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24 January, 16:34

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 * 10-10.

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  1. 24 January, 17:21
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    Since Q > Ksp, a precipitate of AgCl will form.

    Explanation:

    Step 1: Data given

    Molarity AgNO3 = 0.10 M

    Molarity of NaCl = 0.075 M

    Ksp AgCl = 1.77 * 10^-10

    Step 2: The balanced equation

    AgNO3 + NaCl → AgCl (s) + NaNO3 (aq)

    For 0.10 moles AgNO3 we have 0.10 moles Ag + (molarity = 0.10 M)

    For 0.075 moles NaCl we have 0.075 moles Cl - (molarity = 0.075 M)

    Step 3: Calculate Q

    Q = [Ag+][Cl-]

    Q = (0.10 M) (0.075 M) = 0.0075

    Ksp = 1.77 * 10^-10

    Q >>> Ksp

    Since Q > Ksp, a precipitate of AgCl will form.
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