Biochemistry Lecture
BIOCHEMISTRY OF BLOOD AND HOMEOSTASIS xi. Selenium
(1) Homeostasis xii. Copper
a. Organs Involved in Homeostasis xiii. Manganese
(2) Regulatory Processes in the Body xiv. Chromium
a. Oxygen Regulation in the Blood xv. Molybdenum
i. Hemoglobin
HOMEOSTASIS
(3) Factors that Affect Oxygen Binding
→ Series of automatic control systems
(4) Types of Iron Porphyrin
→ State of steady internal physical and chemical
(5) Acid – Base Balance
conditions maintained by living systems.
a. Types of Acids
b. Release of Acids ORGANS INVOLVED IN HOMEOSTASIS
(6) Clinical Ph Range Brain → Dictate what chemicals must be used to
(7) Plasma Bicarbonate Concentration monitor homeostasis.
a. Bicarbonate Concentration → Hypothalamus – regulates temperature
b. Bicarbonate Buffer System and osmotic pressure.
(8) Normal Values Lungs → Circulatory and Respiratory systems
(9) Disorders → Process of gas exchange helps maintain
a. Buffering acid-base balance and pH level.
b. Effects of Buffers on pH → Utilized by hemoglobin.
(10) Compensatory Mechanisms
Pancreas → Hormones produced by pancreas:
a. Golden Rules: Simple Acid – Base
insulin (trigger liver to store glycogen) and
Disorders
glucagon (trigger gluconeogenesis –
(11) Metabolic Acidosis
produce glucose from glycogen when blood
a. Causes of Metabolic Acidosis
sugar level is low).
(12) Metabolic Alkalosis
→ Regulates blood sugar.
a. Causes of Metabolic Alkalosis
Kidneys → Filter waste materials from blood
(13) Respiratory Acidosis
(excreted via urine).
(14) Respiratory Alkalosis
→ Regulates water balance.
(15) Respiratory Disorders
Muscles → Contracts and release heat.
a. Expected pH Changes for Respiratory
Skin → Evaporation of water helps regulate
Disorders
body temperature (thermoregulation).
(16) Renal Acid Excretion
(17) Titratable Acidity REGULATORY PROCESSES IN THE BODY
(18) Ammonium Excretion → Oxygen Regulation
(19) Sodium and Chloride Relationship → Thermoregulation
(20) Mixed Acid – Base Disorders → Acid-Base Balance
(21) Mineral Balance → Mineral Balance
(22) Fluid and Electrolyte Balance
a. Regulation of Fluid and Electrolyte OXYGEN REGULATION IN BLOOD
Balance → Heme – derivative of the porphyrin; most common
b. Regulation of Blood Pressure porphyrin in humans. Is the major component of
c. Electrolytes hemoglobin.
i. Sodium - Porphyrin – cyclic compounds formed by fusion
- Regulation of Fluid and of 4 pyrrole rings linked by methenyl bridges.
Electrolyte Balance Basic component is iron (ferrous).
ii. Chloride o Ferrous – 2
iii. Potassium o Ferric – 3
iv. Calcium - Proteins coming from the Heme family:
- Blood Calcium Regulation hemoglobin, myoglobin (muscles), cytochromes
- Effects of Chronically Low (Electron TC and energy production), catalase,
Calcium Intake peroxidase.
- Factors that Enhance Calcium HEMOGLOBIN
Absorption → Iron porphyrin linked with globulin.
v. Phosphorus → A tetramer – 4-protein component; quaternary
vi. Magnesium structure of protein
vii. Sulfur → Reversibly combine with oxygen and transports oxygen.
viii. Iron
ix. Zinc
x. Iodine
SECG 1
, Biochemistry Lecture
→ There is no blue blood because when it is exposed to ACID – BASE BALANCE
air, it will immediately take up oxygen – which makes the → Balance between input (intake and production) and
blood color red. output (elimination) of hydrogen ion.
→ The lower the oxygen, the lower the hemoglobin ACID
affinity is = lower carbon dioxide present. The higher the - Substance that can donate hydrogen ions.
pH (basic) = lower temperature. - Has lower pH.
→ Higher carbon dioxide present = lower pH (due to the - Below 7 = acidic
formation of carbonic acid) = higher temperature (due to BASE
the increase of acidity) - Substance that can accept hydrogen ions.
→ Basicity in the blood – bicarbonate (HCO3) - Has higher pH.
→ Acidity in the blood – carbon dioxide/carbonic acid - Neutral pH is 7.4.
FACTORS THAT AFFECT OXYGEN BINDING TYPES OF ACIDS
→ Oxygen-carrying capacity of hemoglobin – determines Carbonic Acid → volatile acid – readily change its
how much oxygen is carried in the blood. composition
→ Carbon dioxide levels, blood pH, and body temperature → Can be eliminated by the lungs
affect oxygen-carrying capacity. – When CO2 is in the through respiration. – Body release
blood, it reacts with water to form bicarbonate. carbon dioxide to the air to make it
less acidic.
TYPES OF IRON PORPHYRIN
Non – → non – volatile acid
Myoglobin → Monomer associated with the Carbonic Acid - e.g. phosphoric and sulfuric
muscle (skeletal and cardiac muscle acid (50-100 meq/d)
tissues). → Present in body in very minimal
→ Has higher affinity for oxygen than amount.
hemoglobin but does not → Byproducts of processes in body.
immediately take in oxygen. → Combined with buffers – prevent
→ Storage of oxygen (higher drastic changes in pH.
myoglobin in the system = the longer → Subsequently released by the
one can hold their breath). kidney.
DISEASES RELEASE OF ACIDS
→ Rhabdomyolysis – Damaged (1) Cells utilize carbohydrates, fats, and oxygen.
muscle tissue release myoglobin in (2) Byproduct is energy and carbon dioxide.
high concentrations. Kidneys can filter - Body can produce CO2 13, 000 – 20, 000
myoglobin but it is poisonous to the millimoles/day.
renal tubular epithelium which can - If not released, it could lead to acidosis – blood
cause acute kidney injury. is slightly acidic (6.5 is very acidic to the body)
Cytochromes → Iron porphyrin conjugated to - Kidney – excretes acids that can’t be excreted by
protein. lungs or liver.
→ Important in energy producing o e.g. phosphoric and sulfuric acid
steps in the body. ▪ sulfuric acid – could come
→ Components of respiratory chain in from degradation of protein
mitochondria and transport electron ▪ phosphoric acid –
benefits most the cytochromes. degradation of phospholipids
→ Cyto-P450 – takes part in
CLINICAL pH RANGE
microsomal hydroxylation. Utilized as
→ 7.80 – 6.80 – normal range for body
a genetic marker for different types of
→ 7.4 – normal pH of the body
organisms.
→ Measured by the bicarbonate levels in the body.
→ Involved in redox
reaction/catalysis. – It is a redox- PLASMA BICARBONATE CONCENTRATION
active protein that contain a heme as → Measured by the amount of carbon dioxide present.
a cofactor. - Dissolved carbon dioxide + bicarbonate
→ There are 4 types of cytochromes. concentration (25 – 26 meq/l)
Peroxidase → Iron porphyrin containing enzyme. → As a result, total CO2 concentration exceeds plasma
→ Present mainly in plants (also in bicarbonate concentration by 1.0 – 1.5 meq/l.
bacteria and fungi). - milliequivalent – amount of substance present in
→ Acts on hydrogen peroxide so it the system.
will lessen/remove the damaging → 24 meq/l – normal plasma bicarbonate concentration in
capabilities of hydrogen peroxide. the body.
SECG 2
BIOCHEMISTRY OF BLOOD AND HOMEOSTASIS xi. Selenium
(1) Homeostasis xii. Copper
a. Organs Involved in Homeostasis xiii. Manganese
(2) Regulatory Processes in the Body xiv. Chromium
a. Oxygen Regulation in the Blood xv. Molybdenum
i. Hemoglobin
HOMEOSTASIS
(3) Factors that Affect Oxygen Binding
→ Series of automatic control systems
(4) Types of Iron Porphyrin
→ State of steady internal physical and chemical
(5) Acid – Base Balance
conditions maintained by living systems.
a. Types of Acids
b. Release of Acids ORGANS INVOLVED IN HOMEOSTASIS
(6) Clinical Ph Range Brain → Dictate what chemicals must be used to
(7) Plasma Bicarbonate Concentration monitor homeostasis.
a. Bicarbonate Concentration → Hypothalamus – regulates temperature
b. Bicarbonate Buffer System and osmotic pressure.
(8) Normal Values Lungs → Circulatory and Respiratory systems
(9) Disorders → Process of gas exchange helps maintain
a. Buffering acid-base balance and pH level.
b. Effects of Buffers on pH → Utilized by hemoglobin.
(10) Compensatory Mechanisms
Pancreas → Hormones produced by pancreas:
a. Golden Rules: Simple Acid – Base
insulin (trigger liver to store glycogen) and
Disorders
glucagon (trigger gluconeogenesis –
(11) Metabolic Acidosis
produce glucose from glycogen when blood
a. Causes of Metabolic Acidosis
sugar level is low).
(12) Metabolic Alkalosis
→ Regulates blood sugar.
a. Causes of Metabolic Alkalosis
Kidneys → Filter waste materials from blood
(13) Respiratory Acidosis
(excreted via urine).
(14) Respiratory Alkalosis
→ Regulates water balance.
(15) Respiratory Disorders
Muscles → Contracts and release heat.
a. Expected pH Changes for Respiratory
Skin → Evaporation of water helps regulate
Disorders
body temperature (thermoregulation).
(16) Renal Acid Excretion
(17) Titratable Acidity REGULATORY PROCESSES IN THE BODY
(18) Ammonium Excretion → Oxygen Regulation
(19) Sodium and Chloride Relationship → Thermoregulation
(20) Mixed Acid – Base Disorders → Acid-Base Balance
(21) Mineral Balance → Mineral Balance
(22) Fluid and Electrolyte Balance
a. Regulation of Fluid and Electrolyte OXYGEN REGULATION IN BLOOD
Balance → Heme – derivative of the porphyrin; most common
b. Regulation of Blood Pressure porphyrin in humans. Is the major component of
c. Electrolytes hemoglobin.
i. Sodium - Porphyrin – cyclic compounds formed by fusion
- Regulation of Fluid and of 4 pyrrole rings linked by methenyl bridges.
Electrolyte Balance Basic component is iron (ferrous).
ii. Chloride o Ferrous – 2
iii. Potassium o Ferric – 3
iv. Calcium - Proteins coming from the Heme family:
- Blood Calcium Regulation hemoglobin, myoglobin (muscles), cytochromes
- Effects of Chronically Low (Electron TC and energy production), catalase,
Calcium Intake peroxidase.
- Factors that Enhance Calcium HEMOGLOBIN
Absorption → Iron porphyrin linked with globulin.
v. Phosphorus → A tetramer – 4-protein component; quaternary
vi. Magnesium structure of protein
vii. Sulfur → Reversibly combine with oxygen and transports oxygen.
viii. Iron
ix. Zinc
x. Iodine
SECG 1
, Biochemistry Lecture
→ There is no blue blood because when it is exposed to ACID – BASE BALANCE
air, it will immediately take up oxygen – which makes the → Balance between input (intake and production) and
blood color red. output (elimination) of hydrogen ion.
→ The lower the oxygen, the lower the hemoglobin ACID
affinity is = lower carbon dioxide present. The higher the - Substance that can donate hydrogen ions.
pH (basic) = lower temperature. - Has lower pH.
→ Higher carbon dioxide present = lower pH (due to the - Below 7 = acidic
formation of carbonic acid) = higher temperature (due to BASE
the increase of acidity) - Substance that can accept hydrogen ions.
→ Basicity in the blood – bicarbonate (HCO3) - Has higher pH.
→ Acidity in the blood – carbon dioxide/carbonic acid - Neutral pH is 7.4.
FACTORS THAT AFFECT OXYGEN BINDING TYPES OF ACIDS
→ Oxygen-carrying capacity of hemoglobin – determines Carbonic Acid → volatile acid – readily change its
how much oxygen is carried in the blood. composition
→ Carbon dioxide levels, blood pH, and body temperature → Can be eliminated by the lungs
affect oxygen-carrying capacity. – When CO2 is in the through respiration. – Body release
blood, it reacts with water to form bicarbonate. carbon dioxide to the air to make it
less acidic.
TYPES OF IRON PORPHYRIN
Non – → non – volatile acid
Myoglobin → Monomer associated with the Carbonic Acid - e.g. phosphoric and sulfuric
muscle (skeletal and cardiac muscle acid (50-100 meq/d)
tissues). → Present in body in very minimal
→ Has higher affinity for oxygen than amount.
hemoglobin but does not → Byproducts of processes in body.
immediately take in oxygen. → Combined with buffers – prevent
→ Storage of oxygen (higher drastic changes in pH.
myoglobin in the system = the longer → Subsequently released by the
one can hold their breath). kidney.
DISEASES RELEASE OF ACIDS
→ Rhabdomyolysis – Damaged (1) Cells utilize carbohydrates, fats, and oxygen.
muscle tissue release myoglobin in (2) Byproduct is energy and carbon dioxide.
high concentrations. Kidneys can filter - Body can produce CO2 13, 000 – 20, 000
myoglobin but it is poisonous to the millimoles/day.
renal tubular epithelium which can - If not released, it could lead to acidosis – blood
cause acute kidney injury. is slightly acidic (6.5 is very acidic to the body)
Cytochromes → Iron porphyrin conjugated to - Kidney – excretes acids that can’t be excreted by
protein. lungs or liver.
→ Important in energy producing o e.g. phosphoric and sulfuric acid
steps in the body. ▪ sulfuric acid – could come
→ Components of respiratory chain in from degradation of protein
mitochondria and transport electron ▪ phosphoric acid –
benefits most the cytochromes. degradation of phospholipids
→ Cyto-P450 – takes part in
CLINICAL pH RANGE
microsomal hydroxylation. Utilized as
→ 7.80 – 6.80 – normal range for body
a genetic marker for different types of
→ 7.4 – normal pH of the body
organisms.
→ Measured by the bicarbonate levels in the body.
→ Involved in redox
reaction/catalysis. – It is a redox- PLASMA BICARBONATE CONCENTRATION
active protein that contain a heme as → Measured by the amount of carbon dioxide present.
a cofactor. - Dissolved carbon dioxide + bicarbonate
→ There are 4 types of cytochromes. concentration (25 – 26 meq/l)
Peroxidase → Iron porphyrin containing enzyme. → As a result, total CO2 concentration exceeds plasma
→ Present mainly in plants (also in bicarbonate concentration by 1.0 – 1.5 meq/l.
bacteria and fungi). - milliequivalent – amount of substance present in
→ Acts on hydrogen peroxide so it the system.
will lessen/remove the damaging → 24 meq/l – normal plasma bicarbonate concentration in
capabilities of hydrogen peroxide. the body.
SECG 2
