Pharmacology Quiz on Electrolytes and pH Balance

<p>Acute dehydration (C)</p> Signup and view all the answers

<p>Abnormal decrease in blood pH (A)</p> Signup and view all the answers

<p>Potassium chloride (D)</p> Signup and view all the answers

<p>74.56 (A)</p> Signup and view all the answers

<p>Potassium deficiency treatment (C)</p> Signup and view all the answers

<p>Inability to excrete alkali due to renal damage (B)</p> Signup and view all the answers

<p>Decrease in arterial pCO2 (C)</p> Signup and view all the answers

<p>Formation of insoluble precipitates (D)</p> Signup and view all the answers

<p>As a laxative (C)</p> Signup and view all the answers

<p>Excessive vomiting (D)</p> Signup and view all the answers

<p>Sodium bicarbonate (D)</p> Signup and view all the answers

<p>Excessive Cl– and sodium loss due to diuretics (C)</p> Signup and view all the answers

<p>Increases (A)</p> Signup and view all the answers

<p>It helps maintain the extracellular pH within a narrow range. (D)</p> Signup and view all the answers

<p>It removes more protons for each millimole of oxygen dissociated. (D)</p> Signup and view all the answers

<p>An exchange of bicarbonate for chloride ions. (D)</p> Signup and view all the answers

<p>27/1.35 meq/lt (D)</p> Signup and view all the answers

<p>It reacts with water to form carbonic acid. (B)</p> Signup and view all the answers

<p>Breathing regulation influences the levels of carbon dioxide and bicarbonate. (D)</p> Signup and view all the answers

<p>It provides a sufficient concentration to maintain buffering. (C)</p> Signup and view all the answers

<p>An abundance of oxygen combining with deoxyhemoglobin. (D)</p> Signup and view all the answers

<p>To restore the volume and composition of body fluids to normal (C)</p> Signup and view all the answers

<p>100 ml per minute (D)</p> Signup and view all the answers

<p>Irrigating body cavities or tissues (C)</p> Signup and view all the answers

<p>0.85% to 0.95% (A)</p> Signup and view all the answers

<p>Higher sodium concentration (D)</p> Signup and view all the answers

<p>During maintenance therapy when oral intake is not possible (C)</p> Signup and view all the answers

<p>5.0 to 7.5 (A)</p> Signup and view all the answers

<p>Potassium chloride (C)</p> Signup and view all the answers

<p>4:1 (C)</p> Signup and view all the answers

<p>Sodium hydrogen exchange (D)</p> Signup and view all the answers

<p>Excess production of protons (C)</p> Signup and view all the answers

<p>Administration of sodium salts of bicarbonate (C)</p> Signup and view all the answers

<p>Retention of carbon dioxide (D)</p> Signup and view all the answers

<p>Increased dietary bicarbonate (A)</p> Signup and view all the answers

<p>Diarrhea (C)</p> Signup and view all the answers

<p>Lactate and acetate (B)</p> Signup and view all the answers

<p>As a buffer in metabolic acidosis (B)</p> Signup and view all the answers

<p>Granular crystals (D)</p> Signup and view all the answers

<p>Anticoagulation of blood (C)</p> Signup and view all the answers

<p>Practically insoluble (C)</p> Signup and view all the answers

<p>Diuretic effect (D)</p> Signup and view all the answers

<p>7.5 to 9.2 (C)</p> Signup and view all the answers

<p>In airtight containers (B)</p> Signup and view all the answers

<p>Practically insoluble (A)</p> Signup and view all the answers

The process of restoring the volume and composition of body fluids to normal levels.

A condition that occurs when the body loses excessive fluid, affecting circulation, blood volume, and overall fluid balance.

A solution used to replenish fluids and electrolytes, typically used in intravenous therapy.

A type of sodium chloride solution used in medical treatments, containing a specific concentration of sodium chloride.

A type of sodium chloride solution used in medical treatments, containing a higher concentration of sodium chloride than isotonic solutions.

A type of intravenous solution containing sodium chloride, potassium chloride and calcium chloride, often used for fluid and electrolyte replacement.

Solutions used in medical treatments to restore fluid balance, categorized by their concentration compared to the body's fluids.

The process of providing fluids and electrolytes to maintain normal bodily function, especially during times of illness or dehydration.

A sterile solution containing calcium chloride in water for injection. Used for calcium replacement therapy. It is clear, colorless, and has a pH between 5 and 7.5. It does not contain any antimicrobial agents.

A sterile solution of sodium chloride and dextrose in water for injection. Used for fluid and electrolyte replacement. It is clear, colorless or faintly straw-colored, with a pH between 3.5 and 6.5. It contains a specific concentration of sodium chloride and dextrose.

A white crystalline solid used to replenish potassium in the body. It is less soluble in water than sodium chloride, and more soluble in boiling water. It is also soluble in glycerine but insoluble in alcohol.

A white, odorless powder that is soluble in water. Used as an oral calcium supplement in cases of calcium deficiency.

A decrease in the pH of the blood, making it more acidic.

A clinical state that can lead to acedemia. This state can involve respiratory or metabolic disturbances.

An increase in the pH of the blood, making it more alkaline.

A clinical state that can lead to alkalemia. This can involve respiratory or metabolic issues.

The chemical system in the body that helps maintain a stable pH level, primarily composed of bicarbonate (HCO3-) and carbonic acid (H2CO3).

The ability of the body to maintain a stable pH level within a narrow range, typically between 7.38 and 7.42.

The process by which the body produces acids as a byproduct of normal metabolic reactions.

The process of maintaining a stable pH level in the blood, within a narrow range of 7.38 to 7.42, using various buffer systems.

The primary buffer system that controls blood pH, composed of bicarbonate and carbonic acid.

The process by which carbon dioxide (CO2) produced in cells diffuses into the blood and reacts with water to form carbonic acid (H2CO3).

A process that occurs in red blood cells (RBCs) where bicarbonate ions (HCO3-) diffuse out of the RBCs and chloride ions (Cl-) diffuse into the RBCs to maintain electrical neutrality.

The ability of hemoglobin in red blood cells to bind with and release protons (H+), effectively buffering carbonic acid produced during metabolism.

The phosphate buffer system is a complex of HPO4-2 and H2PO4-, which acts as a buffer in the body fluids. It effectively maintains pH. At pH 7.4, the ratio of HPO4-2 to H2PO4- is approximately 4:1.

Metabolic acidosis occurs due to excess proton production in the body, often caused by accelerated metabolism, intake of acidic drugs, or loss of alkaline fluids.

Respiratory acidosis is caused by an accumulation of carbon dioxide (CO2) in the body, leading to increased carbonic acid content. It can be caused by chronic lung diseases, respiratory muscle paralysis, or drugs that interfere with breathing.

Metabolic acidosis is treated by administering sodium salts like bicarbonate, lactate, acetate, or citrate. These substances help increase the HCO3-/H2CO3 ratio, restoring pH balance.

Renal acidosis occurs when the kidneys are unable to properly remove H+ from the body. It can be seen in tubular disorders, Addison's disease, or when certain drugs interfere with H+ secretion.

Sodium hydrogen exchange is a critical process in the kidney that removes H+ from the body. Sodium (Na+) in the tubular fluid is exchanged for hydrogen ions (H+), leading to the excretion of acidic urine.

The kidneys play a vital role in maintaining acid-base balance by excreting H+ in the urine. They achieve this by filtering and reabsorbing substances, adjusting the concentration of H+ and bicarbonate to stabilize pH.

A state of alkalosis where the hydrogen ion concentration in the plasma remains normal, despite an overall reduction in body's hydrogen ion content.

A type of alkalosis caused by the kidneys' inability to excrete alkali efficiently. It can occur due to alkali ingestion, excessive vomiting, or renal damage.

A type of alkalosis that develops following the administration of diuretics, leading to excessive loss of chloride and sodium ions.

A type of alkalosis caused by hyperventilation, which removes excess carbon dioxide from the body, reducing the hydrogen ion concentration.

A common medicine used in treating metabolic acidosis, diarrhea, acidic drug poisoning, and dyspepsia. It also has uses in ophthalmic and ear care.

A salt used in various medical applications, including as an alternative to sodium bicarbonate in some cases.

A colorless, transparent crystal or white granular powder that is soluble in water and alcohol. It acts as a buffer in metabolic acidosis and is used in peritoneal dialysis fluid.

A white, granular crystal or white crystalline powder that is soluble in water but practically insoluble in ethanol. It has various uses, including systemic alkalizing, anticoagulation, and desensitizing agent in dentifrices.

A transparent, odourless, hygroscopic crystal or a white granular powder, soluble in water and glycerol, but practically insoluble in alcohol. It is used as a systemic alkalizer and a gastric antacid.

A sterile solution of ammonium chloride in water for injection. It contains not less than 99.5% and not more than 105% of ammonium chloride with reference to dried substance. It is used to adjust the acid-base equilibrium of the body and has a diuretic effect.