Using english to give evidance
Some chemical changes are easy to observe. The
products formed by the rearrangement of atoms look different than the
reactants. Other changes are not easy to see but can be detected in other ways.
Color Change
Substances often change color during a chemical reaction.
For example, when gray iron rusts, the product that forms is brown, as shown in
the photograph below.
Formation of a Precipitate
Many chemical reactions form products that exist in
a different physical state from the reactants. A solid product called a may
form when chemicals in two liquids react, as shown in the photograph below.
Seashells are often formed this way when a sea creature releases a liquid that
reacts with seawater.
Formation of a Gas
Chemical reactions may produce a gas, like that formed
when antacid pills are mixed with stomach acid. The photo-graph below shows an
example in which carbon dioxide gas is produced by a chemical reaction.
Temperature Change
Most chemical reactions involve a temperature change.
Sometimes you can recognize the change when you see a flame. Notice the burning
of the metal magnesium in the photograph. Other temperature changes are not
immediately obvious. If you touch concrete before it hardens, you may notice
that it feels warm. This warmth is due to a chemical reaction.
Buffer Solution In The Human Body
The
buffer solution is the solution used to maintain a certain pH value so as not
to change much during the chemical reaction. The chemical reaction occurring in
the human body is an enzymatic reaction, a reaction involving the enzyme as a
catalyst. Enzyme activity as a catalyst in the living system is very sensitive
to changes in pH. Enzyme as catalyst can only work well at certain pH (optimum
pH). To keep the enzyme working optimally, a reaction environment with a
relatively fixed pH is required, therefore a buffer solution is required. The
continuous metabolic process will produce acidic substances, such as lactic
acid, phosphoric acid, and sulfuric acid liberated in body tissues. Absorption
of nutrients can also produce acidic or basic substances. These can all affect
blood pH. Therefore in every body fluid there is a conjugate acid-base pair
which acts as a buffer solution. Body fluids, both as intra-cell fluids (in
cells) and extra cell fluid (outside the cell) require the buffer system to
maintain the pH value of the liquid.
Under
normal circumstances, the pH of body fluids including our blood is in the range
of 7.35-7.45. If the pH-regulating mechanism in the body fails, as can occur
during illness, so that the blood pH falls below 7.0 or rises above 7.8, may
cause permanent damage to the body's organs or even death. The most important
organ to maintain blood pH is the lungs and kidneys. The condition in which the
blood pH is less than 7.35 is called acidosis (decrease in blood pH). Factors
that affect the occurrence of acidosis conditions include heart disease, kidney
disease, diabetes, and persistent diarrhea or high-protein foods in the long
term. The condition of temporary acidosis can occur due to intensive exercise
that is done for too long. Whereas a blood pH of more than 7.45 is called
alkolosis (an increase in blood pH). This condition is caused by severe
vomiting, hyperventilation (the condition when breathing too fast because of
anxiety or hysterics at altitude). A study of mountain climbers who reached the
summit of Everest (8,848 m) without additional oxygen showed their blood pH was
between 7.7-7.8. Hyperventilation is required to deal with very low oxygen
pressures (approximately 43 mmHg) in such high places.
Although
large amounts of H + ions are always present as a result of metabolism of
substances, but a balanced state must always be maintained by removing excess
acid. This is due to a slight decrease in pH indicating a state of illness.
Function of Buffer Solution on Human body:
1. Buffer solution in the blood
Blood
has a relatively constant pH of about 7.4. This is possible because of a
buffering solution in the blood, ie H2CO3 / HCO3-, so that even whenever the
blood of the various acidic or basic substances is infected, the effect on pH
changes can be neutralized. If the blood of the acidic substance is present,
then the H + ion of the acid will react with the HCO3- ion:
H + (aq) + HCO3- (aq) H2CO3 (aq)
Conversely, if the blood is a basic substance, the
OH ion reacts with H2CO3:
OH- (aq) + H2CO3 (aq) HCO3- (aq) + H2O (l)
Comparison of H2CO3 concentrations: HCO3 - in the
blood about 20: 1. This occurs because of the equilibrium between the dissolved
CO2 gas in the blood with H2CO3, as well as the solubility equilibrium of CO2
gas from the lungs with dissolved CO2.
CO2 (g) + H2O (l) H2CO3 (aq)
So
if in the blood dissolved H2CO3, the blood will immediately release CO2 gas
into the lungs. If your metabolism increases (eg due to exercise or fear). So
in the process of metabolism is produced a lot of acidic substances into the
bloodstream that will react with HCO3 - in the blood that produces H2CO3 in the
blood. High levels of H2CO3 will result in a decrease in the pH value. To keep
pH reduction not too large, H2CO3 will soon break down into CO2 and H2O gases.
The result is that breathing progresses more quickly so that blood can get CO2
into the lungs quickly. The opposite will happen if in certain conditions the
blood contains a lot of alkaline (OH- ions). The presence of a base will be
bound by H2CO3 which will subsequently be transformed into HCO3 ions. Thus, it
takes CO2 gas from the lungs that must be inserted into the blood to replace
the H2CO3. This results in breathing also progresses more quickly.
Blood
has a pH range of 7.0 - 7.8. Beyond that value will be fatal to the body. A
disease in which the pH of the blood is too low is called acidosis, whereas if
the blood pH is too high it is called alkalosis.
b. Buffer of Hemoglobin
Oxygen
is the main substance needed by the body cells obtained by breathing. In the
blood, there is a hemoglobin that can bind oxygen to subsequently carried to
all body cells. The equilibrium reaction of the oxyhex hemoglobin buffer
solution is:
HHb + O2 (g) ⇄ HbO2- + H +
The
waste product from the body is CO2-which in the body can form H2CO3 compounds
that will break down into H + and HCO3-. Addition of H + in the body will
affect the pH, but the hemoglobin that releases O2 can bind H + and form
hemoglobin acid (HHb +). Thus the H + ion released in decomposition of H2CO3 is
an acid produced by CO2 dissolved in water during metabolism.
C. Phosphate Buffer
The
phosphate buffer is a buffer within the cell (intracellular fluid). Phosphate
buffers are used to maintain blood pH. The phosphate buffer can maintain a
blood pH of 7.4. This buffer is a mixture of weak acid H2PO4- and its conjugate
base, HPO42-. If the process of cell metabolism produced many acidic
substances, it will soon react with the ion HPO42-
HPO42- (aq) + H + (aq) ⇄
H2PO4- (aq)
And
if the cell metabolism process produces an alkaline compound, then the OH-ion
will react with H2PO4-.
H2PO4- (aq) + OH- (aq) ⇄
HPO42- (aq) + H2O (aq)
So
the ratio [H2PO4-] / [HPO42-] is always fixed and consequently the pH of the
solution remains. This buffer is also outside the cell, but the number is
small. In addition, the phosphate buffer also acts as a buffer of urine.
Ø Maintain
pH in blood plasma to be at pH ranging from 7.35 to 7.45
Namely
from HCO3 ions with Na + ion. If a blood pH of more than 7.45 will develop
alkalosis, the result is hyperventilation / excessive breathing. If the blood
pH is less than 7.35 will experience acidosis consequently heart, kidney, liver
and digestion will be disrupted.
Ø Maintaining
the pH of body fluids for the excretion of H + ions in the kidneys is not
disturbed
Namely
dihydrogenposphat acid (H2PO4-) with a monohydrogenposphat base (HPO42-)
Ø Spit
water as a buffer solution
The
H2PO4- / HPO42 buffer solution is also found in saliva, which serves to keep
the pH of the mouth about 6.8 by neutralizing the acid resulting from the
fermentation of food debris that can damage the teeth.
Function
of buffer solution in everyday life.
Buffer solutions are used in various
fields, such as analytical chemistry, biochemistry, bacteriology,
pharmaceuticals, photography, leather industry, dyestuffs, food industry,
agriculture, and industrial waste processing. A narrow range of specific pH is
required to achieve optimum results in these areas. Eg an enzyme can work at a
certain pH and is very sensitive to changes in pH.
In the field of food industry, for
example fruit canning industry also need buffer solution. The buffer solution
serves as a regulator of the acidity level (pH).
Eg citric acid and sodium citrate.
Both of these substances are the usual buffer solutions added to the canned
fruits. In addition, citric acid is also commonly used to regulate the level of
acidity in milk products, jams, and jellies. If the pH is maintained then the
food product is not easily damaged by bacteria. Meanwhile, buffering is also
needed to regulate pH in industrial waste treatment. Prior to processing, the
pH of the waste is regulated in such a way that when disposed of the waste does
not cause a negative impact on the environment.
Source
http://www.pelajaransekolahonline.com/2016/06/fungsi-larutan-penyangga-dalam-tubuh.html
Can you mention the buffer solution other than the one you mentioned above?
BalasHapusThe buffer solution contains a mixture of weak acids and their conjugate base or weak base and conjugate acid.
HapusThe buffer solution can be distinguished from the acid buffer solution and the alkaline buffer solution. The acid buffer solution maintains the pH in the acid region (pH <7), while the alkaline buffer solution maintains the pH at the base region (pH> 7).
A. Acid buffer solution
The acid buffer solution contains a weak acid (HA) and its conjugate base (A-). Solutions such as these can be made in various ways such as:
1) Mix weak acid (HA) with the salt (LA, LA salt produces ion A- which is the conjugate base of HA acid)
Some examples :
- CH3COOH + NaCH3COO (buffer components: CH3COOH and CH3COO-)
- H2CO3 + NaHCO3 (buffer components H2CO3 and HCO3-)
- NaH2PO4 + Na2HPO4 (buffer components H2PO4- and HPO4 2-)
2) Mixing a weak acid with a strong base where the weak acid is mixed in excess amount. The mixture will produce a salt containing the conjugate base of the corresponding weak acid.
B. Base buffer solution
The base buffer structure contains a weak base (B) and its conjugate acid (H +). The basic buffer solution may be prepared in a manner similar to that of the buffer solution. acid.
1). Mixing a weak base with the salt.
Example:
NH3 + NH4Cl solution (buffer component: NH3 and NH4 +)
2) Mixing a weak base with a strong acid in which the weak base is excessively mixed.
Give me an example of a buffer reaction that is beneficial to the human body
BalasHapusThe chemical reactions occurring within the human body are enzymatic reactions, ie reasks involving enzymes as catalysts. Enzyme as catalyst can only work well at certain pH (optimum pH). In order for enzymes to remain optimum, a reaction environment with a relatively fixed pH is required, therefore a buffer solution is required.
HapusIn each body fluid there is a conjugate acid-base pair that acts as a buffer solution. Body fluids, both as intra-cell fluids (in cells) and extra cell fluid (outside the cell) require the buffer system to maintain the pH value of the liquid. An important extra-cell support system is a carbonate (H2CO3 / HCO3-) buffer that plays a role in maintaining blood pH, and a phosphate buffer system (H2PO4- / HPO42-) which plays a role in maintaining the pH of the intra-cell fluid.
What happen if pH in human body more than normal pH standard have to be?
BalasHapusIf the ph is below 7 then it means the body is too acidic. This is very dangerous because the body can not tolerate acid imbalance for a long time. If the pH is too low it means the buildup of carbon dioxide in the blood. High carbon dioxide will make breathing difficult.
HapusThe acidic body condition causes fatigue, pain, blistering, headache, drowsiness, allergies, colds and flu, sinus problems. Oxygen levels decrease due to carbon dioxide buildup in the blood. If oxygen goes down the cells of the body will die.
People who have too acidic body more easily exposed to bacteria or viruses. Just so you know, cancer cells more easily develop if the body in excessive acid conditions.
Acid blood will block the absorption of vitamins, make toxins clogged in cells, slow down the function of organs, disrupt the good digestive system, release a lot of gas and flatulence, causing unhealthy weight gain and accelerate the aging process. A more moderate diet can help restore the pH balance. For starters, try eating more fresh fruits and vegetables, almonds and yogurt. Begin reducing cheese, soft drinks, alcohol, processed foods, sweeteners and use honey instead. Approximately 75 percent of a good diet should consist of foods that produce bases.
If dietary changes are too difficult to consider using an alkaline supplement. A study has been done that an alkaline supplement can increase the acidic pH to normal. But scientists are more advised to reduce the acidity of the body with healthy foods.
To lower the stress level so that the pH back to normal limits can also try to do breathing exercises and eat alkaline foods. Walking 10 minutes a day can also reduce stress and restore balance.