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Ksp from the solubility (in grams per volume) or the ion concentrations

This type of question, asked 3 times: 27 Jul 2022, 31 Jan 2023, 9 Apr 2024. All 3 questions below, oldest first.

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  1. Question 1

    27 Jul 2022

    56
    At 310 K310\text{ }K, the solubility of CaF2CaF_{2} in water is 2.34×10−3 g/100 mL2.34 \times 10^{-3}\text{ }g/100\text{ }mL. The solubility product of CaF2CaF_{2} is ____\_\_\_\_ ×10−10( mol/L)3\times 10^{-10}(\text{ }mol/L)^{3}. (Given molar mass: CaF2=78 g mol−1CaF_{2}= 78\text{ }g{\text{ }mol}^{-1})

  2. Question 2

    31 Jan 2023

    145
    At 98 K98\text{ }K, the solubility of silver chloride in water is 1.434×10−3 g L−11.434 \times10^{- 3}\text{ }g{\text{ }L}^{- 1}. The value of −log⁡Ksp- \log K_{sp} for silver chloride is (Given mass of AgAg is 107.9 g mol−1107.9\text{ }g{\text{ }mol}^{- 1} and mass of ClCl is 35.5 g mol−135.5\text{ }g{\text{ }mol}^{- 1} )

  3. Question 3

    9 Apr 2024

    132
    For a sparingly soluble salt AB2AB_{2}, the equilibrium concentrations of A2+A^{2 +} ions and B−B^{-}ions are 1.2×10−4M1.2 \times10^{- 4}M and 0.24×10−3M0.24 \times10^{- 3}M, respectively. The solubility product of AB2AB_{2} is:

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