Write 5 pages with APA style on Gravimetric Analysis. Stoichiometry is then used to calculate the chloride content .silver chloride formation is used to determine the chloride ions concentration.

Whereas it is thought that the reaction above goes to completion as a result of AgCl(s)s insolubility, some amount of AgCl(s) do, however, dissolve. By determining the solubility product Ksp, the solubility can be shown.

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Write 5 pages with APA style on Gravimetric Analysis. Stoichiometry is then used to calculate the chloride content .silver chloride formation is used to determine the chloride ions concentration.Where
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Silver chloride will thus be in equilibrium with the ions in the mixture since Ksp is so small, and the dissolved ions can be considered negligible. When AgNO3 is added to a solution mixture of Cl- ions a displacement reaction occurs and the Cl- and Ag ions will precipitate as AgCl(s). This reaction continues until all of the Cl- is consumed.

Depending on the quantity of excess Ag+, added to the mixture, a small quantity of salt will be left in the mixture. Maximum solubility occurs in the absence of excess Ag+ ion, and thus Ksp value is used in calculating the remaining Cl- in the solution.

The particles formed are tiny since there is little time for the formation of crystals. To collect the formed precipitate without some losses through the filter paper, the colloid is gently heated and stirred in nitric acid presence to form larger crystals leaving a semi-clear liquid. The purpose of nitric acid is to prevent the reversion of the newly formed crystals. The precipitate is filtered, weighed and dried for calculation.

Rapid precipitation of the AgCl(s) to the colloid state causes other ions to be trapped as well. To counteract this precipitation performed slowly in an acidic environment. The acid solution mixture is not affected by anions of weak acids that might also form precipitates with the silver ions. Precaution must be taken to avoid a large excess of silver ions since it can lead to unwanted precipitates. Interfering ions might precipitate with excess Ag+ in the solution mixture leading to the increased mass of precipitate.

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