Question

A sample of solution has a mixture of 0.01 M Aluminum Chloride and 0.05 M Magnesium Chloride. What is the molarity of Silver that is required to precipitate all the chloride ions present in the solution? *

Answer 1

Given:

• Molarity of aluminium chloride is equal to 0.01M
• Molarity of magnesium chloride is equal to 0.05M

To find:

The molarity of silver required to precipitate out all the chloride ions as silver chloride.

Solution:

• Each mole of aluminium chloride, magnesium chloride and silver chloride contains 3, 2 and 1 chloride ions respectively.
• Molarity of chloride ions in the solution is equal to (0.01*3 + 0.05*2) = 0.13 M
• The molarity of silver required will be the same as the molarity of chloride ions,i.e equal to 0.13 M

Answer:

The molarity of silver required to precipitate out all the chloride ions as silver chloride is equal to 0.13M