A 0.897 g sample containing the chloride ion is treated with excess lead(II) nitrate. The precipitate is filtered using a 0.923 g piece of filter paper. After washing and drying, the mass of the precipitate and filter paper was 2.686 g. e. The mass percent chloride in the sample.
A 0.897 g sample containing the chloride ion is treated with excess lead(II) nitrate. The precipitate is filtered using a 0.923 g piece of filter paper. After washing and drying, the mass of the precipitate and filter paper was 2.686 g. e. The mass percent chloride in the sample.
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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
Transcribed Image Text:The problem involves a quantitative analysis of chloride ion content in a sample through a precipitation method. Here's the scenario:
A 0.897 g sample containing chloride ions is treated with an excess amount of lead(II) nitrate. This reaction results in the formation of a precipitate. This precipitate is collected using a piece of filter paper that initially weighs 0.923 g. After undergoing processes of washing and drying, the combined mass of the precipitate and filter paper is found to be 2.686 g.
Task:
Calculate the mass percent of chloride in the original sample.
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