What mass (in g)of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC₂H₃O₂ solution with 55.0 mL of 0.109 M MgCl₂ solution? 2 AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2 AgCl(s)+ Mg(C₂H₃O₂)₂(aq) A) 0.838 g B) 1.72 g C) 0.859 g D) 2.56 g E) 1.70 g

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Quizplus · Accepted Answer

First, calculate the moles of AgC₂H₃O₂ and MgCl₂. For AgC₂H₃O₂: moles = 0.075 L * 0.078 mol/L = 0.00585 mol. For MgCl₂: moles = 0.055 L * 0.109 mol/L = 0.005995 mol. The reaction is limited by AgC₂H₃O₂ (since it produces AgCl in a 1:1 ratio), so moles of AgCl = 0.00585 mol. The molar mass of AgCl = 143.32 g/mol, so mass = 0.00585 mol * 143.32 g/mol = 0.838 g.

What Mass (In G)of AgCl Is Formed from the Reaction