0.839 g of AgCl is formed.
<h3>Further explanation</h3>
Given a reaction between:
- 75.0 ml of a 0.078 M AgC₂H₃O₂ solution
- 55.0 ml of 0.109 M MgCl₂ solution
Question:
What mass, in g, of AgCl is formed?
The Process:
<u>Step-1:</u>
Let us find the mole numbers of both reagents:
AgC₂H₃O₂ → 0.078 x 0.075 = 5.85 mmol
MgCl₂ → 0.109 x 0.055 = 5.995 mmol
<u>Step-2:</u>
The equation for the reaction is
According to the equation, 2 mol of AgC₂H₃O₂ react with 1 mol of AgCl.
Let us check which substances will be a limiting reagent.
AgC₂H₃O₂ →
MgCl₂ →
AgC₂H₃O₂ is the limiting reagent because the test results are the smallest.
<u>Step-3:</u>
As AgC₂H₃O₂ is the limiting reagent, the amount of AgCl produced will be determined by the amount of AgC₂H₃O₂. Since the proportion between the mole numbers of AgC₂H₃O₂ and AgCl is one to one, their mole numbers will be equal:
So the amount of AgCl is 5.85 moles.
<u>Step-4:</u>
Prepare the molar mass of AgCl.
Mr = 108 + 35.5 = 143.5 g/mol
Let us find out how many mass, in g, of AgCl is formed.
Mass = 5.85 mmol x 143.5 g/mol
Mass = 839.475 mg ≈ 0.839 g.
Thus the amount of AgCl is formed is 0.839 g.
<h3>
Learn more</h3>
- About the mass and density of substances brainly.com/question/4053884
- Conservation of mass brainly.com/question/9473007
- To make a 0.500 M solution, one could take 0.500 moles of solute and add? brainly.com/question/10278982