Acid and base regulation
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PREPARED BY: MUHAMMAD ARIFF B. MAHDZUB BACHELOR MEDICINE AND SURGERY (MBBS) UNIVERSITY COLLEGE SHAHPUTRA, KUANTAN
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pH Review
• pH = - log [H+
]
• H+
is really a proton
• Range is from 0 - 14
• If [H+
] is high, the solution is acidic; pH < 7
• If [H+
] is low, the solution is basic or
alkaline ; pH > 7](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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1) El documento trata sobre los equilibrios ácido-base, definiendo ácidos y bases según Arrhenius, Brønsted-Lowry y Lewis. Explica la autoionización del agua y la escala de pH.
2) Describe la fuerza de ácidos y bases en términos de sus constantes de ionización y disociación. Las sales pueden ser neutras, ácidas u básicas dependiendo del tipo de ácido y base del que procedan.
3) Se mencionan brevemente las disoluciones amortiguador
Copia de soluciones buffer o amortiguadores
Las soluciones amortiguadoras resisten cambios de pH cuando se añaden pequeñas cantidades de ácido o base. Están constituidas por un ácido débil y su sal o una base débil y su sal, como ácido acético y acetato de sodio o amonÃaco y cloruro de amonio. Mantienen el pH al neutralizar protones u oxonio a medida que se añaden, actuando como reguladores de pH.
acid base balance and imbalance
a brief overview of acid base balance, imbalance. the features, diagnosis, compensation and management.
Bicarbonato de sodio
El bicarbonato de sodio se obtiene quÃmicamente a través de la reacción de sodio, cloro, amonÃaco, agua y dióxido de carbono. Se usa principalmente en reposterÃa para dar volumen y sabor a la masa, asà como en medicina para tratar hiperacidez gástrica y acidosis. Sin embargo, debe consumirse con precaución porque una dosis mayor a una cucharadita puede producir una ruptura gástrica al reaccionar con el ácido estomacal y generar dióxido de carbono.
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El documento trata sobre las reacciones ácido-base. Explica las teorÃas de Arrhenius y Brönsted-Lowry sobre la definición de ácidos y bases. También describe cómo se calculan las constantes de acidez y basicidad y cómo éstas permiten determinar la fuerza relativa de los ácidos y bases. Finalmente, incluye tablas con las constantes de algunos ácidos y bases comunes.
Buffers
Buffers resist changes in pH upon the addition of small amounts of acid or base. They work by providing conjugate acid-base pairs that absorb added H+ or OH- ions. Common buffer systems include acetic acid/sodium acetate and phosphoric acid/sodium phosphate. The Henderson-Hasselbalch equation relates a buffer's pH to the pKa of the acid/base pair and the concentrations of the components. Buffers have important applications in biological systems like blood and pharmaceutical products where a stable and precise pH is required.
Buffer
Este documento describe las soluciones reguladoras, incluyendo su definición, ejemplos y aplicaciones. Explica que las soluciones reguladoras mantienen estable el pH a pesar de pequeñas adiciones de ácido o base. Describe los sistemas reguladores de la sangre, incluyendo el sistema fosfato dihidrogenado/fosfato hidrogenado y el sistema ácido carbónico/bicarbonato, que ayudan a mantener el pH sanguÃneo en 7.35.
Clase buffer
Las soluciones buffer mantienen el pH casi constante al agregar pequeñas cantidades de ácidos o bases. Se componen de un ácido débil o base débil y su sal correspondiente. El buffer controla el pH al reaccionar los iones H+ o OH- agregados con estas especies. Los fluidos biológicos contienen buffers importantes como H2CO3/HCO3- en la sangre y H2PO4-/HPO42- en las células, los cuales ayudan a mantener el pH sanguÃneo entre 7.35-7.45.
3 reacciones de neutralización
1) El documento describe las reacciones de neutralización que ocurren entre ácidos y bases, incluyendo la formación de sales. 2) Explica que los antiácidos funcionan neutralizando el exceso de ácido en el estómago, mientras que los inhibidores de ácido reducen la producción de ácido. 3) Proporciona ejemplos de antiácidos comunes que contienen iones hidróxido, carbonato o bicarbonato para neutralizar los ácidos estomacales.
PROPIEDADES PROTEINAS
Este archivo contiene información sobre algunas propiedades de las proteÃnas como la desnaturalizacion o su capacidad amortiguadora del pH
Soluciones Buffer
1) Las soluciones amortiguadoras son aquellas cuya concentración de hidrogeniones varÃa poco al añadir ácidos o bases fuertes, manteniendo constante el pH.
2) Los amortiguadores más sencillos están formados por mezclas de un ácido débil y la sal del mismo ácido, o una base débil y la sal del ácido conjugado.
3) La aplicación más importante es el estudio de la regulación del equilibrio ácido-base en la sangre, donde admite cantidades mayores de ácido sin variar mucho el pH.
Propiedades de las proteinas (laboratorio bioquimica)
Este documento describe una serie de experimentos sobre las propiedades de las proteÃnas. En el primer experimento, se determinó que las proteÃnas en suero sanguÃneo actúan como un buen amortiguador de pH. En el segundo, se encontró que el punto isoeléctrico de la caseÃna es de aproximadamente pH 4.7. Finalmente, se evaluó cómo diferentes iones pueden hacer precipitar a las proteÃnas dependiendo del pH de la solución.
Buffer
Este documento trata sobre los conceptos básicos de pH, ácidos, bases y soluciones tampón. Explica que las soluciones tampón ayudan a mantener constante el pH en el cuerpo mediante la mezcla de ácidos y bases débiles. Describe los principales sistemas tampón fisiológicos como el fosfato, bicarbonato y hemoglobina, y cómo las proteÃnas y aminoácidos también funcionan como tampones debido a su naturaleza anfótera.
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This document discusses acid-base balance and imbalance in the human body. It covers:
1. The body tightly regulates pH levels and uses several mechanisms to do so, including buffer systems, respiration, and kidney function.
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This document discusses biological buffers and acid-base balance in the human body. It covers:
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3) The body regulates pH through buffers, respiration, and renal excretion of acids and bases. Respiration controls carbonic acid levels while the kidneys regulate bicarbonate.
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Acid and base regulation
- 1. 1 ACID AND BASE BALANCE AND IMBALANCE PROBLEM BASED LEARNING (PBL) PREPARED BY: MUHAMMAD ARIFF B. MAHDZUB BACHELOR MEDICINE AND SURGERY (MBBS) UNIVERSITY COLLEGE SHAHPUTRA, KUANTAN
- 2. 2 pH Review • pH = - log [H+ ] • H+ is really a proton • Range is from 0 - 14 • If [H+ ] is high, the solution is acidic; pH < 7 • If [H+ ] is low, the solution is basic or alkaline ; pH > 7
- 3. 3
- 4. 4
- 5. 5 • Acids are H+ donors. • Bases are H+ acceptors, or give up OH- in solution. • Acids and bases can be: –Strong – dissociate completely in solution • HCl, NaOH –Weak – dissociate only partially in solution • Lactic acid, carbonic acid
- 6. 6 The Body and pH • Homeostasis of pH is tightly controlled • Extracellular fluid = 7.4 • Blood = 7.35 – 7.45 • < 6.8 or > 8.0 death occurs • Acidosis (acidemia) below 7.35 • Alkalosis (alkalemia) above 7.45
- 7. 7
- 8. 8 Small changes in pH can produce major disturbances • Most enzymes function only with narrow pH ranges • Acid-base balance can also affect electrolytes (Na+ , K+ , Cl- ) • Can also affect hormones
- 9. 9 The body produces more acids than bases • Acids take in with foods • Acids produced by metabolism of lipids and proteins • Cellular metabolism produces CO2. • CO2 + H20 ↔ H2CO3 ↔ H+ + HCO3 -
- 10. 10 Control of Acids 1. Buffer systems Take up H+ or release H+ as conditions change Buffer pairs – weak acid and a base Exchange a strong acid or base for a weak one Results in a much smaller pH change
- 11. 11 Bicarbonate buffer • Sodium Bicarbonate (NaHCO3) and carbonic acid (H2CO3) • Maintain a 20:1 ratio : HCO3 - : H2CO3 HCl + NaHCO3 ↔ H2CO3 + NaCl NaOH + H2CO3 ↔ NaHCO3 + H2O
- 12. 12 Phosphate buffer • Major intracellular buffer • H+ + HPO4 2- ↔ H2PO4- • OH- + H2PO4 - ↔ H2O + H2PO4 2-
- 13. 13 Protein Buffers • Includes hemoglobin, work in blood and ISF • Carboxyl group gives up H+ • Amino Group accepts H+ • Side chains that can buffer H+ are present on 27 amino acids.
- 14. 14 2. Respiratory mechanisms • Exhalation of carbon dioxide • Powerful, but only works with volatile acids • Doesn’t affect fixed acids like lactic acid • CO2 + H20 ↔ H2CO3 ↔ H+ + HCO3 - • Body pH can be adjusted by changing rate and depth of breathing
- 15. 15 3. Kidney excretion • Can eliminate large amounts of acid • Can also excrete base • Can conserve and produce bicarb ions • Most effective regulator of pH • If kidneys fail, pH balance fails
- 16. 16 Rates of correction • Buffers function almost instantaneously • Respiratory mechanisms take several minutes to hours • Renal mechanisms may take several hours to days
- 17. 17
- 18. 18
- 19. 19 Acid-Base Imbalances • pH< 7.35 acidosis • pH > 7.45 alkalosis • The body response to acid-base imbalance is called compensation • May be complete if brought back within normal limits • Partial compensation if range is still outside norms.
- 20. 20 Compensation • If underlying problem is metabolic, hyperventilation or hypoventilation can help : respiratory compensation. • If problem is respiratory, renal mechanisms can bring about metabolic compensation.
- 21. 21 Acidosis • Principal effect of acidosis is depression of the CNS through ↓ in synaptic transmission. • Generalized weakness • Deranged CNS function the greatest threat • Severe acidosis causes –Disorientation –coma –death
- 22. 22 Alkalosis • Alkalosis causes over excitability of the central and peripheral nervous systems. • Numbness • Lightheadedness • It can cause : – Nervousness – muscle spasms or tetany – Convulsions – Loss of consciousness – Death
- 23. 23