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PHARMACEUTICAL INORGANIC CHEMISTRY LAB (1ST SEMESTER)


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Dwight Obillos


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[Front]


Acids on the skin
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Wash the affected area immediately with plenty of water, then with saturated SODIUM BICARBONATE SOLUTION and again with water

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PHARMACEUTICAL INORGANIC CHEMISTRY LAB (1ST SEMESTER) - Details

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Acids on the skin
Wash the affected area immediately with plenty of water, then with saturated SODIUM BICARBONATE SOLUTION and again with water
A. Safety Rules: Protecting yourself in the Laboratory
1. The laboratory is a place for serious work. DO NOT ATTEMPT ANY UNAUTHORIZED EXPERIMENTATION. 2. Report all injuries- no matter how minor- to your instructor immediately. 3. Beware of hot glass. Glass cools very slowly and may be very hot without appearing so. Immediately hold the injured area under cold water or cover it with ice. 4. Do not point the test tube at the student before you or yourself when heating substances. Bubbles of vapor that form suddenly may expel the contents violently. 5. When diluting sulfuric acid, pour the acid slowly and carefully into the water, stirring constantly. NEVER ADD WATER TO ACIDS. Remember the AA rule: Add acid to water.
Burns by dry heat
Apply BUTESIN PICRATE ointment or any burn ointment available in the first-aid kit in the laboratory
Alkali on the skin
Wash the affected area immediately with plenty of water, then with 1% ACETIC ACID solution and again with water.
Bromine on the skin
Wash the affected part immediately with plenty of LIGHT PETROLEUM (B.P. 80˚ C) and then rub GLYCERIN well onto the skin. After a short while, remove the glycerin and apply BUTESIN PICRATE ointment or any burn ointment in the first-aid kit.
Sodium on the skin
If a small fragment of sodium metal can still be seen, remove it carefully with a forceps. Wash thoroughly with water; followed with 1% ACETIC ACID solution. Cover the area with GAUZE COVERED IN OLIVE OIL or ACRIFLAVINE JELLY or VASELINE.
Organic substances on the skin.
Wash freely with RUBBING ALCOHOL, then with SOAP and WATER.
Cuts
If the cut is minor, allow it to bleed for a few seconds. If the cut is caused by a glass, see to it that no glass pieces remain. Apply a DISINFECTANT and BANDAGE. For serious cuts, check bleeding by applying pressure above it (a tourniquet) . Send for a doctor at once.
Eye Accidents: Acid in the eyes
Wash the eye/s repeatedly with 1% SODIUM BICARBONATE solution. If the acid is concentrated, wash the eye/s with large amount of water and then with BICARBONATE solution.
Eye Accidents: Caustic Alkali in the eyes
Wash the eye/s with large amount of water and then with 1% BORIC ACID solution.
Eye Accidents: Bromine water in the eyes
Wash thoroughly with 1% SODIUM BICARBONATE solution.
Fires
When clothes catch fire, prevent the person from running. Let him/her roll on the floor or wrap another piece of clothing around him (a laboratory gown or blanket) to cut off the supply of oxygen. When chemicals in beakers and other containers burn, cover the mouth of the vessel with a clean damp cloth so that the flame will be put off. For larger flames, sand may be employed. It is advisable to make use of a fire extinguisher. DO NOT USE WATER.
Poisons: Acid
If an acid is swallowed, dilute by drinking plenty of water followed by LIMEWATER or MILK OF MAGNESIA. MILK may also be given. DO NOT GIVE ANY EMETIC.
Poisons: Caustic Alkali
Dilute by drinking plenty of water, followed by VINEGAR, LEMON or ORANGE JUICE. MILK may also be given. DO NOT GIVE ANY EMETIC.
Poisons: Salts of Heavy Metals
If a salt of heavy metal is swallowed, one may give MILK or RAW EGG WHITE.
Poisons: Arsenic or Mercury Compounds
Give an emetic immediately such as one tablespoonful of SALT or ZINC SULFATE in a glass of warm water.
Hydrogen peroxide reaction with Barium Hydroxide
H2O2 + Ba(OH)2 → BaO2 + 2H2O precipitate - Barium Peroxide (BaO2)
Hydrogen peroxide reaction with Potassium Dichromate and Sulfuric Acid
K2Cr2O7 + 4H2SO4 + 3H2O2 → Cr2(SO4)3 + 3O2 + K2SO4 + 7H2O Produces Deep blue color - chromium (III) ions Chromium (III) Sulfate - Precipitate
Stabilizers:
• Colloidal stannate • Sodium pyrophosphate • Organophosphonates • Nitrate (for pH adjustment and corrosion inhibition) • Phosphoric acid (for pH adjustment) • Colloidal silicate (to minimize H2O2 decomposition in certain applications)
Why is adding stabilizers important in hydrogen peroxide?
Minimize its decomposition under normal storage and handling conditions.
Uses of Hydrogen Peroxide
1 Hair bleaching 2 Antiseptic 3 Mild disinfectant
Potassium Acetate Physical Appearance
Faint Acetic Smell White color Crystalline powder
Potassium Acetate reaction with Acetic Acid
CH3COOH(aq) ←→ CH3COO-(aq) + H+(aq) No reaction, buffer solution is formed
Potassium Acetate reaction with Sulfuric Acid and Ethyl Alcohol
CH3COOK + H2SO4 →CH3COOH + KHSO4 (first reaction) forms acetic acid CH3COOH + C2H5OH → CH3COOC2H5 + H2O (second reaction) acetic acid reacts with ethyl alcohol yielding ethyl acetate Ethyl acetate - fruity odor
Potassium Acetate reaction with Ferric Chloride T.S.
FeCl3 + 3CH3COOK → (CH3COO)3Fe + 3KCl forms Iron (III) acetate and Potassium chloride
Uses of potassium acetate
1 Supplement 2 Preservative and acidity regulator 3 Electrolyte replenisher
Ammonium Bromide Physical Appearance
Color: white Odor: odorless Taste: saline taste Physical state: solid Appearance: crystallized
Ammonium Bromide reaction with Sodium Hydroxide
NH4Br + NaOH → NaBr + NH3 + H2O Produces sodium bromide, ammonia and water Ammonia-like odor
Ammonium Bromide reaction with Silver Nitrate
NH4Br + AgNO3 → AgBr + NH4NO3 Produces silver bromide and ammonium nitrate Silver bromide - Precipitate Orange-brown coloration (Br) - Color
Ammonium Bromide reaction with Chlorine
NH4Br + Cl → NH4Cl + Br produces ammonium chloride and bromine orange-brown color solution
Uses of Ammonium Bromide
1 Sedative 2 Anticonvulsants 3 Photography in films (not therapeutic)
Calcium Carbonate Physical Appearance
White color Odorless powder / Colorless crystals Bitter taste Powder
Calcium Carbonate reaction with Acetic Acid
2CH3COOH + CaCO3 → H2CO3 + Ca(CH3COO)2 (first reaction) Produces Calcium acetate H2CO3 → H2O + CO2 (second reaction) Breaking down of Carbonic Acid to form Water and Carbon Dioxide
Calcium Carbonate reaction with Ammonium Oxalate
CaCO3 + (NH4)2C2O4 → (NH4)2CO3 + CaC2O4 Produces white precipitate - Oxalate Calcium Oxalate (CaC2O4) - Precipitate
Flame Test
Brick Red - color produced by Calcium Intense Yellow - Sodium Carmine Red - Lithium Crimson Red - Strontium
Uses of Calcium Carbonate (pharmaceutical)
1 Antacid 2 Dietary Calcium Supplement 3 Phosphate binder 4 Base material for tablets
Different forms of Calcium Carbonate
1 Calcite 2 Aragonite 3 Vaterite
Magnesium Hydroxide reaction with Sodium Phosphate
Mg(OH2) + Na3PO4 → Mg3(PO4) + NaOH Magnesium Phosphate - Precipitate Sodium Hydroxide - Liquid
Magnesium hydroxide reaction with Ammonium Carbonate
(NH4)2CO3 + Mg(OH)2 → MgCO3 + 2NH3 + 2H2O Magnesium Carbonate - Precipitate Ammonium - Gas
Magnesium Hydroxide in liquid form
Milk of Magnesia / Magnesia Magma
Magnesium Hydroxide Physical Appearance
Color: White Physical state: odorless white solid Appearance: White solid
A strong electrolyte
Magnesium Hydroxide
Common names of Copper Sulfate
1 Blue Vitriol 2 Blue Stone
Copper Sulfate Physical Appearance
Blue Odorless Metallic Solid Crystallized
Copper Sulfate reaction with Potassium Ferrocyanide
2Cu2+(aq)+[Fe(CN)6]4−(aq)↽⇀Cu2[Fe(CN)6](s) Produces 2 moles of Potassium Sulfate Brownish-red(copper ions) - Color of Precipitate Copper (II) Ferrocyanide - Precipitate
Copper Sulfate reaction with Ammonia T.S.
CuSo4 + 5NH3 ↽⇀ [Cu(NH3)5]SO4 forms copper hydroxide precipitate (Cu(OH)2) Deep blue - Color of the solution
Copper Sulfate reaction with Barium Chloride T.S.
CuSO4 + BaCl2 ↽⇀ BaSO4 + CuCl2 Barium Sulfate - Precipitate White - Color of Precipitate
Copper Sulfate reaction with Lead Acetate
Pb(CH3COO)2 + CuSO4 → PbSO4 + Cu(CH3COO)2 Produces copper acetate and lead sulfate Lead sulfate - Precipitate White - Color of Precipitate
Uses of Copper Sulfate
1 Germicide 2 Fungicide 3 Treatment of Swimming pools
Ahydrous form
White solid / greyish
Uses of Iodoform
1 Antiseptic 2 Disinfectant
Iodoform reaction with Ethanol and Potassium Carbonate
2C2H5OH+8I2+K2CO3+H20 → 2CHI3+2HCO2K+CO2+10HI Iodoform - Precipitate Pale white / pale yellow - Color of Iodoform
Color of Iodine solid
Brownish purple / Dark brown
Color when mixed
Brown or Yellow
Effervescent Preparations
Carbonate or Bicarbonate Organic Acids – Tartaric Acid, Citric Acid, Malic Acid, Ascorbic Acid
Also known as the Noble Gases
Group 0 elements Group VIII (8) in the periodic table
What is Helium used for and its container?
Used to prepare synthetic airs ( 20% O2 + 80% He) a. Carrier / diluent of medicinally important gases b. component of artificial gas Container: Brown
Toxicity of Helium
Donald Duck like sound if inhaled
Investigated for possible anesthetics
Krypton (Kr) and Xenon (Xe)
Synthetic Noble Gas
Radon (Rn) aka: niton
What is the use of Radon (Rn) ?
Used for treatment of Cervical Cancer
Isotopes of Hydrogen
Protium - Most abundant Deuterium - heavy hydrogen D2O - heavy water Tritium - radioactive powerful reducing agent pale blue flame
Earth Lightest metal
Lithium (Li) Bridge element of Mg
What is the use of Lithium (Non pcol) ?
Heat exchanger in air conditioners
What are the compounds of Lithium?
1 Lithium Bromide (LiBr) - Depressant sedative 2 Lithium Carbonate (Li2CO3) BN: 3 Lithase - Drug of choice for mania Side Effects: Ebstein anomaly (Congenital cardiac abnormalities) Flame Test - Carmine Red
Most abundant extracellular cation
Sodium (Na) Responsible for fluid retention "Natrium" - nature
Color of Sodium(Na) in flame test
Persistent golden yellow
Effervescent Preparations
Carbonate or Bicarbonate Organic Acids – Tartaric Acid, Citric Acid, Malic Acid, Ascorbic Acid
Ringer’s Solution
1 NaCl (Sodium chloride) 2 KCl (Potassium chlorid) 3 CaCl2 (Calciu chloride)
Bases/Alkaline causes
Liquefactive Necrosis (Lipids)
Acids causes
Coagulative Necrosis (Proteins)
Antidotes
Base – vinegar, fruit juices Acid – antacid For both: Dilution with water or milk Sulfuric Acid – Contraindicated with dilution of water (Exothermic reaction)
Antidote bases
Vinegar, fruit juices
Acid and bases is ingested
Dilute with water or milk
What are the uses of Potassium (K)?
For muscular contraction Diuretics
“Cream of Tartar or Creamor”
Potassium bitartrate (KHC4H4O6)