...The title of the article is “Bicarbonate Infusion and PH Clamp Moderately Reduce Hyperventilation During Ramp Exercise In Humans.” The authors of this article are Francois Pe´ronnet, Tim Meyer, Bernard Aguilaniu, Carl-E´ tienne Juneau, Oliver Faude, and Wilfried Kindermann. The purpose of this study was to find whether bicarbonate infusion and pH clamp moderately reduce hyperventilation during ramp exercise in humans. The study was completely focused upon males; no females were tested during the experiment. “Results from the present experiment confirm that the increase in plasma H concentration contributes to the control of hyperventilation at high workloads. This stimulus could be responsible for at least 30% of the disproportionate increase in VE observed in this situation and when suppressed by bicarbonate infusion was not fully compensated by the remaining putative control mechanisms of hyperventilation”(Pe´ronnet F, Meyer T, Aguilaniu B, Juneau CE´ , Faude O, Kindermann W). This result means when you add the plasma H to your body before a workout it helps control your hyperventilation during the exercise. This study relates to what we have talked in class about the “buffer system” in how in the...
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...6. Blood Gases and Acid-Base Balance Introduction Under normal conditions, physiologic and metabolic processes in the human body require specific and constant conditions for relevant reactions or mechanisms to occur. One of the most important factors that influence reactions and/or metabolic processes is the pH for the system or environment. The end product of most of the metabolic processes of carbohydrates, lipids and proteins is the production of acids ( organic acids, volatile acids and fixed acids). These acids if not neutralized would influence the physiologic pH of blood and tissues of the body. Therefore, a buffer system must be available to prevent the accumulation of these acids and to inhibit their harmful effects. This chapter describes the mechanism and action of buffers in maintaining the proper pH in health and in disease states. Definitions (Review of basic concepts) 1. Acids: Compounds that release hydrogen (proton donors) 2. Bases: Compounds that accepts hydrogen (proton acceptor) 3. Strong Acids: Compounds with weak affinity to H+ (release all H+ ions) 4. Strong Base: Compounds with strong affinity to H+ (Bind H+ ions) 5. The dissociation constant K: It reflects the strength of an acid or base. The larger the K value, the greater the dissociation of H+ ions, thus the stronger the acid. 6. pK: is the negative log of K. The smaller the pK the stronger the acid (Strong acids has a pK 9.0) 7. Buffers: A combination of weak acid and...
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...SaO2 = 97% and HCO3- = 32 meq/liter. Interpretation If you start with the basics on this case, the first thing to determine if it is an alkalosis or an acidosis. pH is 7.5 so the result is alkalosis. pH below the 7.35 is an acidosis and pH above the 7.45 is an alkalosis. There are two organ systems that primarily help with the acid base balance in the body and that is respiratory and renal. The renal system contributes to metabolic acidosis or alkalosis. When we look at the respiratory system we are looking at the PaCO2 which in this case is normal. So the respiratory system is not the problem in this patient. When we look at the renal system then we are looking at the bicarbonate or HCO3-. When we look at that system we discover the bicarbonate is high. When the bicarbonate is high this contributes to an alkalosis so this is a metabolic alkalosis ( Fournier, 2011). Here is a basic overview of how to figure...
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...excess of acid causes pH to fall below 7.35 result in acidosis1. An excess base, causing it to rise above pH 7.45 alkalosis1 called. The imbalance is classified according to the origin of the disturbance (respiratory or metabolic) and the direction of change in pH (acidosis or alkalosis) 2 Thus may occur for example four alkalosis metabolic processes (MK), metabolic acidosis (MA ), respiratory alkalosis (RK) and respiratory acidosis (RA) 2. imbalance causes The general reasons for the accumulation of acid are usually Poor carbon dioxide (CO2) excretion eg COPD The excess production of H + from the overproduction of organic acids Excessive bicarbonate loss through excretion Acid / drug ingestion Inadequate production of H + caused by renal tubular acidosis Typical sources of acid include4 loss: Excessive bicarbonate reabsorption due to gastrointestinal problems Loss of acid through prolonged vomiting...
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...NUR-614 September 16, 2015 Acid-Base Balance The acid base balance is a homeostatic process that aides the body in maintaining a pH in the arterial blood between 7.35-7.45 (Patient, 2015). The body works together through multi-systems to ensure that acidity or alkalinity never take over within the blood. The purpose of the following paper is define the classification of the acid-base balance, define the factors from the case study, explain the pathophysiology, describe the compensatory mechanisms, pharmacological interventions, and the educational needs of patients with an imbalance. Classification In the following case study, the patient presents with metabolic alkalosis. Metabolic acidosis is a state within the blood when sodium bicarbonate (HCO3) increases. This condition can arise when the there is an acid loss within the body and HCO3 in the blood increases (Merk Manual, 2015). This process can cause the intracellular shifting of hydrogen ions, thus causing HCO3 retention. In the case study it is identified that the kidneys have a higher content of HCO3 because of the volume depletions. Normally, the kidneys filter out the HCO3 and excrete it into the urine (Merk Manual, 2015). In the case study, compensatory mechanisms have not activated, because the PaO2 is still within normal range of 35-45mm Hg, with a level of 40mm Hg. When excretion does not occur, the acid-base balance shifts from homeostasis and the body attempts to correct the alkalinity imbalance. Factors ...
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...Which of the following people would be most severely affected by prolonged vomiting? a. 3-year-old male b. 15-year-old male c. 35-year-old male d. 35-year-old female e. 50-year-old male 3-year-old male Extracellular fluid has a higher sodium content than intracellular fluid. The predominant intracellular cation is potassium. The predominant extracellular cation is sodium Which of the following fluid compartments contains the largest volume of water? a. plasma b. interstitial compartment c. intracellular compartment d. extracellular compartment e. lymph intracellular compartment Water moves back and forth across the plasma membrane by the process of osmosis One difference between the plasma and interstitial fluid is that the plasma has significantly more _____ than interstitial fluid. protein The distribution of sodium and potassium ions between intracellular and extracellular compartments is a. potassium mainly intracellular; sodium mainly in extracellular. b. sodium mainly intracellular; potassium mainly in extracellular. c. little of either intracellular but large amounts of both extracellular. d. equal amounts of both ions, in both intracellular and extracellular fluids. e. none of the above potassium mainly intracellular; sodium mainly in extracellular. Which of the following individuals would have the largest percentage of their bodyweight as water? a. a small 7-year-old female b. a lean 35-year-old male athlete c...
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...INTRODUCTION Acid-Base balance is an intricate concept which requires an intimate and detailed knowledge of the body’s metabolic pathways used to eliminate the H+ ion. Clinicians may find it daunting to understand when first introduced to the subject. This roundtable session will demonstrate how to analyze blood gas levels in a very elementary manner so as to diagnose any acid-base disorder in a matter of minutes. The body is in a constant state of flux delicately stabilizing the pH so as to maintain its normalcy. In order to prevent untoward effects of alkalosis or acidosis the body has three major buffering systems that it uses to adjust the pH. They are: 1) Plasma protein (Prot-) 2) Plasma hemoglobin (Hb-) 3) Bicarbonate (HCO3-) The Bicarbonate-Carbonic acid system is the most dominate buffering system and controls the majority of the hydrogen ion (H+) equilibrium. Maintaining homeostasis when these acid-base shifts occur is vital to survival. Metabolic and respiratory processes work in unison to keep the H+ normal and static. II. ACID-BASE ABNORMALITIES The four principal acid-base imbalances are illustrated in Table 1. as well as possible causes for each condition. The H+ ion concentration is reflected in the serum pH value. Normal pH levels range from 7.35 to 7.45 and are slightly alkaline. Elevated levels indicate alkalosis (decreased H+ ion...
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... The acid-base balance in the body largely depends on the hydrogen ion (H+) concentration. In general, high H+ makes the solution acidic with pH less than 7 while low H+ will make the solution basic or alkaline with pH higher than 7 (Lewis, 2013). Acidosis develops when the arterial pH drops below 7.35 while alkalosis develops when the arterial pH rises above 7.45 (Appel & Downs, 2008). The normal metabolic balance generally keeps the carbonic acid and bicarbonate ion to 1: 20 ratio. As the ratio changes, the body will respond to acid-base imbalance through compensation mechanisms to control acids through buffer system by either releasing or taking up H+ depending on the pH changes. Deviations from normal PCO2 cause respiratory problems while deviations from the normal HCO3− cause metabolic problems. Respiratory alkalosis is a condition that occurs when there is carbonic acid deficit as PaCO2 drops to less than 35 mm Hg. The blood pH increases while PaCO2 decreases but the bicarbonate (HCO3−) undergoes no changes (Apple & Downs, 2008). Respiratory alkalosis is primarily caused by hyperventilation due to conditions that stimulate the respiratory center such as oxygen deficiency at high altitudes, pulmonary diseases, congestive heart failure, and acute anxiety. Respiratory acidosis occurs when there is carbonic acid excess that raises the blood levels of CO2 above 45 mmHg. The blood pH decreases than 7.35 as PaCO2 increases while there is very...
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...OCEAN ACIDIFICATION- ESSAY THURSDAY, JANUARY 24TH, 2012 Covering more than 70 percent of the Earth’s surface, the ocean is one of planet Earth’s most distinguishing characteristics. Over recent years, human activities such as the burning of fossil fuels have increased the amount of carbon dioxide gas emitted to the atmosphere and the amount that dissolves into the ocean. Now, so much carbon dioxide has been absorbed by the ocean that the chemistry of seawater is changing, causing the ocean to become more acidic. THE CARBON CYCLE Carbon dioxide is a critical part of Earth’s atmosphere; it traps heat and prevents the Earth from being covered in ice. Normally, the Earth’s carbon cycle maintains a natural balance of carbon in the atmosphere, land, and ocean through the “breathing of the planet”. However, since the beginning of the industrial era, emissions of carbon dioxide have climbed, and now are exceeding the capacity of the carbon cycle to maintain equilibrium between the atmosphere and ocean. Excess carbon dioxide traps more heat in the atmosphere, which changes the Earth’s climate. Not all of the excess carbon dioxide stays in the atmosphere. Scientists estimate that one-third of all the carbon dioxide produced by human activities has been absorbed by the ocean. The ocean’s removal of carbon dioxide from the atmosphere has undoubtedly helped curb the extent of climate change—but this benefit has come at a cost. The absorption of carbon dioxide is fundamentally changing...
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...Anion test; Carbonate; The following paragraphs present the chemical reactions that you will observe in the lab this week. Compounds containing the carbonate ion (or the related ion bicarbonate or hydrogen carbonate, HCO3-) react with acids to give carbon dioxide (CO2), a colorless, odorless, and slightly acidic gas. For example, the reaction of baking soda (NaHCO3) with acids such as those in lemon juice or buttermilk releases carbon dioxide which causes baked goods to rise: HCO3- + H+ CO2 (g) + H2O In this equation the sodium ion, Na+, does not participate in the reaction and is a spectator ion. It is not included in the net ionic equation, given above. Many other gases are colorless and odorless, like CO2. To confirm that the gas formed is carbon dioxide, it can be allowed to react with Ba(OH)2, barium hydroxide, to form a white insoluble precipitate of barium carbonate, BaCO3: CO2 + Ba2+ (aq) + 2 OH- (aq) BaCO3 (s) + H2O Sulfate; Cl- + H+ (aq) HCl (g). In this reaction, the sulfate ion, SO4-2, from the sulfuric acid, is a spectator ion and is not included in the net ionic equation. Another useful reaction for identification of the chloride ion is its reaction with silver nitrate to form a white precipitate of silver chloride: Cl- + Ag+ (aq) AgCl (s) As discussed above, nitrate and sodium are spectator ions and do not appear in the net ionic equation. To test the properties of the sulfate ion, you will examine the reactions of Epsom...
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...concentration, the reaction will move forward. CO2 (g) + H2O (l) -------àH2CO3 2) Write the equilibrium constant expression for the reaction shown in question 1. 3) Calculate the equilibrium constant using the following concentrations [CO2] = 3.56 x 10-10 M and [H2CO3] = 8.8 x 10-2 M. K= [3.56] [10-10] ------------- [8.8] [10-2] = 22.63 Carbon dioxide plays a vital role in the human body and is a colourless, odourless gas produced by organic compounds and by respiration. This essay will discuss the transport and exchange of carbon dioxide, pH levels, acidosis and alkalosis and chemical equilibrium. Firstly, carbon dioxide is transported around the body in a few different ways. Some of those are, “dissolution, haemoglobin binding, and the bicarbonate buffer system” ('Transport of Carbon Dioxide in the Blood', 2015). It is not soluble in water, however, water is the main carrier transporting it from cells to lungs. PH levels for every individual vary according to their body’s organism. A balanced pH is needed “to ensure the proper functioning of metabolic processes and the delivery of the right amount of oxygen to tissues” (Labtestsonline.org, 2015). During a days cycle the body’s’ “chemical environment changed from a weak acid to a...
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...Lewis: Medical-Surgical Nursing, 9th Edition Chapter 17 Fluid, Electrolyte, and Acid-Base Imbalances KEY POINTS HOMEOSTASIS · Body fluids and electrolytes play an important role in maintaining a stable internal environment of the body. · A number of adaptive responses keep the composition and volume of body fluids and electrolytes within the narrow limits of normal to maintain homeostasis and promote health. · Many diseases and their treatments have the ability to affect fluid and electrolyte balance and alter homeostasis. WATER CONTENT OF BODY · Water is the primary component of the body, accounting for approximately 60% of the body weight in the adult. · The two major fluid compartments in the body are intracellular fluid (ICF), or inside the cells, and extracellular fluid (ECF), or outside the cells. ECF is composed of interstitial fluid, plasma, and transcellular fluids. ELECTROLYTES · Electrolyte composition varies between the ECF and ICF, though the overall concentration of the electrolytes is approximately the same in the two compartments. · The measurement of electrolytes is important in evaluating electrolyte balance, as well as in determining the composition of electrolyte preparations. MECHANISMS CONTROLLING FLUID AND ELECTROLYTE MOVEMENT · Many different processes are involved in the movement of electrolytes and water between the ICF and ECF. Some of these include simple diffusion, facilitated diffusion, and active transport. Two forces...
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...rebreathing? Your answer : d. pH and PCO2 will increase. Stop & Think Questions: Which of the following can cause respiratory acidosis? You correctly answered: c. airway obstruction Experiment Data: Condition Normal Rebreathing Min PCO2 40 40 Max PCO2 40 54.88 04/11/16 page 2 Min pH 7.39 7.22 Max pH 7.39 7.42 Post-lab Quiz Results You scored 100% by answering 4 out of 4 questions correctly. 1. Rebreathing simulates You correctly answered: a. hypoventilation and respiratory acidosis. 2. Hypoventilation results in You correctly answered: c. an accumulation of carbon dioxide in the blood. 3. The renal system can compensate for respiratory acidosis by You correctly answered: b. excreting H+ and retaining bicarbonate ion. 4. Respiratory acidosis can be caused by all of the following except You correctly answered: d. an anxiety attack. 04/11/16 page 3 Review Sheet Results 1. Describe what happened to the pH and the carbon dioxide levels during rebreathing. How well did the results compare with your prediction? Your answer: Both were affected bt rebreathing and went up. The results were exactly...
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...levels during rebreathing? Your answer : b. pH will decrease and PCO2 will increase. Stop & Think Questions: Which of the following can cause respiratory acidosis? You correctly answered: c. airway obstruction Experiment Data: Condition Normal Rebreathing Min PCO2 40 40 Max PCO2 40 53.02 Min pH 7.40 7.24 Max pH 7.40 7.42 01/09/14 page 2 Post-lab Quiz Results You scored 100% by answering 4 out of 4 questions correctly. 1. Rebreathing simulates You correctly answered: a. hypoventilation and respiratory acidosis. 2. Hypoventilation results in You correctly answered: c. an accumulation of carbon dioxide in the blood. 3. The renal system can compensate for respiratory acidosis by You correctly answered: b. excreting H+ and retaining bicarbonate ion. 4. Respiratory acidosis can be caused by all of the following except You correctly answered: d. an anxiety attack. 01/09/14 page 3 Review Sheet Results 1. Describe what happened to the pH and the carbon dioxide levels during rebreathing. How well did the results compare with your prediction? Your answer: My prediction was correct. During rebreathing the PCO2 amount in the blood increased 8.95 above the normal maximum...
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...2. Body Maintenance Of Normal pH In order to maintain a proper pH in the bodily fluids, and so that acidosis or alkalosis will not manifest, three major physiological control systems exist within the body. The first mechanism involves a buffer system for the hydrogen ion fluctuations. All bodily fluids are supplied with acid-base buffers which combine with any acid or alkaline substance and prevent excessive change in the hydrogen ion concentration. Another mechanism the body uses to maintain normal pH is within the respiratory system. When the hydrogen ion concentration (H + ) changes measurably, the respiratory system is immediately stimulated to alter the rate of pulminary ventilation. This brings about a change in the quantity of carbon dioxide (CO2) within the system. High levels of carbon dioxide in the system, as created when holding the breath or due to physiological impairments of respiration, increase the acidity of the bloodstream. Any disease that interferes with normal breathing, such as emphysema or asthma, will impede the release of CO2 from the lungs and, subsequently, this CO2 will combine with water to form carbonic acid. This increases the concentration of hydrogen ions, and thus the acidity of the blood is simultaneously increased. The last of the three major physiological control systems of the body to maintain normal pH involves the kidneys. When the (H + ) (hydrogen concentration) deviates from a normal value, the kidneys excrete either an acid or alkaline...
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