Buffer solutions. Blood buffer systems and their mechanisms of action. [Group 10] 1st Year 2nd Semester Kursk State Medical university

1. KURSK STATE MEDICAL
UNIVERSITY
 DEPARARTMENT – Chemistry
 TOPIC - 10. Buffer solutions. Blood buffer systems and
their mechanisms of action.
 NAME – Sahil Singh
 GROUP – 10
 1ST YEAR 2nd SEMESTER
 Teacher's Name : Yampolsky Leonid Mikhailovich

2. ⦿Abuffer solution is one which maintains
its pH fairly constant even upon the
addition of small amounts of acid or
base.
⦿There are two types of buffer solution.
1. Acidic Buffer
2. Basic Buffer

3. Acidic Buffer:
A weak acid together with a salt of
the same acid with a strong base.These are
calledAcidic Buffer.
For Example.
CH3COOH CH3COONa.
Basic Buffers:
Aweak base and its salt with a strong
acid.These are called Basic Buffers.

4. For Example.
NH4OH+NH4CL
Let us illustrate buffer action by taking
example of a common buffer system
consisting of solution of acetic acid and
sodium acetate.
CH3COOH ⇌ H+ + CH3COO-
CH3COONa Na+ + CH3COO-
Since the salt is comletely ionized,it
provides the common ion CH3COO in
excess.

5. The Buffer solution has a higher pH than
the acid itself;

6. The pH of Buffer changes only slightly upon
addition of an acid or base;

7. It can be defined as the ability of a
buffer to resist the change of potential of
hydrogen.
Mathematically it can be expressed as;
How it can be determined?
Buffer capacity of a buffer solution is
determined by the size of actual molarities.
How do you calculate the Buffer Capacity?
Buffer Capacity refers to the maximum
amount of a strong acid or a strong base that is
added so that a significant change in pH occur.

8. IMPORTANCE:
It is important in chemical as well as in
biological term.
Buffer Capacity of water:
As the purity of fresh water increases,the buffer
capacity decreases and 100 percent pure fresh water is no
buffer at all.
What factors determined buffer capacity ?
The concentration of the buffer (the higher the
concentration,the larger the buffering capacity) and how
close the pka of buffer is compared to the pH of solution.

9. Blood Buffer System

10. Introduction
The maintenance of the blood pH is important for the
proper functioning of our body and can be critical if
not maintained.
The main buffers in blood are bicarbonate,
haemoglobin, plasma proteins and phosphates.
Mainly, the buffer involves carbonic acid (H2CO3), a
weak acid, and bicarbonate ion (HCO3-), the
conjugate base.

11. Bicarbonate Buffer System
- When an acid enters the bloodstream:
This is to prevent the blood from becoming acidic.
- When a base enters the bloodstream:
This is to prevent the blood from becoming basic.
Due to this, the concentrations of H2CO3 and HCO3-
fluctuate.

12. Other Blood Buffer Systems
⚫Haemoglobin:
⚫Plasma Protein:
⚫Phosphate:

13. Why is This Critical?
If the blood pH goes lower than 6.8 or higher than
7.4, the enzymes and cells would denature and
stop functioning which would cause death.
Cells and enzymes function at a specific
temperature and pH level. Therefore, anything
below or above the specific temperature and pH
level would denature it and the body would stop
functioning causing a lot of diseases and
eventually death!

14. Abnormalities
 Acidosis: an abnormal condition due to excess of
acid in blood that cause the pH to drop below 7.35.
 Alkalosis: an abnormal condition due to excess of
base in blood that cause the pH to rise above 7.45.

15. Causation
Acidosis is caused by:
⚫ Increased acid
production within body.
⚫ Consumption of
substances metabolized
by acid.
⚫ Decreased acid
secretion
⚫ Increased base
secretion
Alkalosis is caused by:
⚫ Disturbances in
electrolyte due to
severe dehydration or
prolonged vomiting.
⚫ Consumption of base
⚫ Hyperventilation with
increased excretion of
acid in the form of CO2.
Also any disease that affects the lungs, kidneys, metabolism
or breathing can cause these two conditions.

16. Treatment
The treatment for Acidosis and Alkalosis is to
identify the cause of the pH imbalance and
providing medications or support according to it.
The treatment to this is mostly never direct. But at
times, health practitioners give intravenous HCO3-
to people who have dangerously low blood pH.