A solution contains 1.77 g of dissolved silver. How many moles of potassium chloride must be added to the solution to completely precipitate all of the silver? What mass of potassium chloride must be added?
Here, we are going to calculate the number of moles and mass of potassium chloride that must be added to the given solution.
One mole of any species is that quantity in number having a mass equal to its atomic or molecular mass in grams.
Thus, the number of moles = given mass / molar mass
Here, given mass of silver = 1.77 g
Molar mass of silver = 107.8682 g/mol
Therefore, number of moles of silver in solution =
= 0.0164 mol
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
This full solution covers the following key subjects: added, chloride, silver, potassium, must. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Since the solution to 112P from 7 chapter was answered, more than 1120 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 112P from chapter: 7 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. The answer to “A solution contains 1.77 g of dissolved silver. How many moles of potassium chloride must be added to the solution to completely precipitate all of the silver? What mass of potassium chloride must be added?” is broken down into a number of easy to follow steps, and 35 words.