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30 July, 14:32

Calculate the solubility at 25°c of cubr in pure water and in a 0.0030m cobr2 solution. you'll find ksp data in the aleks data tab. round both of your answers to 2 significant digits. solubility in pure water: gl

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  1. 30 July, 14:46
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    the solubility at 25°c of cubr in pure water = 0.011 g/L

    The solubility at 25°c of cubr in a 0.0030m cobr2 solution = 0.00014 g/L

    Explanation:

    Step 1: Data given

    Ksp of CuBr = 6.27 * 10^-9

    Molar mass CuBr = 143.45 g/mol

    Step 2: Calculate the solubility at 25°c of cubr in pure water

    Ksp = [Cu+][Br-]

    The initial concentration

    [Cu+] = 0M

    [Br-] = 0M

    The concentration at the equilibrium

    [Cu+] = X M

    [Br-] = X M

    Ksp = 6.27 * 10^-9 = X * X = X²

    S = 7.9 * 10^-5 mol / l

    7.9 * 10^-5 mol/L * 143.45 g/mol = 0.011 g/L

    Step 3: Calculate the solubility at 25°c of cubr in a 0.0030m cobr2 solution.

    The balanced equation:

    CoBr2 (aq) → Co^2 + (aq) + 2 Br⁻ (aq)

    For 1 mol CoBr2 we'll have 1 mol Co^2 + and 2 moles Br-

    For 0.0030 M CoBr2 we'll have 0.0030 M Co^2 + and 0.0060 M Br-

    The initial concentration

    [Cu+] = 0M

    [Br-] = 0.0060 M

    At the equilibrium

    [Cu+] = X

    [Br-] = 0.0060 + X

    Ksp = 6.27 * 10^-9 = X * (0.0060+X)

    6.27 * 10^-9 = 0.0060 X + X²

    X = 1.0 * 10^-6 mol/L

    1.0 * 10^-6 mol/L * 143.45 g/mol = 0.00014 g/L
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