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

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

SrCO3 |
2.4 × 10−5 |
2.4 × 10−5 |
_____ |

SrF2 |
1.0 × 10−3 |
_____ |
4.0 × 10−9 |

Ag2CO3 |
_____ |
1.3 × 10−4 |
8.8 × 10−12 |

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 |

SrCO3 | 2.4 x 10-5 | 2.4 x 10-5 | 5.76 x 10-10 |

SrF2 | 1.0 x 10-3 | 2.0 x 10-3 | 4.0 x 10-9 |

Ag2CO3 | 2.6 x 10-4 | 1.3 x 10-4 | 8.8 x 10-12 |

SrCO3 Sr2+ + CO32-

Solubility product for the reaction, Ksp = [Sr2+][CO32-]

= (2.4 x 10-5)(2.4 x 10-5)

= 5.76 x 10-10

b) The ionization of SrF2 takes place in the following manner:

SrF2