2. What are electrolytes?
• Electrolytes are minerals that are present in our blood & body tissue
• Electrolytes are important for
1. Maintaining fluid and pH balance
2. Nerve and muscle functioning
3. SODIUM
• Major cation of ECF
• RDA <2gm/day
• Normal range : 135-145 mmol/L
• Na levels are regulated by the kidneys
• Maintain the normal distribution of water and the osmotic pressure in ECF
• Maintain membrane potential of cells
6. HYPONATREMIA
Volume Status
Hypovolemia Euvolemia Hypervolemia
TBW ↓
Total body sodium↓↓
UNa > 20
Renal losses
UNa < 10
Extra renal losses
Vomiting
Diarrhea
trauma
TBW ↑
Total body Sodium ↔
UNa>20
Polydipsia
TBW ↑↑
Total body sodium ↑
UNa < 10 UNa > 20
Renal
failure
Cirrhosis
CCF
7. HYPERNATREMIA >145 mmol/L HYPONATREMIA <135 mmol/L
Dehydration Vomiting
Elderly with poor water intake Diarrhea
Excessive salt intake Excess non-electrolyte iv infusion
Hyperglycemia and Ketoacidosis
8. POTASSIUM
• Major cation of ICF
• High cellular concentration maintained by Active transport mechanism via
Na+/K+ ATPase pump
• RDA : 3.5 g/day
• Normal range : 3.5-5 mmol/L
• Major determinant of cell volume and osmolality of Intracellular compartment
11. HYPERKALEMIA >5.5 mmol/L HYPOKALEMIA <3mmol/L
Renal failure Diarrhea, Vomiting
Burns Hyperaldosteronism
Increased haemolysis Thyrotoxic periodic paralysis (ab N Na-K-
ATPase)
Tumor lysis syndrome Alkalosis
Insulin deficiency (DM) Malabsorption
Drug induced: ACE inhibitors Drug Induced: Bronchodialators
Rhabdomyolysis, Crush injury
12. Estimation of Na+ & K+
1. Ion selective electrodes
2. Atomic absorption spectroscopy
3. Flame emmision photometry
13. ION SELECTIVE METHOD
• Ion selective membrane:
1. Na+ : Glass
2. K+ : PVC impregnated with Valinomycin
• I.S.E. consists of a thin membrane across which only the intended ion
can be transported.
• The transport of ions from a high concentration to a low one through
selective binding with some sites within the membrane creates a
potential difference
14. • An ISE with its own internal
reference electrode is immersed in
an aqueous solution containing the
ions to be measured, together with
a separate, external reference
electrode.
• The electrochemical circuit is
completed by connecting the
electrodes to a sensitive milli-volt
meter.
• A potential difference is developed
across the ISE membrane when the
target ions diffuse through from
the high concentration side to the
lower concentration.
15. ISE : Principle
• The electrode produces a difference in potential between itself and a
reference electrode.
• This difference in potential is proportional to the concentration of the
selected ion in solution and is described by the Nernst equation
• The ISE system is calibrated with solution containing known
concentration of analytes
• the concentration of an unknown solution is derived by comparing its
potential with that of a solution of known concentration.
16. E = Eo – 2.3 (RT/nF) log (C + Co)
• E = measured potential (mV) between the ion-selective and the reference
electrode
• Eo = measured potential (mV) at the lower concentration standard
• R = universal gas constant (R = 8.314 J mol–1 K–1)
• T = temperature in K (Kelvin), with T (K) = 273.15 + t °C where t is the
temperature of the measured solution in °C
• F = Faraday constant (96485 C·mol–1)
• n = valency of the ion
• C = concentration of ion to be measured
• Co= detection limit
17. COMPONENTS OF ELECTROLYTE ANALYZER
• Reagents Calibrator, Slope standards and the wash solution.
• Electrode Module houses the air/fluid detector,
measuring electrodes and reference electrode
• Peristaltic Pump pushes the reagent fluids and patient sample
through the tubing to the sample probe and electrode module out to
the waste bottle.
• Sample Probe aspirates fluids into the analyzer via the peristaltic
pump. The probe automatically accepts samples from a test tube
• Waste Chamber