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26 January, 15:22

Calculate the molar solubility of ca (io3) 2 in each solution below. the ksp of calcium iodate is7.1 * 10-7.

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Answers (2)
  1. 26 January, 18:52
    0
    In order to find the answer, use an ICE chart:

    Ca (IO3) 2 ... Ca2 + ... IO3-

    some ... 0 ... 0

    less ... + x ... + 2x

    less ... x ... 2x

    Ca (IO₃) ₂ ⇄ Ca⁺² + 2 IO⁻³

    K sp = [Ca⁺²][IO₃⁻]²

    K sp = (x) (2 x) ² = 4 x³

    7.1 x 10⁻⁷ = 4 x³

    x = molar solubility = 5.6 x 10 ⁻³ M

    The answer is 5.6 x 10 ^ 3 M. (molar solubility)
  2. 26 January, 18:58
    0
    Answer: 5.62 x 10⁻³ M

    Explanation:

    1) Equilibrium equation:

    Ca (IO₃) ₂ ⇄ Ca⁺² + 2 IO⁻³

    2) By stoichimetry ratio, the concentrtion of IO⁻³ ions is the double than the concentraion of Ca⁺², so call them x and 2x.

    3) Solubility product constant, Ksp:

    Ksp = [Ca⁺²] [IO⁻³]² = x (2x) ² = 4x³

    => 4x³ = 7.1 x 10⁻⁷

    => x^3 = 1.775 x 10⁻⁷

    => x = 5.62 x 10⁻³ M
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