Acid and base balance - Renal 4 Flashcards
Learning outcomes
* Acid-base disturbance
* H+ handling secretion
* Bicarbonate buffering
* Acidosis and alkalosis – metabolic and respiratory
Arterial pH if it is?
Less than 6.8 / greater than 8 this is not compatible with life and death occurs
Optimal pH in the body?
7.4 is equivalent to 40nMols/L [H+]
Arterial and venous pH differ
What pH is acidosis?
Exists when blood pH falls below 7.35
What is Alkalosis?
Occurs when blood pH is above 7.45
Why is maintaining pH in the body so important? 3
- pH changes cause conformational changes in
proteins and can alter functions
e.g. enzyme activity is pH dependent - Nervous system function is v sensitive to pH changes, can lead to seizures, coma
- Cardiac arrhythmia: change in H+ ions can have domino effect on other ions and cause detrimental effects
While reabsorbing Na+ from the filtrate, renal tubular cells secrete?
Predominantly?
Changes in K+ leads to?
Either H+ or K+
Predominantly K+ but H+ secretion increases to
compensate for acidosis.
Changes in [K+] ECF can lead to cardiac abnormalities
SEE SLIDE 5
Antiport via same carrier proteins or other carrier proteins
Movement of K,H+Na ions is interlinked across membrane
Thus if pH changes this will have knock on effects -> Disturbingly wise
Sources of H+ gain? 4
- CO2 in blood (combine with H2O via carbonic anhydrase)
- Non-volatile acids from metabolism (e.g. lactic)
- Loss of HCO3 - in diarrhoea or nongastric GI fluids
- Loss of HCO3 - in urine
Sources of H+ loss? 3
- Loss of H+ in vomit
- Loss of H+ in urine
- Hyperventilation (blow off CO2)
What is an acid - Brønsted-Lowry definition?
An acid is a substance that donates protons
and a base is a substance that accepts
protons
A strong acid is?
An acid which is completely ionised in an aqueous solution
Completely dissociates from rest when in water
A weak acid is?
Is an acid that ionises only slightly in an aqueous solution
Not complete dissociation in every instance when acid is in water
What are buffers?
Buffers are balanced mixtures of a weak
acid and its conjugate base: substance that is formed when weak acid gives up its proton
Chemical buffer systems minimise changes in pH how?
By binding or yielding free H+
First line of defence
H2CO3: HCO3 buffer system major function?
Primarily ECF buffer against non-carbonic acid changes
Protein buffer system major functions?
Primary ICF buffer but also buffers ECF
Haemoglobin buffer system major function?
Primary buffer against carbonic acid changes
Phosphate buffer system major functions?
Important urinary buffer, also buffers ICF
Intracellular pH regulation occurs via what system?
See slide 9
Phosphate buffer system
Phosphate buffer system - in a test tube:
Add a strong acid to a mixture of these two substances (for example HCl): H+ is accepted by HPO4 2- producing H2PO4–
What is the result?
The strong acid is replaced by a weak acid, ‘buffering’ the decrease in pH.
Phosphate buffer system - in a test tube:
Add a strong base to a mixture of these two substances (for example NaOH) : H2PO4– donates a proton to OH– to form HPO4 2- + H2O.
What is the result?
The strong base is replaced by a weak base, ‘buffering’ the increase in pH.
ICF pH regulation: Phosphate buffer system
1. In acid solution what happens?
2. In basic solution what happens?
- In acidic solution: (HPO4)^2- accepts H^+ and caused an increase in pH.
- In basic solution: H2PO4 donates H+ and causes a decrease in pH.
Phosphate buffer system is important for buffering what?
What is this system made up of?
Within cells
Monohydrogen phosphate ions: (HPO4)^2-
Dihydrogen phosphate ions H2PO4-