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Cathartics( Sodium Phosphate, Magnesium carbonate, Magnesium hydroxide, Magnesium sulphate).pptx

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Gayatri Patra
Gayatri Patra

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Cathartics Gayatri Patra Asst. Professor EPCP, Bangalore
Cathartics • Cathartics: These are those agents or drugs which bring about defection. They are beneficial in constipation. • Constipation: It is a condition when a person passes less than three bowel movement( defecation) in a week or has difficult. Defecation is the process of passing stool. It is mainly depends on peristaltic (bowel) movement i.e. movement of intestines. • It is occurs due to continuously ignoring the urge to defecate. • It can also be brought about by many factors like weakness of intestine, injury or use of certain drugs and diet etc. • In constipation faecal material becomes dry and hard.
• Cathartics are present into two forms: • A) Laxative: These are mild acting cathartics, which are used to treat constipation. • B) Purgative: These are strong cathartics, which are basically used to remove faecal material. • Classification: • On the basis of their mechanism, they are classified as follow:- • Stimulants: These are the drugs or chemicals which act by local irritation on intestinal tract and bring about stimulation of peristaltic activity. Drug like: Senna, Podophyllum, Castor oil, Aloe. • Bulk purgatives: These are the agents which are able to increase bulk of intestinal content which further increases the bowel movement. • These are cellulose or non- digestable type of materials. Ex. Methyl cellulose, Sodium Carboxy methyl cellulose, gum, isapgol etc.
• Lubricants: It cause smooth clearance of the fecal material. e.g. Liquid paraffin, glycerine, mineral oils etc. Saline cathartics: Saline cathartics, also known as osmotic laxatives, are a class of laxatives that work by drawing water into the intestines, thereby increasing the volume of intestinal contents and stimulating bowel movements. These act by increasing the osmotic load of intestine by absorbing large quantity of water and thereby stimulate peristalsis. Poorly absorbable cations like calcium, magnesium and anions like phosphate, sulphate. These cathartics are taken in the form of suspension, tablet or in other suitable formulations. Saline laxative and cathartic agents are different magnesium salts such as magnesium hydroxide, magnesium sulphate, etc.
Magnesium sulphate • It is also known as Epsom salt. • Chemical formula: Mgso4. 7H2O • Molecular Weight: 246.47 g/mol • Method of preparation: 1. It is obtained by the action of dilute sulphuric acid on magnesium carbonate or magnesium oxide or from native carbonate. • MgCO3 + H2SO4 MgSO4 + H2O + CO2 • The solution is filtered and filtrate is evaporated to crystallisation. • 2. It is manufactured by the action of sulphuric acid on the native carbonate or dolomite(rich in MgCO3). • When dolomite is used, magnesium sulphate passes into solution, sparingly soluble calcium sulphate gets deposited.
• MgCO3 . CaCO3 + 2H2SO4 MgSO4 + CaSO4 + 2CO2 + 2H2O • The liquid is filtered and evaporated to crystallization. • 3. Magnesium salt occurring in brine which is used for the extraction of bromine. The liquors after removal of bromine are treated with milk of lime, thus ppt. out magnesium salt as magnesium hydroxide. • Sulphur dioxide and air are passed through the suspension of magnesium hydroxide. • 2Mg(OH)2 + 2SO2 + O2 2MgSO4 + 2H2O • On crystallization, crystals of MgSO4 , 7H2O are obtained.
• Properties: It occurs as colourless crystals having a cool, saline bitter taste. It is soluble in water and sparingly soluble in alcohol. • Identification: It gives reactions which are characteristic of magnesium and sulphate • Tests for purity: It has to be tested for As, Fe, Zn, Heavy metals and loss on drying. • Clarity and colour of solution: 5 g of magnesium sulphate is dissolved in sufficient water to produce 50 ml. It should give a clear and colourless solution. • Acidity or alkalinity: 1 g of magnesium sulphate is dissolved in 10 ml of water. This solution is neutral to litmus solution. • Assay: 0.3 g of the sample weighed accurately. It is dissolved in 50 ml of water. To it 10 ml of strong ammonia ammonium chloride solution is added. Now this solution is titrated with 0.05 M disodium ethylenediaminetetraacetate using 0.1 g of Mordant Black 11 mixture as indicator until the pink colour gets discharged from the blue.
• Storage: It is kept in tightly closed-container. • Action and uses: Magnesium sulphate is given orally in dilute solutions. About 5 g gives rise to laxative effect. • Due to bitter and nauseating taste it is given in fruit juices. • The mechanism of action is that magnesium sulphate does not get absorbed from intestinal tract and thus retains sufficient water within the lumen and hydrostatic pressor is able to promote motor activity. • Usual dose is 10-15 g.
Magnesium hydroxide • Formula : Mg(OH)2 • Mol. wt. : 58.32g/mol • It is having not less than 95% and not more than 100.5 % Mg(OH)2. • Preparation: The magnesium hydroxide obtained in the preparation of milk of magnesia is evaporated to dryness. It is also prepared by treating sea water or other natural brines with sufficient calcium hydroxide to ppt. magnesium as magnesium hydroxide, then washing and drying the ppt. • Properties: It is a white fine amorphous powder. It is almost insoluble in water and slightly in alkaline. It dissolves in dilute mineral acids.
• Assay: An accurately weighed amount of sample is taken in a flask. To it 25 ml of 1 N H2SO4 is added. Now the excess of acid is back titrated with 1 N NaOH using methyl red as an indicator. • Each ml of 1 N H2SO4 = 0.02917 g of MG (OH)2 • Uses: It is used as an antacid. In larger doses (2-4g) this acts as cathartic.
Magnesium carbonate • Magnesium carbonate Molecular mass is 84.31 g/mol. • Carbonate having an approximate chemical composition 3 MgCO3. Mg (OH)2 . 5H2O. • It contains the equivalent of not less than 40% and not more than 45% of MgO. • Heavy magnesium carbonate is different from light magnesium carbonate in density. 15g of heavy magnesium carbonate occupies a volume of 30 ml while light magnesium carbonate occupies a volume of 125 ml. • Preparation: Magnesium sulphate (125 Parts) and sodium carbonate (150 parts) are dissolved separately in water and the solutions are mixed (1:1 ratio) . The residue is digested with boiling water for 30 minutes with water and the insoluble magnesium carbonate is filtered on calico cloth, washed until it becomes free from sulphate ions and dried in an oven. MgSO4 + Na2CO3 MgCO3 + Na2SO4 • Properties: It is a white granular powder, odourless and tasteless. It is insoluble in water and alcohol.
• Tests for purity: It has to be tested for As, Ca, Fe, Copper, chloride, sulphate and soluble matter. • Residue on ignition: Residue should not be less than 42% and not more than 45%. • Tests for soluble matter: 1 gm heavy magnesium carbonate + 50 ml water , boiled for 5 minutes, then filtered and finally dried to constant weight at 105 ° c. The residue weighs not more than 10 mg. • Assay: 1 g sample is dissolved in sufficient quantity of dilute hydrochloric acid and the volume is made to 250 ml with the help of water. To 50 ml of this solution, add 100 ml of water and 15 ml of NaOH solution. After addition of 40 mg of murexide indicator and 3 ml of naphthol green, titrate with 0.05 M disodium EDTA until deep blue colour develops. • Uses: It is used as an antacid in the dose range of 500 mg to 2 g four times a day as a laxative in the dosage range of 2-4 g.
Sodium Phosphate • It is also known as Disodium hydrogen phosphate • Chemical formula: Na2HPO4 . 12H2O • Molecular weight: 358.14 g/mol. • It contains not less than 98.5 % and not more than 101.0% of Na2HPO4 which is calculated with reference to the substance dried at 130°. • Preparation: Adding sodium carbonate to a hot solution of phosphoric acid. Sodium carbonate fails to affect the third hydrogen of phosphoric acid and causes the formation of disodium hydrogen phosphate. • H3PO4 + Na2CO3 Na2HPO4 + CO2 + H2O • The solution is neutralized, conc. and crystals are separated ,wash and dried.
• Calcium phosphate which is treated with sulphuric Acid, yields calcium sulphate and monobasic calcium phosphate. • Ca3 (PO4)2 + 2H2SO4 Ca(H2PO4)2 + 2CaSO4 • Now the filtrate is treated with sodium carbonate when dibasic calcium phosphate gets deposited leaving sodium phosphate in solution. • Ca(H2PO4)2 + Na2CO3 CaHPO4 + Na2HPO4 + CO2 + H2O
• Properties: It occurs in the form of colourless transparent crystals. • It is odourless and it is soluble in water and insoluble in alcohol. On heating over 300° it is converted into sodium pyrophosphate. • Reaction: Its 2 % solution has pH between 9 to 12. • Tests for purity: It is tested for alkalinity, As, Ca, Mg, Heavy metals, chloride, sulphate and LOD. • Heavy metals: It should not be more than 10 parts per million. • For calcium, magnesium: 2g substance + 50 ml water + 3 ml dilute ammonia solution = No turbidity should get produced. • Loss on dry: It should be between 57 % and 61%. It is determined on 0.5 g by drying in an oven at 130 ° c
• Assay Method: 1. 4 g of the sample is put in 25 ml of HCL and then diluted to 100 ml with water. Now 10 ml of this solution is treated potentiometrically with 0.1 N Sodium hydroxide until pH 4.4 is reacted(n1 ml). To the titrated solution 4 g of sodium chloride is added. Now this titration is continued with 0.1 N sodium hydroxide pH 9.2 (n2 ml). • The % of sodium phosphate is determined from the expression 1420 (n2-n1) w (100 – d), where d is the % of LOD. • 2. The solution of the salt (6 g in 100 ml of water) is treated with 0.5 N H2SO4 using bromocresol green as a indicator to its green colour indicative of Ph 4.5 .The results may be expressed on the basis of the salt dried at 130 °c ; so it is neutralised to sodium acid phosphate. • Storage: It is stored in tightly closed containers. • Uses: It is used as a saline laxative. It is a cathartic and buffering agent ( pharmaceutical aid). • Dose: 2 to 16 g.

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Cathartics( Sodium Phosphate, Magnesium carbonate, Magnesium hydroxide, Magnesium sulphate).pptx

  • 2. Cathartics • Cathartics: These are those agents or drugs which bring about defection. They are beneficial in constipation. • Constipation: It is a condition when a person passes less than three bowel movement( defecation) in a week or has difficult. Defecation is the process of passing stool. It is mainly depends on peristaltic (bowel) movement i.e. movement of intestines. • It is occurs due to continuously ignoring the urge to defecate. • It can also be brought about by many factors like weakness of intestine, injury or use of certain drugs and diet etc. • In constipation faecal material becomes dry and hard.
  • 3. • Cathartics are present into two forms: • A) Laxative: These are mild acting cathartics, which are used to treat constipation. • B) Purgative: These are strong cathartics, which are basically used to remove faecal material. • Classification: • On the basis of their mechanism, they are classified as follow:- • Stimulants: These are the drugs or chemicals which act by local irritation on intestinal tract and bring about stimulation of peristaltic activity. Drug like: Senna, Podophyllum, Castor oil, Aloe. • Bulk purgatives: These are the agents which are able to increase bulk of intestinal content which further increases the bowel movement. • These are cellulose or non- digestable type of materials. Ex. Methyl cellulose, Sodium Carboxy methyl cellulose, gum, isapgol etc.
  • 4. • Lubricants: It cause smooth clearance of the fecal material. e.g. Liquid paraffin, glycerine, mineral oils etc. Saline cathartics: Saline cathartics, also known as osmotic laxatives, are a class of laxatives that work by drawing water into the intestines, thereby increasing the volume of intestinal contents and stimulating bowel movements. These act by increasing the osmotic load of intestine by absorbing large quantity of water and thereby stimulate peristalsis. Poorly absorbable cations like calcium, magnesium and anions like phosphate, sulphate. These cathartics are taken in the form of suspension, tablet or in other suitable formulations. Saline laxative and cathartic agents are different magnesium salts such as magnesium hydroxide, magnesium sulphate, etc.
  • 5. Magnesium sulphate • It is also known as Epsom salt. • Chemical formula: Mgso4. 7H2O • Molecular Weight: 246.47 g/mol • Method of preparation: 1. It is obtained by the action of dilute sulphuric acid on magnesium carbonate or magnesium oxide or from native carbonate. • MgCO3 + H2SO4 MgSO4 + H2O + CO2 • The solution is filtered and filtrate is evaporated to crystallisation. • 2. It is manufactured by the action of sulphuric acid on the native carbonate or dolomite(rich in MgCO3). • When dolomite is used, magnesium sulphate passes into solution, sparingly soluble calcium sulphate gets deposited.
  • 6. • MgCO3 . CaCO3 + 2H2SO4 MgSO4 + CaSO4 + 2CO2 + 2H2O • The liquid is filtered and evaporated to crystallization. • 3. Magnesium salt occurring in brine which is used for the extraction of bromine. The liquors after removal of bromine are treated with milk of lime, thus ppt. out magnesium salt as magnesium hydroxide. • Sulphur dioxide and air are passed through the suspension of magnesium hydroxide. • 2Mg(OH)2 + 2SO2 + O2 2MgSO4 + 2H2O • On crystallization, crystals of MgSO4 , 7H2O are obtained.
  • 7. • Properties: It occurs as colourless crystals having a cool, saline bitter taste. It is soluble in water and sparingly soluble in alcohol. • Identification: It gives reactions which are characteristic of magnesium and sulphate • Tests for purity: It has to be tested for As, Fe, Zn, Heavy metals and loss on drying. • Clarity and colour of solution: 5 g of magnesium sulphate is dissolved in sufficient water to produce 50 ml. It should give a clear and colourless solution. • Acidity or alkalinity: 1 g of magnesium sulphate is dissolved in 10 ml of water. This solution is neutral to litmus solution. • Assay: 0.3 g of the sample weighed accurately. It is dissolved in 50 ml of water. To it 10 ml of strong ammonia ammonium chloride solution is added. Now this solution is titrated with 0.05 M disodium ethylenediaminetetraacetate using 0.1 g of Mordant Black 11 mixture as indicator until the pink colour gets discharged from the blue.
  • 8. • Storage: It is kept in tightly closed-container. • Action and uses: Magnesium sulphate is given orally in dilute solutions. About 5 g gives rise to laxative effect. • Due to bitter and nauseating taste it is given in fruit juices. • The mechanism of action is that magnesium sulphate does not get absorbed from intestinal tract and thus retains sufficient water within the lumen and hydrostatic pressor is able to promote motor activity. • Usual dose is 10-15 g.
  • 9. Magnesium hydroxide • Formula : Mg(OH)2 • Mol. wt. : 58.32g/mol • It is having not less than 95% and not more than 100.5 % Mg(OH)2. • Preparation: The magnesium hydroxide obtained in the preparation of milk of magnesia is evaporated to dryness. It is also prepared by treating sea water or other natural brines with sufficient calcium hydroxide to ppt. magnesium as magnesium hydroxide, then washing and drying the ppt. • Properties: It is a white fine amorphous powder. It is almost insoluble in water and slightly in alkaline. It dissolves in dilute mineral acids.
  • 10. • Assay: An accurately weighed amount of sample is taken in a flask. To it 25 ml of 1 N H2SO4 is added. Now the excess of acid is back titrated with 1 N NaOH using methyl red as an indicator. • Each ml of 1 N H2SO4 = 0.02917 g of MG (OH)2 • Uses: It is used as an antacid. In larger doses (2-4g) this acts as cathartic.
  • 11. Magnesium carbonate • Magnesium carbonate Molecular mass is 84.31 g/mol. • Carbonate having an approximate chemical composition 3 MgCO3. Mg (OH)2 . 5H2O. • It contains the equivalent of not less than 40% and not more than 45% of MgO. • Heavy magnesium carbonate is different from light magnesium carbonate in density. 15g of heavy magnesium carbonate occupies a volume of 30 ml while light magnesium carbonate occupies a volume of 125 ml. • Preparation: Magnesium sulphate (125 Parts) and sodium carbonate (150 parts) are dissolved separately in water and the solutions are mixed (1:1 ratio) . The residue is digested with boiling water for 30 minutes with water and the insoluble magnesium carbonate is filtered on calico cloth, washed until it becomes free from sulphate ions and dried in an oven. MgSO4 + Na2CO3 MgCO3 + Na2SO4 • Properties: It is a white granular powder, odourless and tasteless. It is insoluble in water and alcohol.
  • 12. • Tests for purity: It has to be tested for As, Ca, Fe, Copper, chloride, sulphate and soluble matter. • Residue on ignition: Residue should not be less than 42% and not more than 45%. • Tests for soluble matter: 1 gm heavy magnesium carbonate + 50 ml water , boiled for 5 minutes, then filtered and finally dried to constant weight at 105 ° c. The residue weighs not more than 10 mg. • Assay: 1 g sample is dissolved in sufficient quantity of dilute hydrochloric acid and the volume is made to 250 ml with the help of water. To 50 ml of this solution, add 100 ml of water and 15 ml of NaOH solution. After addition of 40 mg of murexide indicator and 3 ml of naphthol green, titrate with 0.05 M disodium EDTA until deep blue colour develops. • Uses: It is used as an antacid in the dose range of 500 mg to 2 g four times a day as a laxative in the dosage range of 2-4 g.
  • 13. Sodium Phosphate • It is also known as Disodium hydrogen phosphate • Chemical formula: Na2HPO4 . 12H2O • Molecular weight: 358.14 g/mol. • It contains not less than 98.5 % and not more than 101.0% of Na2HPO4 which is calculated with reference to the substance dried at 130°. • Preparation: Adding sodium carbonate to a hot solution of phosphoric acid. Sodium carbonate fails to affect the third hydrogen of phosphoric acid and causes the formation of disodium hydrogen phosphate. • H3PO4 + Na2CO3 Na2HPO4 + CO2 + H2O • The solution is neutralized, conc. and crystals are separated ,wash and dried.
  • 14. • Calcium phosphate which is treated with sulphuric Acid, yields calcium sulphate and monobasic calcium phosphate. • Ca3 (PO4)2 + 2H2SO4 Ca(H2PO4)2 + 2CaSO4 • Now the filtrate is treated with sodium carbonate when dibasic calcium phosphate gets deposited leaving sodium phosphate in solution. • Ca(H2PO4)2 + Na2CO3 CaHPO4 + Na2HPO4 + CO2 + H2O
  • 15. • Properties: It occurs in the form of colourless transparent crystals. • It is odourless and it is soluble in water and insoluble in alcohol. On heating over 300° it is converted into sodium pyrophosphate. • Reaction: Its 2 % solution has pH between 9 to 12. • Tests for purity: It is tested for alkalinity, As, Ca, Mg, Heavy metals, chloride, sulphate and LOD. • Heavy metals: It should not be more than 10 parts per million. • For calcium, magnesium: 2g substance + 50 ml water + 3 ml dilute ammonia solution = No turbidity should get produced. • Loss on dry: It should be between 57 % and 61%. It is determined on 0.5 g by drying in an oven at 130 ° c
  • 16. • Assay Method: 1. 4 g of the sample is put in 25 ml of HCL and then diluted to 100 ml with water. Now 10 ml of this solution is treated potentiometrically with 0.1 N Sodium hydroxide until pH 4.4 is reacted(n1 ml). To the titrated solution 4 g of sodium chloride is added. Now this titration is continued with 0.1 N sodium hydroxide pH 9.2 (n2 ml). • The % of sodium phosphate is determined from the expression 1420 (n2-n1) w (100 – d), where d is the % of LOD. • 2. The solution of the salt (6 g in 100 ml of water) is treated with 0.5 N H2SO4 using bromocresol green as a indicator to its green colour indicative of Ph 4.5 .The results may be expressed on the basis of the salt dried at 130 °c ; so it is neutralised to sodium acid phosphate. • Storage: It is stored in tightly closed containers. • Uses: It is used as a saline laxative. It is a cathartic and buffering agent ( pharmaceutical aid). • Dose: 2 to 16 g.