is also used in Wet dressings & irrigation of body cavities.

6. Potassium Chloride
• Molecular formula- KCl
• Molecular weight- 74.55
• Synonyms- potassium muriate, potash muriate.
• Preparation- It can be commonly obtained by mining its
minerals, followed by extraction.
• It is also extracted from brine (salt water).
• It can also be prepared in the laboratory in small scales by
reacting potassium hydroxide (KOH) with hydrochloric acid
(HCl).
KOH + HCl → KCl + H2O

7. Properties-
Physical properties-
It is white crystalline powder, odourless & strong saline taste.
Like Sodium Chloride it is freely soluble in Water, & insoluble
in alcohols.
Chemical properties-
Another important reaction of KCl is used to produce metallic
potassium, by reducing KCl with metallic sodium at 850 °C.
KCl + Na → NaCl + K
Uses-
• It is used as electrolytes replenisher.
• pH buffers
• Preparation of fertilizers, explosives, potassium metal and
potassium hydroxide.

8. • It is also used in Medicine & Food processing.
• As a substitute for table salt (sodium chloride).
• Like Sodium chloride, it is used in various purposes including-
• de-icing,
• roads
• homes,
• In petroleum and natural gas industry
• In water softening.

9. Calcium gluconate
• Molecular formula- C12H22CaO14
• Molecular weight- 430.37
• Synonyms- Calcium D-gluconate
Calcarea gluconica
Calcii gluconas
Calcium di-gluconate
Calcium gluconate anhydrous
Calcium gluconate, anhydrous
D-gluconic acid, calcium salt

10. Preparation-

11. Properties-
Physical properties-
• It is available in While crystalline granuler or crystalline.
• Odourless & Tasteless.
• It is soluble in Water & Insoluble in Organic solvents and
alcohols.

12. Assay-
Weigh accurately about 0.5 g of the dried sample and dissolve in 5 ml of
dilute hydrochloric acid. Add 50 ml of water, 25 ml of sodium hydroxide
TS and about 0.1 g of 2-hydroxy-1-(2'-hydroxy-4'-sulfo-1'-naphthylazo)-3-
naphthoic acid.
Titrate with 0.05 M EDTA immediately. At the end-point, the red colour
changes completely to blue. Each ml of 0.05 M EDTA is equivalent to 22.42
mg of C12H22CaO14 · H2O.

13. Uses-
1. Used as Electrolyte replenisher. Added to that patient diet which have the
hypoglycaemic condition.
2. It is also used to treat conditions caused by low calcium levels such
as-
Bone loss (osteoporosis),
Weak bones (osteomalacia/rickets),
Decreased activity of the parathyroid gland
(hypoparathyroidism),
A certain muscle disease (latent tetany).
3. Calcium plays a very important role in the body.

14. 4. Necessary for normal functioning of nerves, cells,
muscle, and bone.
5. If there is not enough calcium in the blood, then
the body will take calcium from bones, thereby
weakening bones. Having the right amount of calcium
is important for building and keeping strong bones.