How do you calculate the mass of silver chloride in this chemistry problem?

Silver chloride, often used in silver plating, contains 75.27% Ag.

Calculate the mass of silver chloride required to plate 165 mg of pure silver?

use molar masses:
0.165 grams Ag @ (143.32 g/mol AgCl) / (107.9 g/mol Ag) =
0.219 g AgCl would be required

using a ratio of % ’s
0.165 g Ag @ (100 % AgCl) / (75.27% Ag) =
0.219 g of AgCl would be required

in both ways,
your answer is
219 mg of AgCl

This entry was posted on Thursday, January 28th, 2010 at 1:09 am and is filed under silver. You can follow any responses to this entry through the RSS 2.0 feed. You can leave a response, or trackback from your own site.

One Response to “How do you calculate the mass of silver chloride in this chemistry problem?”

Steve O on January 28th, 2010 at 6:44 am

use molar masses:
0.165 grams Ag @ (143.32 g/mol AgCl) / (107.9 g/mol Ag) =
0.219 g AgCl would be required

or

using a ratio of % ’s
0.165 g Ag @ (100 % AgCl) / (75.27% Ag) =
0.219 g of AgCl would be required

in both ways,
your answer is
219 mg of AgCl
References :

The Fools Gold