🤓 Based on our data, we think this question is relevant for Professor Taylor's class at UTD.

We are asked to arrange the following oxyanions from the **strongest base to weakest** using the acid-dissociation constants in the table.

SO_{3}^{2-}, PO_{4}^{2-}, SO_{4}^{2-}, CO_{3}^{2-}

**The acid dissociation constant**, *K*_{a}, (also known as **acidity constant**, or **acid-ionization constant**) is a quantitative measure of the strength of an acid in solution.

For an aqueous solution, the general form of the equilibrium reaction is:

HA(aq) + H_{2}O(l) ⇆ A^{-} (aq)+ H_{3}O^{+}(aq)

where:

HA is an acid that dissociates into the conjugate base of the acid A^{-}

and a hydrogen ion that combines with water to form the hydronium ion H_{3}O^{+}.

Use the acid-dissociation constants in the following table to arrange these oxyanions from strongest base to weakest.

SO_{3}^{2-}, PO_{4}^{2-}, SO_{4}^{2-}, CO_{3}^{2-}

Name | Formula | K_{a1} | K_{a2} | K_{a3} |

Ascorbic | H_{2}C_{6}H_{6}O_{6} | 8.0 x 10^{-5} | 1.6 x10^{-12} | |

Carbonic | H_{2}CO_{3} | 4.3 x 10^{-7} | 5.6 x 10^{-11} | |

Citric | H_{3}C_{6}H_{5}O_{7} | 7.4 x 10^{-4} | 1.7 x 10^{-5} | 4.0 x 10^{-7} |

Oxalic | H_{2}C_{2}O_{4} | 5.9 x 10^{-2} | 6.4 x 10^{-5} | |

Phosphoric | H_{3}PO_{4} | 7.5 x 10^{-3} | 6.2 x 10^{-8} | 4.2 x 10^{-13} |

Sulfurous | H_{2}SO_{3} | 1.7 x 10^{-2} | 6.4 x10^{-8} | |

Sulfuric | H_{2}SO_{4} | Large | 1.2 x10^{-2} | |

Tartaric | H_{2}C_{4}H_{4}O_{6} | 1.0x 10^{-3} | 4.6 x10^{-5} |