Bicarbonate Buffer Lab Report

Introduction: This experiment is going to test the ability of antacids and how they absorb acid to see which is a better buffer. An antacid neutralizes acid, and this helps the most with heartburn. Heartburn is where stomach acid is regurgitated back into the esophagus, and this causes a burning feeling in the chest (Oxford University Press, 2017). A buffer is a source of hydroxide ions that can absorb hydrogen ions, which in turn keeps the pH stable (Mader, 2017). In this experiment, the different antacids that are being tested to absorb the hydrogen ions from stomach acid are the buffers. The pH scale helps determine how acidic or basic a solution

As shown in the graph above, a constant pH 7 was recorded throughout the increase of acid and base. With this observation, it was clear that the liver responded in the same manner as the buffer #1. Therefore, it can be concluded that liver has a buffer characteristic in it. Another solution named buffer #2 was tested with HCL and NaOH, which results had a similar pattern to the tap water, however the rate of change in pH was quite different. The rate of pH change in buffer #2 was gradual but a sudden drop from 8-3 when 20 or more drops of HCL were added, where tap water has a higher rate of change from 1-3 drops and then became constant from 6 drops onwards. The increase in pH for Buffer #2 occured after 10 drops of NaOH was added which was quite different from the rate of change in tap

The blood pH value changes as PCO2 changes because CO2 dissolves in the blood forming carbonic acidic and lowering the pH value.

A mixture, unlike a compound, can be separated by physical means. There are multiple ways in which a mixture can be separated; furthermore, the ways it can be separated is based on what the mixture is made up of.

Metabolic alkalosis is a condition in which the body fluids have excess base. The kidneys and lungs maintain the proper balance of chemicals, called acids and bases, in the body. Decreased carbon dioxide or increased bicarbonate level makes the body too alkaline. There are different types of alkalosis such as: respiratory alkalosis, which is caused by a low carbon dioxide level in the blood. This can be due to: fever, lack of oxygen, lung disease, or liver disease; hypochloermic alkalosis is caused by an extreme lack or loss of chloride, from prolonged vomiting; hypokalemic alkalosis is caused by the kidneys’ response to an extreme lack of potassium, this can occur from taking certain water pills. Compensated alkalosis occurs when the body returns to the acid-base balance to normal in cases of alkalosis, but bicarbonate and carbon dioxide levels remain abnormal. Symptoms of alkalosis can include: confusion, hand tremor, light-headedness, muscle twitching, vomiting, and numbness or tingling in the face, hands, or feet. Treatment for alkalosis depends on

The buffer is a solution that minimises the changes in pH when small amounts of acid or base is added.There are two types of buffer solutions.They can either be acidic or alkaline.An acidic buffer is made by mixing equal amounts of a weak acid and its conjugate base.Similarly, an alkaline buffer has equal amounts of weak base and its conjugate

K.) How would you have expected Cari’s decreased Pco2 and alkaline blood pH to have affected her breathing?

Why does the blood pH value change as PCO2 changes? Because the PCO2 is directly proportional to the H+ levels which are inversely proportional to the pH level of the blood.

The possible causes of this acid base imbalance are the vomiting and the overuse of antacids. As the name implies it is bicarbonate which has been added to the body. The vomiting reduces the extracellular fluid and this in turn leads to a release of angiotensin and aldersterone. This release then increases the bicarbonate absorption and increased hydrogen ion and potassium excreted. This patient may also have hypokalemia which is very common in metabolic alkalosis and would need to be replaced if it occurred ( Thomas, 2015). The respiratory rate would also slow to try and compensate for the alkalosis.

A short term compensatory response for respiratory acidosis might include an immediate slight increase in bicarbonate levels. Another example of compensation would be hyperventilation as a response to metabolic acidosis. The compensatory response for respiratory alkalosis is a fall in the bicarbonate level – in chronic respiratory alkalosis this is achieved through renal excretion over time, while in an acute state, lower levels of CO2 produce a slight decrease of HCO3-. The compensatory response for metabolic alkalosis is hypoventilation. If all three values are abnormal, the patient is in a partially compensated state because the buffer is actively working to push the equation to equilibrium to obtain a normal pH value. If the pH is normal and the CO2 and HCO3 are both abnormal, the patient is in a fully compensated state. If the pH is abnormal and either the CO2 or HCO3 are abnormal, the patient is in an uncompensated state. The overall goal of compensation is to push the above equation as close to equilibrium as

The pH of a solution is the measure of the concentration of charged Hydrogen ions in that given solution. A solution with a pH lower than seven is considered to be acidic. A solution with a higher pH is a base. It is very important for organisms to maintain a stable pH. Biological molecules such as proteins function only at a certain pH level and any changes in pH can result in them not functioning properly. To maintain these constant pH levels, buffer solutions are used. A buffer solution can resist change to small additions of acids or base’s. A good buffer will have components that act like a base, and components that act like an acid.

HCO3-: Her bicarbonate on the day of admittance was 29.6, which is slightly elevated from the normal range of 24-28mEq/L. Bicarbonate is formed from carbon dioxide in the blood and helps to regulate the pH of the blood by acting as a buffer. It can be elevated due to the buildup of carbon dioxide due to not being exhaled properly.

Metabolic acidosis results from all conditions that decrease the pH of the body fluids below 7.35 and HCO3- levels are <22 mEq/L, with the exception of conditions resulting from altered function of the respiratory system. As hydrogen ions accumulate in the body fluids, buffers first resist a decline in pH. If the buffers cannot compensate for the increase in hydrogen ions, the respiratory center helps regulate the body fluid pH. The reduced pH stimulates the respiratory center, which causes hyperventilation. During hyperventilation, carbon dioxide is eliminated at a greater rate. The elimination of carbon dioxide also eliminates excess hydrogen ions and helps maintain the pH of the body fluids within a normal range. (Angus, 2006)

Acidosis is when the pH of one’s blood is below the normal level of 7.35. Alkalosis is when the pH of one’s blood is above 7.45. These can be broken down into two categories respiratory and metabolic. Normal oxygen (CO2) levels are 35-45 mmHg in systemic arterial blood. Normal levels for HCO3− 22-26mEq/liter in systemic arterial blood.

If an acid-base disturbance shifts the pH outside of the physiologic range, various control measures are activated to resist the change in pH. Compensatory mechanisms try to preserve the normal 20:1 ratio of bicarbonate to carbonic acid to keep the pH at normal range. The body works to maintain normal ratios through a compensation mechanism using renal and respiratory methods (Crowley, 2010).