Monday
March 30, 2015

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?

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry - The mass percentage of chloride ion in a 29.00 sample of seawater ...
Chemistry - Science - A 6.70 g sample of a binary mixture of silver (I) nitrate...
Chemistry - A 0.4584 g sample of impure zinc chloride, ZnCl2, FW = 136.3 g/mole...
chemistry - An aqueous solution of silver nitrate contains 5.00 g of silver ...
Chemisty 20 - A sample of water was known to contain chloride ions. To determine...
chemistry - the chlorine in a 0.12g sample of 95% pure magnesium chloride is to ...
chemistry - problem 2. a sample of calcium chloride weighs 1.64g. it is ...
Chemistry - A mixture contains only CuCl2 and FeCl3. A 0.7391 g sample of the ...
chem - a 6.54 g sample consisting of a mixture of silver nitrate and sodium ...
Chemistry - 0.12 g of rock salt(NaCl and impurities) was dissolved in water and ...

Members