ABSTRACT
Tris buffer
solution was prepared in the laboratory by dissolving 4.6g of boric acid, 6.5g
of EDTA and 60.5g of trisma base in 1000cm3 of distilled water.
Comparative study were done on the commercially produced tris buffer solution,
using and laboratory produced tris buffer solution, using pH meter
for the p H and by carrying out genotype test for the efficacy of
Tris buffer solution prepared in the laboratory was used as an electrolyte.
This genotype test reduces the occurrence of sickle cell anemia. This expresses
the efficacy rate and pH of laboratory produced Tris buffer solution
as compared with that of commercially produced tris buffer solution. The result
obtained for the pH of laboratory produced tris buffer solution was
found to be 9.0 while that of commercially produced tris buffer solution was
found to be 8.9. the result obtained for the efficacy using genotype test
showed that tris buffer solution produced in laboratory has more efficacy than
that produced commercially, but the difference is not significant.
TABLE OF CONTENT
Certification i
Dedication
ii
Acknowledgment iii
Abstract
iv
Table of
contents v
CHAPTER ONE
1.0 Introduction
1.1 Constituent of a buffer
1.2 Statement of problem
1.3 Objective of the research
1.4 Hypothesis
CHAPTER TWO
2.0 Literature review
2.1 Definition
2.2 Other types of buffer solutions
2.3 Importance and uses of buffers
2.4 Location of buffer in the body
2.5 Mechanism of action
2.6 What type of buffer is tris buffer solution
2.7 What is sickle cell anaemia
2.8 Physiological importance
2.9 Diagnostic use of buffer solution
2.10 Diagnostic significance
2.11 Storage/ shelf life
CHAPTER THREE
3.O Materials and methodology
3.1 Reagents
3.2 Apparatus/materials
3.3 Method of preparation
3.4 Comparative study
CHAPTER FOUR
4.0 RESULTS AND DISCUSSION
CHAPTER FIVE
5.0 CONCLUSIONS AND RECOMMENDATION
REFERNCES
CHAPTER
ONE
1.0
INTRODUCTION
Martin et
al (1989) defined buffer as a solution that has the ability to resist change in
pH, when small amounts of strong acids or bases are added to it. For
example, when 0.01 mole of strong acids or base is added to distilled water,
the pH drops to 2 with the acids and rises to 12 with the base. If
the same amount of acid or base is added to an acetic acid-sodium acetate
buffer, the pH may only change a fraction of a unit.
Buffers are
important in many areas of chemistry. When the pH must be controlled
during the course of a reaction, the solutions are often buffered. This is
often the case in biochemistry when enzymes or proteins are being studied. Our
blood is often buffered to a pH of 7.4. Variations of a few tenths
of a pH unit can cause illness or death. Acidosis is the condition
when pH drops too low. Alkalosis is the condition when pH
becomes higher than normal. Acidosis or alkalosis affects the functions of the
heart.
In buffer
solution two species are required one is capable of reaction with OH-
and the other will react with H3O+. The two species must
not react with each other. Many buffers are prepared by combing a weak acid and
its conjugate (acetic acid and sodium acetate) or a weak base and its conjugate
(ammonia and ammonium chloride). In general, the pH range in which a
buffer solution is effective is + or – one pH unit on either side of
the pka.
Buffering
however is the tendency of a solution to resist change in pH
following addition of acid or base, according to Martin et al, 1989.