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Related Concept Videos

Potentiometric Titration: Overview01:31

Potentiometric Titration: Overview

Potentiometric titration is a quantitative analytical technique that determines the concentration of an analyte by measuring the potential difference between the two electrodes in the solution. The endpoint of a potentiometric titration is the point at which there is a significant change in the potential difference. It occurs when the stoichiometric reaction between the analyte and the titrant is complete. The endpoint is usually determined graphically by plotting the measured potential...
Titration of a Weak Base with a Strong Acid01:20

Titration of a Weak Base with a Strong Acid

The titration curve of a weak base like ammonia with a strong acid like hydrochloric acid is the mirror image of the titration curve of a weak acid with a strong base.
Using the ICE table and substituting the Kb value, we calculate the initial pH of 50 mL of 0.1 M ammonia to be 11.11. Addition of 25 mL of 0.1 M hydrochloric acid to this solution of ammonia results in a buffer with an equal concentration of ammonia and ammonium ions. The pH of this buffer can be calculated by substituting these...
Precipitation Titration: Endpoint Detection Methods01:19

Precipitation Titration: Endpoint Detection Methods

In argentometric precipitation titrations, endpoints can be detected visually by the Mohr, Volhard, and Fajans methods. In the Mohr method, adding a soluble chromate indicator gives an initial yellow color to the analyte solution. As the titrant is added, the first excess of silver ions forms a red silver chromate precipitate, marking the endpoint. The solution pH should be maintained at about 8 by adding solid CaCO3.
In the Volhard method, a standard excess of AgNO3 is first added to the...
Titration in Nonaqueous Solvents01:16

Titration in Nonaqueous Solvents

Most acid-base titrations are performed in an aqueous medium. In aqueous titrations, water competes with weaker acids or bases for proton donation or acceptance, leading to ambiguous endpoints in the titration curve. Water also affects the partial ionization of weak acids or bases. For example, water accepts a proton from acetic acid to form hydronium and acetate ions. The hydronium ion formed is a stronger acid than acetic acid, and the acetate ion is a stronger base than water. As a result,...
Titration of a Weak Acid with a Weak Base01:08

Titration of a Weak Acid with a Weak Base

Weak acids and bases do not undergo dissociation completely, and titrations between these two are rarely studied. When such studies are performed, say, for the titration of a weak acid with a weak base, the titration curve plots the change in pH as a function of the volume of base added. Take the titration of acetic acid with ammonia, for instance. During the titration, these two species form ammonium acetate and water, but the pH change is slow and gradual.
As a result, there is no simple...
Titration of Polyprotic Base with a Strong Acid01:18

Titration of Polyprotic Base with a Strong Acid

The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titration curve. At the first equivalence point, the carbonate ions in the base are completely converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which dissociates into carbon dioxide and water. The region before the first equivalence point corresponds to the...

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Related Experiment Video

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Qualitative Identification of Carboxylic Acids, Boronic Acids, and Amines Using Cruciform Fluorophores
09:46

Qualitative Identification of Carboxylic Acids, Boronic Acids, and Amines Using Cruciform Fluorophores

Published on: August 19, 2013

Potentiometric and visual titrations with bromamine-B.

H S Gowda1, H N Ahmed Khan

  • 1Department of Post-graduate Studies & Research in Chemistry, University of Mysore, Manasa Gangotri, Mysore-570006, India.

Talanta
|September 1, 1982
PubMed
Summary
This summary is machine-generated.

Bromamine-B is a versatile oxidimetric titrant for various reductants, including arsenic and ascorbic acid. Several indicators are proposed for accurate potentiometric and visual titrations, with arsenic(III) and hexacyanoferrate(II) suitable for standardizing bromamine-B solutions.

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Area of Science:

  • Analytical Chemistry
  • Inorganic Chemistry

Background:

  • Oximetric titrations are crucial for quantitative analysis.
  • Developing new titrants and indicators enhances analytical accuracy.
  • Bromamine-B offers potential as a reliable oxidimetric agent.

Purpose of the Study:

  • To propose Bromamine-B as an oxidimetric titrant.
  • To evaluate its efficacy in titrating various reductants.
  • To identify suitable indicators for precise end-point detection.

Main Methods:

  • Potentiometric and visual end-point titrations were employed.
  • Bromamine-B was used as the titrant against multiple reductants.
  • Various organic and inorganic compounds were tested as indicators.

Main Results:

  • Bromamine-B successfully titrated arsenic(II), hexacyanoferrate(II), antimony(III), hydroquinone, semicarbazide hydrochloride, isonicotinic acid hydrazide, hydrazine sulphate, ascorbic acid, phenylhydrazine hydrochloride, and metol.
  • Ten indicators (Quinoline Yellow, naphthidine, dimethylnaphthidinedisulphonic acid, o-dianisidine, diphenylbenzidine, Variamine Blue, alpha-naphthoflavone, Amaranth, Methyl Orange, Methyl Red) were proposed.
  • Transition potentials for four indicators during ascorbic acid titration were determined.
  • Arsenic(III) and hexacyanoferrate(II) were identified as suitable for standardizing Bromamine-B.

Conclusions:

  • Bromamine-B is a viable and effective oxidimetric titrant for a wide range of reductants.
  • The proposed indicators facilitate accurate macro and micro titrations.
  • Standardization methods using arsenic(III) and hexacyanoferrate(II) are recommended.