AgNO3(aq)+KCl(aq)?AgCl(s)+KNO3(aq)

Question

Part A
What mass of silver chloride can be produced from 1.19L of a 0.293M solution of silver nitrate?
Express your answer with the appropriate units.

mass of AgCl =

Part B
The reaction described in Part A required 3.47L of potassium chloride. What is the concentration of this potassium chloride solution?
Express your answer with the appropriate units.

Answer 1

Part A:

First, convert molarity to moles by multiplying by the volume:

0.293 M AgNO₃ = (0.293 moles AgNO₃)/1 L x 1.19 L = 0.349 moles AgNO₃

 

We are only interested in AgCl, not AgNO₃. We convert moles of silver nitrate to moles of silver chloride using the balanced equation. This is a 1:1 conversion:

0.349 moles AgNO₃ x (1 mole AgCl)/(1 mole AgNO₃) = 0.349 moles AgCl

 

To get mass from moles, we multiply by the molar mass:

0.349 moles AgCl x (143.32 g/mol) = 50.0 g AgCl

 

The appropriate unit for mass is, of course, grams.

 

Part B:

Use the moles of AgNO₃ from Part A. Then use the balanced equation to convert from moles of silver nitrate to moles of potassium chloride:

0.349 moles AgNO₃ x (1 mole KCl)/(1 mole AgNO₃) = 0.349 moles KCl

 

Concentration units are molarity, M. This is equal to moles/Liter. We were told that 3.47 L were required. Now we just plug in the numbers.

M = (0.349 moles KCl)/(3.47 L) = 0.101 M