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Non-aqueous acid base titrimetry
Non-aqueous acid-base titrimetry involves titrating weakly acidic or basic substances in non-aqueous solvents to achieve sharp endpoints, addressing solubility and interaction issues seen in aqueous titrations. Various types of non-aqueous solvents are used, including protophilic and protogenic, with specific indicators and titrants tailored for weak acids and bases. Advantages include better solubility for organic acids/bases and selectivity in titration, while disadvantages encompass costs and environmental concerns.
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Non-aqueous acid base titrimetry
- 1. Non-aqueous acid basetitrimetry Md : Obydulla Al Mamun Id:131-29-500 9th(B) Department Of Pharmacy Daffodil International University almamundcc94@gmail.com
- 2. Non-aqueous acid basetitrimetry Non- aqueous titrations are those in which the titrations of too weakly acidic or basic substances are carried out using non-aqueous solvents so as to get sharp end point. Such titrations can also be used for the titration of the substances not soluble in water. The speed, precision and accuracy of the non- aqueous method are close to those of classical acidimetric and alkalimetric titrations.
- 3. REASONS FOR PERFORMINGNON – AQUEOUS ACID – BASE TITRATION Non – aqueous Acid – Base Titration is performed to eliminate 2 problems encountered during the aqueous titration of weakly acidic or weakly basic analyte by a Strong Acid or Strong Base Titrant respectively. The 2 problems are – Interaction of the Titrant with H2O Poor Solubility of Weakly Acidic (WA) or Weakly Basic (WB) Analyte in H2O
- 4. ACIDS & BASES Acids: Arrhenius acid: Any substance that, when dissolved in water, increases the concentration of hydronium ion (H3O+) Bronsted-Lowry acid: A proton donor conjugate base Lewis acid: An electron acceptor Bases: Arrhenius base: Any substance that, when dissolved in water, increases the concentration of hydroxide ion (OH-) Bronsted-Lowery base: A proton acceptor conjugate acid Lewis acid: An electron donor
- 5. Solvents Non-aqueous solvents areclassified into the 4 groups: - Protophilic solvents - Protogenic solvents - Amphiprotic solvents - Aprotic solvents
- 6. Protophilic solvents Possess highaffinity for proton Weak acids are normally used as solute Strong protophilic solvents convert weak acid to strong acid-known as ’leveling effect’ Example: Liquid ammonia, amines, ether and ketones HA + S SH+ + A- Weak Acid (appeared as strong acid) Basic solvent Solvated proton Conjugated base of acid
- 7. Protogenic solvents Acidic innature Readily donates protons Strong protogenic solvents increase the strength of weak bases Such solvents exert a leveling effect on all bases dissolved in them Example: Anhydrous acid like hydrogen fluoride & sulfuric acid B + H+ BH+ Weak Base (appeared as strong base) From solvent Conjugated acid of base
- 8. Amphiprotic solvents Combine protogenicand protophilic properties of solvent Able to both donate and accept proton Example: Water, alcohol & weak organic acid Acetic acid shows acidic property by releasing proton- CH3COOH CH3COO- + H+ In presence of perchloric acid (strong acid) acetic acid shows basic property by accepting proton and produce ‘onium’ ion- CH3COOH + HClO4 CH3COOH2 + + ClO4 - ‘onium’ ion
- 9. APROTIC SOLVENTS Chemicallyneutral substances Virtually un-reactive Do not cause ionization of solute No reactions with acids and bases Used to dilute reaction mixture Example: Carbon tetrachloride, benzene, tolune.
- 10. NON AQUEOUS TITRATIONOF WEAK ACIDS Many weakly acidic substances (aicohol or aprotic solvent)can be titrated in an appropiate non aqueous solvents with a sharp end point . Ex:- acidic halides, acids,amino acids, enols(barbiturates,xanthines), phenols, pyrroles sulphonamides etc,. 1) Solvents used in the titration of weak acids: Ex:-Ethylenediamine,n-butylamine,morpholine 2) Titrant used in the titration of weak acids: Ex:-sodium methoxide, lithium methoxide, potasium methoxide ,tetrabutyl ammonium hydroxide etc. 3) Indicatores used in the titration of weak acids Ex:-azo violet.thymol blue,thymolphthalein.,O-Nitro aniline
- 11. NON AQUEOUS TITRATIONOF WEAK BASES Solvents used in the titration of weak bases; Neutral solvents : Ex: - alcohol,chloroform,benzene,chlorobenzene Acidic solvents: Ex:-formic acid,glacial acetic acid,propionic acids Titrant used in the titration of weak basess: Ex:-Perchloric acid Indicatores used in the titration of weak bases Ex:-oracat blue ,crystal violet,naphtholbenzein(weak bases)
- 12. BASIS OF INDICATORSELECTION Indicator colour change, from acid to alkali pKind pH range example of titration use Methyl orange, (red ==> yellow) 3.7 3.1-4.4 weak base - strong acid titration e.g. ammonia titrated with hydrochloric acid Bromophenol blue, (yellow ==> blue) 4.0 2.8-4.6 weak base - strong acid titration Methyl red, (red ==> yellow) 5.1 4.2-6.3 weak base - strong acid titration Bromothymol blue, (yellow ==> blue) 7.0 6.0-7.6 strong acid - strong base titration e.g. hydrochloric acid <=> sodium hydroxide titration Phenol red, (yellow ==> red) 7.9 6.8-8.4 strong acid - strong base titration e.g. hydrochloric acid <=> sodium hydroxide titration Thymol blue (base form), (yellow ==> blue) 8.9 8.0-9.6 weak/strong acid - strong base titration Phenolphthalein, (colourless ==> pinky-red) 9.3 8.3- 10.0 weak acid - strong base titration e.g. ethanoic acid titrated with sodium hydroxide
- 13. Preparation of a0.1 N solution: When metal has dissolved, have to add sufficient methanol until clear solution Then add dry benzene slowly with continuous shaking until the solution appears cloudy Repeat the addition of methanol followed by benzene until 1 liter clear solution has been prepared. Mixture of 40 ml methanol and 50 ml dry benzene in Erlenmeyer flask Add 4 gm of K or 2.3 gm of Na or 0.6 gm of Li to the flask (the metal should be freshly cut and have to add slowly)
- 14. 1. Minimum amountof methanol have to use to ensure clear solution. 2. Have to store in sodium free glass. 3.Have to protect it from atmospheric CO2. Precaution: Titrants are usually standardized by using reference standard- benzoic acid. 0.5% thymol blue in anhydrous methanol used as indicator. Dimethylformamide used as solvent for the titration. Standardization:
- 15. ADVANTAGES OF NONAQUEOUS SOLVENT OVER AQUEOUS SOLVENT: 1) Organic acids and bases that are insoluble in water are soluble in non-aqueous solvent. 2) Organic acid, which is of comparable strength to water, can be titrated easily in non-aqueoussolvent. Bases also follow the same rules. 3) A non-aqueous solvent may help two are more acids in mixture. The individual acid can giveseparate end point in different solvent. 4) By the proper choice of the solvents or indicator, the biological ingredients of a substance whether acidic or basic can be selectively titrated. 5) Non aqueous titrations are simple and accurate, examples of non aqueous titration are:Ephedrine preparations, codeine phosphate in APC, tetracycline, teramycin, Antihistamines andvarious piprazine preparations
- 16. DISADVANTAGES NON-AQUEOUS ACIDBASE TITRATION Temperature ,moisture,co2 should be control. Solvents are expensive. Volatile solvents can polute environment Indicator must be prepare in non aquous medium.