Incoming and Outgoing Shipments in 1 STEP Using Odoo 17
olumide adeola pidan
1.
2. Homeostasis
The Interstitial Fluid is the environment of the cells, and life
depends on the constancy of this internal sea.
Homeostatic Mechanisms : Maintain within a narrow range.
Tonicity
Volume
Specific ion concentration
Defence of Tonicity –(280-295mOsm/L)
Vasopressin secretion
Increased Osmolality of ECF
Thirst Mechanism
Thirst Increased
Vasopressin Secretion
Increased
Water Intake Water Retention
Dilution of ECF
Inhibitor
y
3. Homeostasis
Defence of Volume:
ECF Na+ - Most important
Renin-Angiotensin-
Aldosterone System
Vasopressin Secretion:
Volume stimuli override
osmotic regulation
ANP & BNP
Angiotensinogen
Renin
Angiotensin I
ACE
Angiotensin II
Adrenal
Cortex
Brain
Thirst
Aldosterone Vasopressin
Kidney
Na Retention
Water
Retention
Blood Vessel
Vasoconstriction
4. Homeostasis
Defence of Specific Ionic Concentration:
Glucose
Na+ & K+
Ca++ - Mainly by Parathyroid & Calcitonin
Mg++ - Incompletely understood mechanisms
Also dependent on H+ ion
pH is maintained within a narrow range.
5. Acid Base Equilibrium
What is Acid Base Equilibrium About?
Buffers
? Fixed
Cation?
Base Excess/
Deficit? Anion
Gap?
6. Acid Base Equilibrium
Acid Base Equilibrium is all about
Maintenance of H+ ion concentration of
the ECF.
Source of H+ ion in Body:
CO2 from
metabolism
H+ load from
AA
metabolism
Strenuous Exercise Lactic
Acid
Diabetic
KA
Ingestion of
NH4Cl, CaCl2
Failure of Kidneys to
Excrete PO4--, SO4--
12500 mEq/d
50 - 100 mEq/d
7. Some Basic Chemistry
Definitions:
Arrhenius:
Acid: H+ Donor in Solution
Base: OH- donor in Solution
Browsted and Lowry:
Acid: Proton Donor
Base: Proton Acceptor
H20 can be both
8. Some Basic Chemistry
Simple Rule of Thumb:
Acid Higher conc. Of H+ ion
Base Lower conc. Of H+ ion
Strong Acid/Base Dissociates completely and irreversibly
Weak Acid/Base Dissociates partially and reversibly
Strong Electrolyte: Dissociates completely in solution at
physiological pH
Eg: NaCl, KCl
Weak Electrolyte: Dissociates incompletely in solution at
physiological pH
Eg: CO2 – HCO3
- System, Proteins
9. Some Basic Chemistry
pH (Puissant of Hydrogen):
Negative logarithm of H+ ion concentration to the base of 10
Why pH?
Normal H+ ion conc: 0.00004meq/L or 40nEq/L or 4x10-9
mol/L
pH converts to decimal numbers & takes away negative
sign.
Normal pH: 7.35-7.45
Normal H+ Conc: 0.00002mEq/L – 0.0001 mEq/L
10. Some Basic Chemistry
Pitfalls: Non-linear Negative Logarithmic scale
pH Decreases as [H+] increases.
Each unit change in pH from 7 represents 10 fold change in
H+ ion conc.
Eg: At pH 4, there are 10 times as much H+ than at pH 5, & 100 times
as at pH 6
Same numeric change in different portions of the pH scale
implies vastly different nanomolar change in H+ ions
Eg: pH 56 => 100 times greater change in ionic conc than when pH
7 8
Body H+ ion conc is not as tightly controlled as the other ion,
though the pH scale implies so.