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Argentometric titration. Definition: The process of determining the quantity of a sample by adding measured increments of a titrant until the end-point, at which. automatic titrator will be used to perform the titration, and to obtain the titration curve. Background. Argentometric Titrations. In order for a titrimetric method to be . A titration in which Ag+ is the titrant is called an argentometric titration. Table provides a list of several typical precipitation titrations.

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One of the earliest precipitation titrations—developed at titdations end of the eighteenth century—was the analysis of K 2 CO 3 and K 2 SO 4 in potash. A simple equation takes advantage of the fact that the sample contains only KCl and NaBr; thus.

The Fajans method was first published in the s by Kasimir Fajans. Prior to the end-point of the titration, chloride ions remain in excess. Ferric acetate removes phosphates. All chlorides are dissolved out of the residue, and titrated.

Calculate pCl at the equivalence point using the K sp for AgCl to calculate the concentration of Cl —. Calculate the titration curve for the titration of It is tittrations suitable for titrating against chloride anions because it binds to AgCl more strongly than chloride does.

The reaction in this case is. The analysis argentoemtric I — using the Volhard method requires a back titration. After the equivalence point, the titrant is in excess. As we have done with other titrations, we first show how to calculate the titration curve and then demonstrate how we can quickly sketch a reasonable approximation of the titration curve.


Although precipitation titrimetry is rarely listed as a standard method of analysis, it may still be useful as a secondary analytical method for verifying other analytical methods. Chloride ions react with silver I ions to give the insoluble silver chloride: Like, we use alkalimetric titration to calculate the real concentration of table vinegar. Before the titeations point, Cl — is present in excess argejtometric pCl is determined by the concentration of unreacted Cl —.

Argentometric (silver nitrate) titrations overview

Our goal is to sketch the titration curve quickly, using as few calculations as possible. Waylander 5, 1 10 Before precipitation titrimetry became practical, better methods for identifying the end point were necessary. They adsorb on the AgCl surface, imparting tjtrations negative charge to the particles. By using this site, you agree to the Terms of Use and Privacy Policy.

Chemistry Stack Exchange works best with JavaScript enabled. Email Required, but never shown. What about argentometric titration?

Argentometry – Wikipedia

Home Questions Tags Users Unanswered. Because dichlorofluoroscein also carries a argentommetric charge, it is repelled by the precipitate and remains in solution where it has a greenish-yellow color.

The end point is found by visually examining the titration curve. As a result, the end point is always later than the equivalence point. The quantitative relationship between the titrand and the titrant is determined by the stoichiometry of the titration reaction.


Carbonates and phosphates precipitate with silver, and need to be absent to prevent inaccurate results. At the beginning of this section we noted that the first precipitation titration used the cessation of precipitation to signal the end point. Precipitation titrations also can be extended to the analysis of mixtures provided that there is a significant difference in the solubilities of the precipitates.

Titration is in aqueous solution against a solution of silver nitrate of known concentration for silver I salts that give an insoluble precipitate. Eosin tetrabromofluorescein is suitable for titrating against bromideiodideand thiocyanate anions, giving a sharper end-point than dichlorofluorescein.

Precipitation Titrations – Chemistry LibreTexts

The pH also argentomeric be less than 10 to avoid the precipitation of silver hydroxide. A better fit is possible if the two points before the equivalence point are further apart—for example, 0 mL and 20 mL— and the two points after the equivalence point are further apart.

David Harvey DePauw University.