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5 October, 19:36

Predict whether or not a precipitate forms upon mixing 175.0 ml of a 0.0055 mkcl solution with 145.0 ml of a 0.0015 m agno3 solution. identify the precipitate, if any. express your answer as a chemical formula. enter noreaction if no precipitate is formed.

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  1. 5 October, 20:49
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    Step 1: Write down the chemical reaction

    KCl (aq) + AgNO3 (aq) → AgCl (s) + KNO3 (aq)

    The precipitate that can be expected is AgCl

    Step 2: Calculate the moles of KCl and AgNO3

    # moles of KCl = V (KCl) * M (KCl)

    = 0.175 L * 0.0055 moles/L = 9.63*10⁻⁴ moles

    # moles of AgNO3 = V (AgNO3) * M (AgNO3)

    = 0.145 L * 0.0015 moles/L = 2.18*10⁻⁴ moles

    Since moles of AgNO3 < KCl, the former is the limiting reagent

    Therefore, moles of AgCl formed = 2.18*10⁻⁴ moles

    Step 3: Predict if AgCl precipitate will be formed

    The solubility product Ksp for AgCl = 1.6 * 10⁻¹⁰

    i. e.

    AgCl (s) ↔ Ag⁺ (aq) + Cl⁻ (aq)

    Ksp = [Ag+][Cl-]

    if [Ag+][Cl-] > Ksp then precipitation will occur

    Now total volume of the solution = 175 + 145 = 320 ml = 0.320 L

    [Ag+] = [Cl-] = 2.18*10⁻⁴ moles/0.320 L = 6.81*10⁻⁴ M

    [Ag+][Cl-] = (6.81*10⁻⁴) ² = 4.64 * 10⁻⁷

    Since [Ag+][Cl-] > Ksp, AgCl precipitate will be formed.
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