Ask Question
13 September, 11:37

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

+3
Answers (2)
  1. 13 September, 11:47
    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. 13 September, 12:03
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Calculate the molar solubility of ca (io3) 2 in each solution below. the ksp of calcium iodate is7.1 * 10-7. ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers