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7 October, 13:22

60.0 mL of 0.322 M potassium iodide are combined with 20.0 mL of 0.530 M lead () nitrate. What is the limiting reactant? How many grams of precipitate form?

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  1. 7 October, 13:48
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    Limiting reagent: Potassium iodide

    Mass of the precipitate (PbI₂) is 4.453 g

    Explanation:

    We are given;

    60.0 mL of 0.322 M potassium iodide 20.0 mL of 0.530 M lead () nitrate

    We are required to identify the limiting reactant and determine the mass of the precipitate formed.

    Step 1: Write the balanced equation for the reaction The balanced equation for the reaction between potassium iodide and lead (II) nitrate is given by;

    2KI + Pb (NO₃) ₂ → 2KNO₃ + PbI₂ (s)

    Step 2: Determine the number of moles of the reagents

    Moles of KI

    Moles = Molarity * volume

    Moles of KI = 0.322 M * 0.060 L

    = 0.01932 moles

    Moles of KNO₃

    Moles = 0.530 M * 0.020 L

    = 0.0106 M

    From the equation;

    2 moles of KI reacts with 1 mole of Pb (NO) ₂ Therefore; 0.01932 moles of KI will require 0.00966 moles of Pb (NO₃) ₂ This means, KI is the limiting reagent while Pb (NO₃) ₂ is the excess reagent. Step 3: Determine the mass of the precipitate PbI₂

    2 moles of KI reacts to produce 1 mole of PbI₂

    Therefore;

    Moles of PbI₂ = Moles of KI : 2

    = 0.01932 moles : 2

    = 0.00966 moles

    But molar mass of PbI² is 461.01 g/mol

    Therefore;

    Mass of PbI₂ = 0.00966 moles * 461.01 g/mol

    = 4.453 g

    Therefore, the mass of the precipitate formed (Pbi₂) is 4.453 g
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