Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.

Compound |
[Cation] |
[Anion] |
Ksp |

CdS |
3.7 × 10−15 |
3.7 × 10−15 |
_____ |

BaF2 |
_____ |
7.2 × 10−3 |
1.9 × 10−7 |

Ag2SO4 |
2.8×10−2 |
_____ |
1.1 × 10−5 |

Solution: Here, we are going to complete the given table.

Step1:

Solubility product of any substance is the product of the concentrations of the dissolved ions raised to the power of their stoichiometric coefficients.

Consider the ionization of a substance AB,

AB A+ + B-

Then, the solubility product, Ksp = [A+][B-]

\Step2:

Compound | [Cation] | [Anion] | Ksp |

CdS | 3.7 x 10-15 | 3.7 x 10-15 | 1.369 x 10-29 |

BaF2 | 3.665 x 10-3 | 7.2 x 10-3 | 1.9 x 10-7 |

Ag2SO4 | 2.8 x 10-2 | 1.403 x 10-2 | 1.1 x 10-5 |

CdS Cd2+ + S2-

Solubility product for the reaction, Ksp = [Cd2+][S2-]

= (3.7 x 10-15)(3.7 x 10-15)

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