Suppose we carry out the precipitation of Ag 2 CrO 4 (s) described in Example 4-10. If

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Suppose we carry out the precipitation of Ag2CrO4(s) described in Example 4-10. If we obtain 2.058 g of precipitate, we might conclude that it is nearly pure Ag2CrO4 but if we obtain 2.112 g, we can be quite sure that the precipitate is not pure. Explain this difference.

Example 4-10

A 25.00 mL pipetful of 0.250 M K2CrO4 is added to an excess of AgNO3(aq). What mass of Ag2CrO4 will precipitate from the solution?

K2CrO4(aq) + 2 AgNO3(aq)→Ag2CrO4(s) + 2 KNO3(aq)

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General Chemistry Principles And Modern Applications

ISBN: 9780132931281

11th Edition

Authors: Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette

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