Tuesday
July 22, 2014

Homework Help: chemistry

Posted by James on Tuesday, March 16, 2010 at 8:05pm.

The traditional method of analyzing the amount of chloride ion present in a sample was to dissolve the sample in water and then slowly add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample.

Ag+(aq) + Cl-(aq) -> AgCl(s_

Suppose that a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?

I'm confused on what to do. What do I do with the silver nitrate?

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