...THEORIES OF ACIDS AND BASESThis page describes the Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases, and explains the relationships between them. It also explains the concept of a conjugate pair - an acid and its conjugate base, or a base and its conjugate acid. | | | The Arrhenius Theory of acids and basesThe theory * Acids are substances which produce hydrogen ions in solution. * Bases are substances which produce hydroxide ions in solution.Neutralisation happens because hydrogen ions and hydroxide ions react to produce water.Limitations of the theoryHydrochloric acid is neutralised by both sodium hydroxide solution and ammonia solution. In both cases, you get a colourless solution which you can crystallise to get a white salt - either sodium chloride or ammonium chloride.These are clearly very similar reactions. The full equations are:In the sodium hydroxide case, hydrogen ions from the acid are reacting with hydroxide ions from the sodium hydroxide - in line with the Arrhenius theory.However, in the ammonia case, there don't appear to be any hydroxide ions!You can get around this by saying that the ammonia reacts with the water it is dissolved in to produce ammonium ions and hydroxide ions:This is a reversible reaction, and in a typical dilute ammonia solution, about 99% of the ammonia remains as ammonia molecules. Nevertheless, there are hydroxide ions there, and we can squeeze this into the Arrhenius theory.However, this same reaction also happens...
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...Acid-Base Imbalance Janet J Memoli Grand Canyon University NUR 641E September 30, 2015 Acid- Base Imbalance One of the basic concepts that new nurses need to learn is that homeostasis in the body is maintained by the acid base balance in the body. That concept is critical when looking at arterial blood gases. This can help guide the nurse to anticipate what the doctor will order and the education that she needs to give the patient and the family. This case study should help to illustrate the point. Case Study The case study that was given to us is a 22 year old woman who reports being “sick with the flu” She has been vomiting and having difficulty keeping food and drink down. In addition she has been taking antacids to calm down the nausea. After fainting at home she was driven to the local hospital where they have put in an IV. Her blood gas reveals the following: pH of 7.5, PaCO2 = 40 mm Hg, PaO2= 95 mm Hg, 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...
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...emergency department for management of acute mushroom poisoning. Her respirations are slow and shallow, and she is non-responsive. She is admitted to the critical care unit to be closely monitored for the development of ventilatory failure and renal failure, which often accompany mushroom poisoning. Her urine output is decreased at about 20 ml/hr. Her laboratory values are: * Serum K+ = 5.7 mEq/L * Arterial blood gases (ABGs) * pH = 7.13 * PaCO2 = 56 mm Hg * PaO2 = 89 mm Hg * HCO3– = 18 mEq/L. Questions 1. What is the relationship between acid-base balance and serum potassium level? 2. What is the reason for L.S.’s low urine output? How should her fluids be managed? 3. Categorize and explain the probable cause of L.S.’s acid-base disorder. 4. Can L.S. compensate for her acid-base disorder? Why or why not? 5. How should her acid-base imbalance be medically managed? 1. Acid-base balance can influence the serum K+ levels detected in the blood. When a patient experiences hypokalemia, K+ is excreted from the cells and H+ takes its place creating an alkalotic state; K+ is processed out of the body via the kidneys and polyuria can be a clinical symptom. In the case of hyperkalemia, K+ is not properly processed by the kidneys as a result of renal failure; decreased urine output is a clinical symptom. 2. The reason for the patient’s low urine output is due to her acute renal failure. Since the kidneys are in failure, they cannot properly...
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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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...Acid-Base Balance Kelly Heffron Grand Canyon University 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...
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...School of Nursing, Midwifery and Interprofessional Studies. With reference to acid-base balance explore the role of the respiratory system in maintaining blood pH? ‘We live and die at the cellular level’ (Reid, 2011). Homeostasis is crucial for normal cellular function. Acid-base homeostasis is the part of human homeostasis and refers to the balance between the production and elimination of H+ hydrogen ions (pH) within the body fluids (William, Simpkins, 2001, p.236). Metabolic reactions within the cells often produce a huge excess of H+. Lack of any mechanism for its excretion would lead H+ levels in body fluids rise quickly to the lethal levels (Tortora, Grabowski 2006, p.1001); therefore the homeostasis of the right H+ levels is crucial for our survival. In a healthy person several systems work interdependently on maintaining blood’s pH (Sheldon, 2001, p.23): buffer, renal and respiratory systems. In this essay I will concentrate on the pH of the blood in relation to the acid-base balance and the role that respiratory system has in maintaining it. Blood pH is a measure of its acidity or alkalinity. A pH of 7.4 is considered neutral in the systemic arterial blood within its narrow range of around 7.35 and 7.45. When the pH is greater than 7.45 the blood is considered to be alkalotic and when the pH is lower than 7.35 then the blood is considered acidotic (Sheldon, 2001, p.23). Fig. 1: Diagram of blood pH scale: (JupiterIonizer, 2004) The acidity or alkalinity...
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...Outcome I Acids and Bases Define acid and base using Arrhenius, Bronsted-Lowry, and Lewis definitions. Classify common items as acid or base by their characteristics such as taste, reaction with indicators, etc. Calculate the pH and pOH of solutions and use pH to classify them as acids or bases Perform titration calculations using pH, pOH and molarities Definitions: Acid Base Arrhenius model Brønsted-Lowry model Conjugate Acid Conjugate Base Conjugate acid-base pair Amphoteric Lewis model Hydronium Strong acid Stron base Weak acid Weak base Ion product constant for water pH pOH Logarithm Neutralization reaction Salt Titrant Equivalence point End point Titration Indicator Questions and Calculations 1) a.What is Kw? b. What is the concentration of H3O+ in pure water? c. What is the concentration of OH- in pure water? d. What are the properties of a neutral solution? 2) Identify each of these as an acid, a base, both or neither | |Acid |Base |Both |Neither | |Fe | | | | X | |NaOH | | | | | |H2SO4 | ...
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...Acids taste sour, are corrosive to metals, change litmus (a dye extracted from lichens) red, and become less acidic when mixed with bases. Bases feel slippery, change litmus blue, and become less basic when mixed with acids. While Boyle and others tried to explain why acids and bases behave the way they do, the first reasonable definition of acids and bases would not be proposed until 200 years later. In the late 1800s, the Swedish scientist Svante Arrhenius proposed that water can dissolve many compounds by separating them into their individual ions. Arrhenius suggested that acids are compounds that contain hydrogen and can dissolve in water to release hydrogen ions into solution. For example, hydrochloric acid (HCl) dissolves in water as follows: HCl | H2O | H+(aq) | + | Cl-(aq) | Arrhenius defined bases as substances that dissolve in water to release hydroxide ions (OH-) into solution. For example, a typical base according to the Arrhenius definition is sodium hydroxide (NaOH): NaOH | H2O | Na+(aq) | + | OH-(aq) | The Arrhenius definition of acids and bases explains a number of things. Arrhenius's theory explains why all acids have similar properties to each other (and, conversely, why all bases are similar): because all acids release H+ into solution (and all bases release OH-). The Arrhenius definition also explains Boyle's observation that acids and bases counteract each other. This idea, that a base can make an acid weaker, and vice versa, is called neutralization...
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...Acid and Base Extraction Finding the unknown compound by extraction using their conjugate acid and base. Huda Introduction The purpose of the acid and base extraction lab is to determine the unknown mixture that contains three compounds which is made of an organic acid, an organic base and an organic neutral. To find out what the unknown compounds are found in the mixture, a series of techniques are done. To extract the compounds from the given unknown mixture, they were changed back to their conjugate acids by adding a strong acid and back to their conjugate bases by adding a strong base. The first technique is called extraction in which organic Bases and organic acids are separated from neutral compounds and from each other by using an aqueous solution of different PH values. Compounds that contain less than six carbons are not affected by changing the pH value. The compounds are extracted based on the solubility properties of the acid, bases and salts. The unknown compound will be dissolved in dichloromethane and HCl will be added and extraction will occur by mixing the solution and removing the aqueous layer. The extracted aqueous layer will be isolated by adding NaOH which will make the solution basic that will lead it to precipitate. The organic acid will be extracted NaOH to the dichloromethane solution and separating the aqueous solution. The majority of organic carboxylic acids are highly soluble in dilute NaOH since the acid gets deprotonated by the base and...
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...Acis CHEMICAL REACTIONS: ACID-BASE BUFFERS Short Overview Acids and bases represent two of the most common classes of compounds. Many studies have been done on these compounds, and their reactions are very important. Perhaps the most important reaction is the one in which an acid and base are combined, resulting in the formation of water (in aqueous solution) and a salt; this reaction is called neutralization. A buffer solution is a solution that contains both an acid and a salt containing the conjugate base anion in sufficient concentrations so as to maintain a relatively constant pH when either acid or base is added. In this experiment you will prepare a buffer solution and observe its behavior when mixed both with an acid and a base. You will also compare the behavior with that of solutions containing only the acid. Theory In his theory of ionization in the 1880’s, Svante Arrhenius defined acids are substances which form H+ and bases as substances which form OH- in water. He further defined a salt as a substance other than an acid or base which forms ions in aqueous solution. Such substances are thus capable of producing an electric current and are called electrolytes. The amount of electricity produced is directly proportional to the concentration of ions in solution. With regard to electrolytes we have learned previously that strong acids and strong bases ionize completely, and are therefore strong electrolytes because they...
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...1. Write all acid-base hydrolysis reactions for the polyprotic acid. Clearly show the structure of the species, and the charges. Identify all possible acidic and basic species. Answer: Pyrophosphoric acid, also known under the name diphosphoric acid, is colorless, odorless, hygroscopic and is soluble in water, diethyl ether, and ethyl alcohol. It is produced from phosphoric acid by dehydration. Pyrophosphoric acid slowly hydrolyzes in the presence of water into phosphoric acid. H4P2O7 + H2O ↔ H3P2O7-1 + H3O+ structure of species: + H3O+ Acid con. base H3P2O7-1 + H2O ↔ H2P2O7-2 + H3O+ structure of species: + H3O+ Acid con. base H2P2O7-2 + H2O ↔ HP2O7 -3 + H3O+ structure of species: + H3O+ Acid con. base HP2O7 -3 + H2O ↔ P2O7-4 + H3O+ structure of species: + H3O+ Acid con. Base : fully deprotonated speices will undergo base hydrolysis reaction to produce conjugate acid P2O7-4 + H2O ↔ HP2O7 -3 + OH- Base Con. Acid Species Acid Dissociation constants H3P2O7-1 Ka1 1.50E-01 Pka1 0.83 H2P2O7-2 Ka2 5.50E-03 Pka2 2.26 HP2O7-3 Ka3 1.90E-07 Pka3 6.72 P2O7-4 Ka4 3.50E-10 Pka4 9.46 Pyrophosphoric acid is a medium strong inorganic acid. Anions, salts, and esters of pyrophosphoric acid are called pyrophosphates. 2. Calculate fractions (αI ) of all the species as a function of pH in the range of 1-13. Use the equations given in the handout. Calculate...
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...Acid-base disturbances The Acid Base Imbalance Regulation of hydrogen ion concentration in the body is a necessity for normal body functions.1 H + concentration in all body fluids are maintained to maintain pH ranges within narrow limits, this service is known as the balance acid-base (AB) 2.Arterial blood pH is maintained between 7.35-7.45, venous blood remains near 7,352. Most diseases / conditions disrupt AB, AB changes may be more harmful than the initial pathology. When AB is affected, causing the pH to vary from its limits, is called an acid-base (ABI) imbalance 2 However, there are processes instead of ABI less likely to occur. AB is maintained sequentially by several mechanisms: chemical buffers, respiratory system and renal system 3. Acid-Base Imbalance ABI is an irregularity in the body's balance of acids and bases. These deviations cause blood pH deviates outside its normal range. Imbalances can become life threatening. When an 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...
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...Background: Acids are substances that are characterized by their ability to donate protons (H+) to other substances in a solution. Acids can be strong or weak. Weak acids do not ionize completely and are found in everyday substances. Acidity is a measure of the amount of dissolved hydrogen ions in a solution. The greater the number of hydrogen ions in a solution, the more acidic the solution. Strong acids donate hydrogen ions in water, to a much greater extent than weak acids. Bases are substances that are characterized by their ability to accept protons or produce hydroxide ions (OH-) in an aqueous solution. As for acids, the difference in strength of bases directly relates to the degree in which hydroxide ions are formed by the base in water. Like strong acids, strong bases are also dangerous chemicals. Weak bases are found in many everyday items. When feeling the consistency of a base, it feels slippery because it degrades the fatty acids and oils in the skin on contact. However, due to the possibility that an acid or a base could be very dangerous to human tissue, never experiment with an acid or base by tasting or touching it. To determine if a substance is an acid or a base, a pH scale may be used. pH is a measure of the concentration of hydrogen ions in a substance. The equation for pH is: pH = -log [H+]. The logarithm for pH is based on a scale of 10. As pH is a negative logarithm, the pH of a substance increases as the concentration of hydrogen ions decreases. For...
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... AA Acids, Bases & Indicators Comprehensive tutorial notes Julius G.Thungu jgthungu@gmail.com 0711 354 885 INTRODUCTION TO ACIDS, BASES AND INDICATORS 1.In a school laboratory: (i)An acid may be defined as a substance that turn litmus red. (ii)A base may be defined as a substance that turn litmus blue. Litmus is a lichen found mainly in West Africa. It changes its colour depending on whether the solution it is in, is basic/alkaline or acidic. It is thus able to identify/show whether another substance is an acid, base or neutral. (iii)An indicator is a substance that shows whether another substance is a base/alkaline,acid or neutral. 2.Common naturally occurring acids include: Name of acid | Occurrence | 1.Citric acid | Found in ripe citrus fruits like passion fruit/oranges/lemon | 2.Tartaric acid | Found in grapes/baking powder/health salts | 3.Lactic acid | Found in sour milk | 4.Ethanoic acid | Found in vinegar | 5.Methanoic acid | Present in ants, bees stings | 6.Carbonic acid | Used in preservation of fizzy drinks like coke, Lemonade, Fanta | 7.Butanoic acid | Present in cheese | 8.Tannic acid | Present in tea | 3.Most commonly used acids found in a school laboratory are not naturally occurring. They are manufactured. They are called mineral acids. Common mineral acids include: Name of mineral acid | Common use | Hydrochloric acid (HCl)...
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...29 EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric acid is prepared, standardized against pure sodium carbonate, and used to determine the percentage of carbonate in a sample. An aqueous solution of hydrochloric acid is almost completely dissociated into hydrated protons and chloride ions. Therefore, in a titration with hydrochloric acid the active titrant species is the hydrated proton. This species is often written H3O+, although the actual form in solution is more correctly (H2O)nH+. For convenience we designate it simply H+. Carbonate in aqueous solution acts as a base; that is, it is able to accept a proton to form bicarbonate ion. 2CO3 + H+ HCO3 (1) Bicarbonate is able to combine with another proton to form carbonic acid: HCO3 + H+ H2CO3 (2) Equilibrium expressions for the dissociation of bicarbonate and carbonic acid may be written 2[H+] [CO3 ] K2 = (3) [HCO3] [H+] [HCO3] [H2CO3] and K1 = (4) 30 where K1 and K2 are the first and second acid dissociation constants for H2CO3; the experimentally determined values are K1 = 3.5 x 10-7 and K2 = 5 x 10-11. When successive protonation reactions such as (1) and (2) occur, the extent to which the first reaction proceeds before the second begins depends on the difference between the two acid dissociation constants. By combination of Equations (3) and (4) with those for charge and...
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