This document discusses electrolytes, including their definition, functions, normal ranges, and imbalances. The four main electrolytes covered are sodium, potassium, chloride, and bicarbonate. Sodium is important for nerve impulses, fluid balance, and acid-base regulation. Potassium influences neuron function, osmotic balance, and muscle contraction. Chloride impacts fluid balance and acid-base regulation. Bicarbonate maintains acid-base homeostasis. Imbalances like hyponatremia, hypokalemia, hypernatremia, and hyperkalemia are explained along with their causes and effects. Methods for electrolyte detection include flame photometry and ion-selective electrodes.

2. AHMED USMAN
TRAINEE TECHNOLOGIST
AGA UNIVERSITY HOSPITAL

3. Definition
 Electrolyte are grouped which are charged ions.
The important physiologically active electrolyte are
 Sodium
 Potassium
 Chloride
 Bicarbonate.

4. Physiology of electrolytes

5. Sodium Functions
• Transmission and conduction of nerve impulses
• Responsible for osmolality of vascular fluids
• Regulation of body fluid levels
• Sodium shifts into cells and potassium shifts out
of the cells (sodium pump)
• Assists with regulation of acid-base balance by
combining with Cl or HCO3 to regulate the
balance

6. Chloride Functions
• Found in ECF
• Changes the serum osmolality
• Goes with Na in retention of water
• Assists with regulation of acid-base balance
• Cl combines with hydrogen to form hydrochloric
acid in the stomach

7. Potassium function
 Potassium cation are important in neuron function.
 Potassium influencing osmotic balance between cells
and the interstitial fluid, with their distribution by the
so-called Na+/K+-ATPase pump.
 K+: essential for normal membrane excitability for
nerve impulse Contraction of muscle
 Promotes enzyme action
 Assist in the maintenance of acid-base

8. Bicarbonate function
 Bicarbonate is alkaline and a vital component of the
pH buffering system of the human body (maintaining
acid-bace homeostasis).

9. Normal ranges
Potassium 3.5-5.1mmol/L
Chloride 101-112mmol/L
Sodium 136-145mmol/L
Bicarbonate 22-32mmol/L

10. Rules of Electrolyte Balance
1. Most common problems with electrolyte balance are
caused by imbalance between gains and losses of
sodium ions
2. Problems with potassium balance are less common,
but more dangerous than sodium imbalance

11. • Hyponatremia
Excessive sodium loss or H2O gain
• CAUSES
– Prolonged diuretic therapy
– Insufficient Na intake
– vomiting
– Administration of hypotonic fluids
– Compulsive water drinking
– alcoholism

12. Hypokalemia
• Causes
– Prolonged diuretic therapy
– Inadequate intake
– vomiting
– Excess insulin
– Excess stress
– Hepatic disease
– Acute alcoholism

13. Hypernatremia
• Occurs with excess loss of H2O or excessive
retention of Na
• Can lead to death if not treated
• Causes
– Vomiting/diarrhea
– Inadequate ADH
– Some drugs
– Hypertonic fluids/tube feedings
– Major burns

14. Hyperkalemia
• Results form impaired renal function
• Metabolic acidosis
• Acts as myocardial depressant; decreased heart
rate, cardiac output
• Muscle weakness
• GI hyperactivity

15. Method of detection
 Photoelectric flame photometer
 In principle, it is a controlled flame test with the
intensity of the flame quantified by photoelectrically.
The sample is introduced to the flame at a constant
rate. Filters select which colours the photometer
detects and exclude the influence of other ions.

16. Ion selective electrode
 The sample is mixed with ISE providing constant
pH.As the buffered sample is moved through the ion
selective electrode , changes in the electrical potential
take place .The electrical potential changes are
measured against the potential of a refrence electrode.