Expectorants & emetics

Slides:



Advertisements
Similar presentations
Biochemical Tests By Cheryl Kent.
Advertisements

Chapter 19 - Neutralization
Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer’s Law Chapter
Fluid and Electrolyte Therapy. Introduction: The molecules of chemical compounds in solution may remain intact, or they may dissociate into particles.
Acids, Bases and Salts Mrs Teocc.
Reactions in Aqueous Solutions
Extraction Lab # 6.
Testing for Cations and Anions Determine the presence of a cation or anion by a chemical reaction Determine the identity of cations and anions in an unknown.
Element Elements and Compounds Compounds of Sodium Structure of Atom Compounds A compound is a substance composed of two or more elements, chemically combined.
REFER TEXT BOOK : PAGE 138 EXAMPLE : Metal ions Ammonium ion replace Ammonium chloride Sodium chloride.
Volumetric Analysis Concentration of Solutions. Remember: Solution – A mixture of a solute and a solvent Solvent – The liquid in which the solute is dissolved.
Introduction The Equipment The Process Calculations
Unit 6 – Acids and Bases.  Indicators are dyes that change colour under varying conditions of acidity.  Although not as accurate as instruments such.
 All salts are ionic compounds.  A salt is formed when a metallic ion or an ammonium ion (NH 4 + ) replaces one or more hydrogen ions of an acid. HClNaCl.
Acids, Alkalis and Indicators Prepared by Mdm RY Leow The Chinese High School.
Lipids.
Making Salts Soluble salt Insoluble salt Acid + excess insoluble solid
Salt soluble? yes, then choose an acid and a base base soluble? yestitrationno excess base no precipitation choose two soluble salts.
Ch. 16: Ionic Equilibria Buffer Solution An acid/base equilibrium system that is capable of maintaining a relatively constant pH even if a small amount.
Ammonia (NH3) Metal oxides Metal hydroxides
Maintaining Water-Salt/Acid-Base Balances and The Effects of Hormones
Acids and Alkalis Learning Objectives To know that solutions can be sorted by whether they are: acid, alkali or neutral. To understand that an alkali reacts.
Acids and Bases. Acids are substances that turn blue litmus red, and usually react with metals such as zinc, releasing hydrogen. Examples: hydrochloric.
Aqueous Solutions. Soluble and Insoluble Soluble generally means that more than 1 g of solute will dissolve in 100 mL of water at room temperature. Insoluble.
Chemistry 101 : Chap. 4 Aqueous Reactions and Solution Stoichiometry (1) General Properties of Aqueous Solutions (2) Precipitation Reactions (3) Acid-Base.
1 Types of Chemical Reactions and Solution Stoichiometry Chapter 4.
Solutions. Definitions Solution: homogeneous mixture of 2 or more substances in a single physical state Solute: the substance dissolved in the solution.
Anatomy & Physiology Tri-State Business Institute Micheal H. McCabe, EMT-P.
Prepared by PhD Halina Falfushynska 1 Lecture 7. Electrolytes. Reactions in Aqueous Solutions.
Soluble or Insoluble: General Solubility Guidelines Many factors affect solubility so predicting solubility is neither straightforward nor simple. The.
Acids and Bases.
Ch. 18: Acids & Bases Sec. 18.4: Neutralization.
19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day The pH for a 0.10 M solution of a.
Types of Reactions. In Chemistry, we can identify a lot of different types of chemical reactions. We can put these chemical reactions into groups, so.
ACIDS AND BASES Questions may involve any of the following: description of acids and bases in terms of proton transfer calculations involving K w and pH.
2.3 Solutions. Objectives 9. Define solution, solute, solvent, and concentration 10. Explain the dissociation of water 11. Contrast properties of acids.
Volumetric Analysis – Titrations Volumetric Analysis a process of analysis accomplished by adding together particular volumes of 2 solutions the objective.
Buffers. Buffer Capacity A buffer solution has limited ability to react with acids and bases without changing it is pH, a solution acts as a buffer because.
Water: removing dissolved solutes Chapter 12. Precipitation Reactions When two solutions are mixed, an insoluble compound sometimes forms. When two solutions.
Aqueous Reactions and Solution Stoichiometry
Salts.
Solutions and Acids and Bases. Matter synthesis.com/webbook/31_matter/matter2.jpg.
1 Chapter 20Neutralization and Salts 20.1Neutralization 20.2Practical applications of neutralization 20.3Salts of some common acids 20.4Water of crystallization.
iGCSE chemistry Section 4 lesson 1
Analysis of aspirin Tablet
You’ll find out what buffer solutions are and how they are prepared. Buffer Solutions Definition and Preparation.
The Solution Process Electrolytes, non-electrolytes.
Dr. Rida Shabbir DPT –IPMR (KMU). Acid Base Balance Acid: is any chemical that releases H ion in solution. Strong acid: Ionizes freely, gives up most.
AS Revision Lessons Identification tests.
I. pH of Body Fluids water ionizes to form protons (H + ) and proton acceptors (OH - ) A. Remember that to an extent water ionizes to form protons (H.
Solutions Chemistry. Solution = homogeneous mixtures made up of individual particles (molecules, atoms or ions). 1.May include combinations of phases.
Antioxidants. Anti-oxidant “ They are the reducing agents which are added to the drugs or other pharmaceuticals to prevent their oxidation through oxidative.
Maintaining Water-Salt/Acid-Base Balances and The Effects of Hormones
Experiment two The identification and the assay of Ammonium Chloride
Acids and Alkalis.
Acids and Alkalis Grade 10.
Pharmaceutical Technology
Pharmaceutical Technology
By: S iju Prakash Asst. Professor. Emetics These are the drugs which give rise to forced emesis by which the contents of the stomach get expelled through.
Pharmaceutical Chemistry ( Inorganic Chemistry).  Pharmaceutical chemistry is a science that makes use of the general laws of chemistry to study drugs.
Expectorants Dr. M.Y. Ansari.
Emetics Agents that induce vomiting Used in overdoses Example
Determination of Cu in Brass
Expectorants.
What is the function of Antacids ? These are drugs which are usually alkaline substances Used for neutralizing excess acid in the stomach Helps patients.
PRACTICAL METHODS FOR MAKING SALTS: Learn THIS!
PRACTICAL METHODS FOR MAKING SALTS: Learn THIS!
Presentation transcript:

Expectorants & emetics

Expectorants “Drugs that help in removing sputum from the respiratory tract. -either by increasing the fluidity (or reducing the viscosity) of sputum or -increasing the volume of fluids that have to be expelled from the respiratory tract by coughing.”

Both the action and mechanism of expectorants have been questioned and remain controversial. However, these may serve a placebo role and help the patient Ammonium chloride Potassium iodide Sodium iodide .

Dose related side-effects If the patient is sensitive, dose of expectorant is high enough, this may induce vomiting (emetic action). Hence, it is advisable to give the doses of expectorants that could be tolerated (by the patient) along with other pharmaceutical aids (flavours, sweetners, etc.) and cough suppressants.

Classification of Expectorants According the their mechanism of action… (1) Sedative type (2) Stimulant type

Sedative expectorants These are stomach irritant expectorants which are able to produce their effect through stimulation of gastric reflexes. e.g. Bitter drugs – Ipecac, Senega, Indian Squill Compounds – Antimony potassium tartrate, Ammonium chloride, Sodium citrate, Potassium iodide, etc.

Stimulant type These are the expectorants which bring about a stimulation of the secretory cells of the respiratory tract directly or indirectly. Since these drugs stimulate secretion, more fluid in respiratory tract and sputum is diluted. e.g. - Eucalyptus, lemon, anise - Active constituents of oil like terpine hydrate, anethole

Emetics These are the drugs which give rise to forced regurgitation (emesis) by which the contents of the stomach get expelled through the oral cavity. They are very important in cases of poisoning.

Mechanism of action The emetics act by.. - either by local irritation of gastric mucosa. e.g. Ammonium bicarbonate, ipecacuanha - or directly on the chemoreceptor trigger zone (i.e. centrally acting emetics).

Although vomiting is primarily considered to be a respiratory function, its ultimate result would cause the evacuation of the stomach. Emetics are sometimes added to cough preparations in low doses to stimulate flow of respiratory tract secretions.

Clinical facts… There are certain types of poisoning in which the toxic substances themselves may be able to induce emesis by reflex action. There are some types of poisoning in which poisons may remain in stomach for sometime before entering intestine where they may get absorbed. Before this occurs, emetics are given to patients for physically expelling the toxic substances and reduce the harmful effects and may be able to save patient’s life. When a patient is in unconscious state, emetics may not be very useful and gastric lavage may be required.

2NaCl + (NH4)2SO4  2NH3 + HCl + Na2SO4 Ammonium chloride Molecular formula: NH4Cl Preparation: (i) Commercially, it is prepared by neutralising NH3 with HCl. NH3 + HCl  NH4Cl (ii) It is produced by heating ammonium sulphate with NaCl 2NaCl + (NH4)2SO4  2NH3 + HCl + Na2SO4

Ammonium chloride Properties: - White coloured fine or coarse crystalline powder - Cooling saline taste - Slightly hygroscopic - Partialy soluble in mixture of water & alcohol - Freely soluble in glycerine - 0.8% w/v of NH4Cl is isotonic with serum. - Freshly prepared aqueous solutions are neutral to litmus but become quickly acidic on standing because of hydrolysis.

Ammonium chloride Assay: It was previously assayed by precipitation titration by using the Volhard’s method. Now, it is assayed by acid-base titration method. Uses: (1) It acts as mild expectorant and diaphoretic when administered in small doses. It does so due to local irritation which produces increasing secretion of respiratory tract, and makes the mucus less viscous. NH4Cl and NH4HCO3 are therefore used in cough preparations.

Ammonium chloride (2) It acts in maintaining acid-base equilibrium of body fluids. (3) It is also used as diuretic in combination with mercurial compounds. The diuretic effect is because of utilization of NH4+ cation in conversion into urea and in the process portion H+ and Cl- ions are formed. The H+ ion reacts with bicarbonate and CO2 and water is produced. On continue use, it increases acidity of urine and metabolic acidosis is produced. Thus, it can be useful in some cases of systemic alkalosis.

Ammonium chloride Dose: As systemic acidifier : 1-2 g four times a day As expectorant : 0.3-0.5 g Storage: It is stored in tightly closed container

Antimony potassium tartrate Synonym: Tarter emetic Molecular formula: C4H4KO7Sb Structural formula: KOOC-CHOH-CHOH-COO(SbO) Properties: - Colourless crystals - Odourless - Sweetish taste - On exposure to air, crystals effloresce - Solubility : 1 in 12 (Water at 25°C) - Insoluble in alcohol and soluble in glycerin

Antimony potassium tartrate Preparation: It is obtained by mixing 5 parts of antimony trioxide (Sb2O3) with 6 parts of potassium acid tartrate in a fine paste. Keep this paste aside for a day. Boil it with water for 15 minutes with constant stirring. The liquid is then filtered and left for crystallization 2KHC4H6O6 + Sb2O3  2K(SbO)C4H4O6 + H2O

Antimony potassium tartrate Assay: Iodimetric titration using starch indicator Uses: - As an expectorant and emetic (hence named- ‘tartar emetic’) - The emetic action is because of irritant action on the gastric mucosa. The emetic action has slow onset and marked depression can follow. - It can also be used to treat schistosmiosis (drug of choice in infections produced by Schistosoma japonicum).

Copper sulphate Synonym: Cupric sulphate, Blue vitriol Molecular formula: CuSO4.5H2O Molecular weight: 249.7 Preparation: 2Cu + 2H2SO4 + O2  CuSO4 + H2O Assay: - Iodometric titration (oxidation-reduction method)

Copper sulphate Burette : 0.1N Na2S2O3 solution Iodine flask : 5 ml of CuSO4 (sample soln) + 5 ml of CH3COOH + 5 ml of KI + 10 ml of distilled water + 0.5 ml of starch mucilage + 5 ml of KCNS Indicator : Starch mucilage End-point : Brown – yellow – blue - colourless

Copper sulphate Uses: - As an emetic (in dose of 300mg in 30ml of H2O). However, its use as an emetic can be dangerous because of large and corrosive doses. - As chemical antidote in phosphorus poisoning. - As an astringent and also as a fungicide (1.5% solution). - It is an ingredient of Benedict’s reagent and Fehling’s reagent.