When 50.0 mL of a 0.3000 M AgNO₃ solution is added to 50.0 mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of 0.1183 g, what is the concentration of magnesium ions in the original MgCl₂ solution? A)0.300 M B)8.25 * 10^-3 M C)1.65 * 10^-2 M D)2.06 * 10^-5 M E)4.13 * 10^-3 M

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:2AgNO₃(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO₃)₂(aq)From the stoichiometry of the balanced equation, we see that 2 moles of AgNO₃ react with 1 mole of MgCl₂. Therefore, the concentration of MgCl₂ in the original solution can be calculated as follows:[MgCl₂] = (0.3000 M AgNO₃)(50.0 mL AgNO₃ solution)(1/2 mol MgCl₂/2 mol AgNO₃)/(50.0 mL MgCl₂ solution) = 0.0150 MTherefore, the concentration of magnesium ions in the original MgCl₂ solution is 0.0150 M, which is choice B.

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