TITRATION

• Acid-base titration: Principle, Types, Applications and Procedure
• Advantages and disadvantages of acid-base titration
• Advantages and disadvantages of complexometric titration
• Advantages and disadvantages of gravimetric analysis method
• Advantages and disadvantages of non-aqueous titration
• Advantages and disadvantages of precipitation titration
• Assay of ammonium chloride
• Assay of borax
• Assay of boric acid
• Assay of calcium carbonate
• Assay of calcium gluconate
• Assay of calcium lactate
• Assay of ferrous sulphate
• Assay of hydrogen peroxide
• Assay of magnesium sulphate
• Assay of sodium benzoate
• Assay of sodium bicarbonate
• Assay of sodium chloride
• Bromothymol blue indicator in titration
• Buffer solution in EDTA complexometric titration
• Characteristics of a good primary standard
• Complexometric EDTA titration
• Complexometric titration procedure
• Conductometric titration of strong acid against strong base
• Conductometric titration of strong acid and weak acid against a strong base
• Definitions and basic terms used in titration
• Determination of acetic acid in vinegar
• Difference between acid-base titration and redox titration
• Difference between aqueous and non-aqueous titration
• Difference between back titration and direct titration
• Difference between coulometric and volumetric titration
• Difference between endpoint and equivalence point
• Difference between equivalence point and half equivalence point
• Difference between gravimetric and volumetric analysis
• Difference between internal and external indicator
• Difference between iodometric and iodimetric titration
• Difference between methyl red and methyl orange
• Difference between Mohr method and Volhard method
• Difference between phenolphthalein and methyl orange indicator
• Difference between primary and secondary standard solution
• Difference between standardization and titration
• Difference between titrant and titrand
• Difference between volumetric analysis and titration
• Endpoint and equivalence point in chemistry
• Endpoint in KMnO4 titration
• Eriochrome black T indicator in complexometric titration
• Estimation of hardness of water by EDTA method
• Fajan's method of precipitation titration
• How and where should NaOH solution be stored?
• How do acid-base indicators work?
• How do you measure permanent hardness by EDTA titration?
• How does back titration work?
• How does iodometric back titration work?
• How does starch work as an indicator?
• How does the bromothymol blue indicator work?
• How does the methyl orange indicator works?
• How does the phenolphthalein indicator work?
• How to find first and second equivalence points
• How to remove air bubbles from burette tip
• Identification test for barium sulphate
• Identification test for bentonite
• Identification test for borax
• Identification test for boric acid
• Identification test for hydrogen peroxide
• Identification test for iodine
• Identification test for magnesium sulphate
• Identification test for sodium chloride
• Identification test for sodium thiosulphate
• Identification test for zinc oxide
• Identification test for zinc sulphate
• Identification test of ammonium chloride
• Identification test of calcium gluconate
• Identification test of copper sulphate
• Identification test of ferrous sulphate
• Identification test of sodium bicarbonate
• Identification tests of magnesium hydroxide
• Importance of titration in chemistry
• Iodometric Titration: Principle, Example, Advantages, and How Does it Work
• Limit test for arsenic
• Limit test for chlorides for water insoluble substances
• Limit test for chlorides in sodium bicarbonate
• Limit test for heavy metals
• Limit test for Iron
• Limit test for lead
• Limit test for sulphate
• Methyl orange indicator in titration
• Methyl red indicator in titration
• Methyl red: Frequently Asked Questions
• Methyl yellow indicator in titration
• Modified limit test for chloride
• Modified limit test for sulphate
• pH range and color change of indicators used in titration
• Potentiometric titration of strong acid against strong base
• Preparation and standardization of 0.02 M mercuric nitrate
• Preparation and standardization of 0.05 M EDTA solution
• Preparation and standardization of 0.05 M magnesium sulphate
• Preparation and standardization of 0.1 M ceric ammonium sulphate
• Preparation and standardization of 0.1 M ferrous ammonium sulphate
• Preparation and standardization of 0.1 m H2SO4
• Preparation and standardization of 0.1 M lead nitrate
• Preparation and standardization of 0.1 m NaOH
• Preparation and standardization of 0.1 M oxalic acid
• Preparation and standardization of 0.1 M perchloric acid
• Preparation and standardization of 0.1 M potassium hydroxide
• Preparation and standardization of 0.1 M potassium iodate
• Preparation and standardization of 0.1 M silver nitrate
• Preparation and standardization of 0.1 M sodium methoxide solution
• Preparation and standardization of 0.1 M sodium nitrite
• Preparation and standardization of 0.1 M tetrabutylammonium hydroxide solution
• Preparation and standardization of 0.1 M zinc chloride
• Preparation and standardization of 0.1 M zinc sulphate
• Preparation and standardization of 0.1 N ammonium thiocyanate
• Preparation and standardization of 0.1 N HCl
• Preparation and standardization of 0.1 N iodine solution
• Preparation and standardization of 0.1 N potassium dichromate
• Preparation and standardization of 0.1 N potassium permanganate
• Preparation and standardization of 0.1 N sodium thiosulphate
• Preparation and standardization of 1N HCl
• Preparation and standardization of oxalic acid using sodium hydroxide
• Preparation of 2, 4-dinitrophenol indicator solution
• Preparation of 3-Nitrophenol indicator solution
• Preparation of acetic acid solution
• Preparation of alkali blue 6B indicator solution
• Preparation of amaranth indicator solution
• Preparation of bromocresol green indicator solution
• Preparation of bromocresol purple indicator solution
• Preparation of bromophenol blue indicator solution
• Preparation of calcon indicator solution
• Preparation of catechol violet indicator solution
• Preparation of cresol red indicator solution
• Preparation of crystal violet indicator solution
• Preparation of dichlorofluorescein indicator solution
• Preparation of dithizone indicator solution
• Preparation of eriochrome black T indicator solution
• Preparation of ferroin indicator solution
• Preparation of hydrochloric acid solution
• Preparation of m-cresol purple indicator solution
• Preparation of methyl orange indicator solution
• Preparation of methyl red indicator solution
• Preparation of methyl yellow indicator solution
• Preparation of methylene blue indicator solution
• Preparation of nitric acid solution
• Preparation of phenol red indicator solution
• Preparation of phenolphthalein indicator solution
• Preparation of phenosafranine indicator solution
• Preparation of potassium chromate indicator solution
• Preparation of quinaldine red indicator solution
• Preparation of sodium alizarin sulfonate indicator solution
• Preparation of sodium bicarbonate solution
• Preparation of sodium carbonate solution
• Preparation of pyridylazo naphthol indicator solution
• Preparation of sodium hydroxide solution
• Preparation of starch indicator solution
• Preparation of sulphuric acid solution
• Preparation of thymol blue indicator solution
• Preparation of thymolphthalein indicator solution
• Preparation of xylenol orange indicator solution
• Preparation of α-Naphtholbenzein indicator solution
• Prepare and standardize 0.1 n NaOH using succinic acid
• Prepare and standardize 0.1 n NaOH using succinic acid
• Prepare and standardize 0.1 M sodium thiosulphate
• Prepare and standardize 1M potassium permanganate
• Prepare and standardize 1M sulphuric acid
• Principle and procedure of Mohr’s method
• Principle and types of complexometric titration
• Principle and types of gravimetric analysis
• Principle and types of non-aqueous titration
• Principle and types of potentiometric titration
• Principle and types of precipitation titration
• Principle and types of redox titration
• Purpose of back titration
• Selection of indicators for a titration
• Sources of error in titration
• Standardization of HCl solution
• Standardization of NaOH with KHP
• Standardization of NaOH with oxalic acid
• Starch indicator in iodometric titration
• To perform the assay of copper sulphate by iodometry
• To perform the limit test of chloride
• Volumetric Analysis: Principle, Types, Procedure & Applications
• What are precautions taken during titration?
• What are the applications of titration?
• What causes the temporary and permanent hardness of water?
• What does the bromothymol blue indicate the presence of?
• What happens if too much indicator is added to a titration?
• What happens if you use the wrong indicator in a titration?
• What is a blank titration and why is it necessary
• What is acid base titration in chemistry?
• What is back titration in chemistry?
• What is complexometric titration in chemistry?
• What is end point in iodometric titration?
• What is equivalence point in chemistry?
• What is indicator in chemistry and its types
• What is litmus paper and how does it work
• What is pH and how is it measured
• What is pH paper and how does it work
• What is phenolphthalein and why is it used
• What is primary standard in chemistry?
• What is redox titration in chemistry?
• What is replacement titration in chemistry?
• What is self indicator with example
• What is standardization in chemistry?
• What is the color of methyl orange and phenolphthalein?
• What is the endpoint of titration?
• What is the first equivalence point in titration?
• What is the process of titration?
• What is the purpose of acid-base titration?
• What is the purpose of titration?
• What is the role of an indicator in the titration process?
• What is universal indicator and how does it work
• What is Volhard method of precipitation titration?
• What solution usually goes in the burette in titration?
• What type of a reaction is acid-base titration?
• What will be the pH at the equivalence point of strong base weak acid titration?
• When and why is back titration used?
• When we titrate oxalic acid with a KMnO4 solution, it gets pink with the first drop of KMnO4 from the burette, why is that?
• Which indicator is used in the titration of a weak acid and strong base?
• Which indicator is used in the titration of strong acid and a strong base?
• Which indicator is used in the titration of strong acid and weak base?
• Which indicator is used in the titration of the weak acid-weak base?
• Which titration falls under the category of acid-base?
• Why acid-base titration is important in food industry
• Why are strong acids generally used as standard solutions in acid-base titrations?
• Why did the color of phenolphthalein change after the addition of an acid?
• Why do we need to standardize NaOH solution?
• Why do we standardize a solution?
• Why does a temporary color appear in KMnO4 titration with oxalic acid?
• Why does EDTA need to be standardized?
• Why does oxalic acid decolorize potassium permanganate?
• Why does phenolphthalein turn pink?
• Why does the burette need to be rinsed before titration?
• Why is a weak acid best titrated with a strong base?
• Why is an indicator not needed in titration with KMnO4?
• Why is back titration used for insoluble salts?
• Why is EDTA used in complexometric titration?
• Why is EDTA used in the hardness of water?
• Why is H2SO4 used in titration?
• Why is it necessary to heat the oxalic acid solution?
• Why is methyl orange a suitable indicator for titrating weak base and strong acid?
• Why is methyl orange used in titration?
• Why is phenolphthalein better than methyl orange?
• Why is phenolphthalein used as an indicator in weak acid vs strong base titration?
• Why is the buffer solution used in the determination of hardness of water?
• Why is titration between a weak acid and a weak base not possible?
• Why is titration known as volumetric analysis?
• Why is used or not used as a primary standard?
• Why KMnO4 is a self indicator
• Why methyl orange changes color at differenr pH
• Why no indicator is suitable for weak acid and a weak base
• Why phenolphthalein is colorless in acid?
• Why phenolphthalein is used as indicator in titration?
• Why sodium hydroxide is not a primary standard
• Why starch is added towards the end of iodometric titration?
• Why the endpoint of titration is wine red to blue in the hardness determination?