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Life Sciences
Acid / Base Balance & Buffers
| Question | Answer |
|---|---|
| pH needs to be tightly controlled to maintain | homeostasis |
| This is a chemical substance that is capable of releasing hydrogen ions (H⁺) when dissolved in water. | Acids |
| E.g. Hydrochloric acid (HCl) acid found in the | Stomach juices |
| HCl will release hydrogen ions in solutions as follows | HCl → H⁺ + Cl ⁻ (hydrochloric acid) (hydrogen ion) (chloride ion) |
| pH examples of solutions | 0 battery acid 3 soda 5 soft drinking water, coffee 6 urine, saliva 7 'pure' water 8 sea water 12 soapy water 14 liquid drain cleaner |
| What is a Base (Alkaline) | A base is a chemical substance that can accept (react with) a hydrogen ion. |
| Most bases release a hydroxide ion (OH ⁻) in solution. The hydroxide will then accept a hydrogen ion to form water. | E.g. Sodium hydroxide is an example of a base; NaOH → Na⁺ + OH ⁻ (Sodium Hydroxide) (Sodium ion) (Hydroxide ion) OH⁻ → H⁺ + H₂0 (Hydroxide ion) (Hydrogen ion) (Water |
| A reaction between an acid and a base produces a ....... and also water | Salt In this reaction, the hydrogen in the acid is replaced by the positive ion in the base. • E.g. common example of a salt is sodium chloride NaCl produced by this reaction HCl + NaOH → Na Cl + H₂O |
| Buffers are | Substances which prevent sharp changes in hydrogen ion (H⁺) concentration and maintain a relatively constant pH. |
| Buffers work by | They work by accepting or releasing these ions as needed to keep pH steady. |
| The main buffers are | The main ones are; bicarbonate, phosphate, and proteins such as haemoglobin in RBC’s and plasma proteins. |
| Buffer systems facts | Buffer systems are extremely efficient Different systems work at different rates It takes seconds for chemical buffers in the blood to make adjustments to pH |
| Several mechanisms help maintain pH of arterial blood between pH | 7.35 and 7.45 |
| Acidosis levels in blood are | under 7.35 |
| Alkalosis levels in blood are | Over 7.45 |
| Acidosis levels in respiratory are | Under 6.0 PaCO2 |
| Alkalosis levels in respiratory are | Over 4.5 PaCO2 (pH under 7.35) |
| Acidosis levels in metabolic are | Under 22 HCO3 |
| Alkalosis levels in metabolic are | Over 26 HCO3 |
| Respiratory Acidosis symptoms | Rapid, shallow, respirations BP down, vasodilation Dyspnea Headache Hyperkalemia Dysrhythmias Drowsiness, Dizziness, Disorientation Muscle weakness, hyperlexia Retention of CO2 in lungs |
| Respiratory Acidosis causes | COPD Pneumonia Anesthesia Drug Overdose |
| Respiratory Alkalosis symptoms | Deep, rapid breathing seizures Hyperventilation Tachycardia Low or normal BP Hypokalemia Numbness and tingling of extremities Light headed Lethargic, Confusion Nausea, vomiting |
| Respiratory Alkalosis causes: | Hyperventilation Anxiety, PE, Fear Mechanical ventilation |
| Metabolic acidosis symptoms: | Headache Decreased BP Hyperkalemia Muscle twitching warm flushed skin nausea vomiting Changes in LOC - Confusion dizziness compensatory hyperventilation |
| Metabolic acidosis causes: | DKA Severe diarrhea Renal failure Shock |
| Metabolic alkalosis symptoms: | Restlessness followed by lethargy Tachycardia (dysrhythmias) Compensatory Hypoventilation Confusion, LOC down Dizzy, irritable Nausea, vomiting, diarrhea tremors, muscle cramps, tingling of fingers and toes Hypokalemia |
| Metabolic alkalosis causes: | Severe vomiting, Excessive GI suctioning Diuretics Excessive NaHCO3 |
| Carbonic acid - bicarbonate buffer system | Large amounts of Bicarbonate produced from CO2 made during metabolism create the body’s most important extracellular buffer system. |
| Carbonic acid- bicarbonate buffer system | If pH rises: H2CO3 H+ + HCO3 Because CO2 and H2O combine to form this buffer system it cannot protect against pH changes due to respiratory problems in which there is an excess or shortage of CO2 |
| How Carbonic acid - bicarbonate buffer system works | HCO3is a significant anion in both ICF and ECF Based on bicarbonate ion (HCO3) acting as weak base and carbonic acid (H2CO3) acting as weak acid If pH falls: H+ + HCO3- H2CO3 H2CO3 then dissociates into water (H2O) & CO2, which can be exhaled |
Created by:
paramedicscienceUK
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