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20 November, 21:58

48.0 mL of 1.70 M CuCl2 (aq) and 57.0 mL of 0.800 M (NH4) 2S (aq) are mixed together to give CuS (s) as a precipitate. The other product of the reaction is aqueous ammonium chloride. What is the concentration of the Cu (II) ion after the complete reaction?

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  1. 20 November, 22:42
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    The concentration of the Cu (II) ion is 0.777M

    Explanation:

    Step 1: Data given

    Volume of 1.70 M CuCl2 = 48.0 mL = 0.0480 L

    Volume of 0.800 M (NH4) 2S = 57.0 mL = 0.0570 L

    Step 2: The balanced equation

    CuCl2 (aq) + (NH4) 2S (aq) → 2 NH4Cl (aq) + CuS (s)

    Step 3: Calculate moles CuCl2

    moles CuCl2 = 0.0480 L * 1.70 M=0.0816 moles

    Step 4: Calculate moles (NH4) 2S

    moles (NH4) 2S = 0.0570 L * 0.800 M = 0.0456 moles

    Step 5: Calculate the limiting reactant

    The ratio between CuCl2 and (NH4) 2S is 1 : 1 so (NH4) 2S is the limiting reactant. IT will completely be consumed (0.0456 moles).

    CuCl2 is in excess. There will remain 0.0816 - 0.0456 = 0.0360 moles

    Step 6: Calculate moles of CuS

    For 1 mol CuCl2 we need 1 mol (NH4) 2S to produce 2 moles of NH4Cl and 1 mol CuS

    For 0.0456 moles we'll produce 0.0456 moles CuS

    Step 7: Calculate moles of Cu (II) ion

    There remains 0.0360 moles CuCl2.

    There will be 0.0456 moles CuS produced

    Total moles Cu^2 + = 0.0816 moles

    Step 8: Calculate concentration of Cu (II) ion

    Concentration = moles / volume

    Concentration = 0.0816 moles / (0.048+0.057)

    Concentration = 0.777 M

    The concentration of the Cu (II) ion is 0.777M
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