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Vilka [71]
3 years ago
7

Given the ion C2O4-2, what species would you expect to form with each of the following ions?

Chemistry
1 answer:
Ksivusya [100]3 years ago
6 0

Answer:

A. K₂C₂O₄          Potassium oxalate

B. CuC₂O₄          Copper oxalate

C. Bi₂(C₂O₄)₃         Bismuth (III) oxalate

D. Pb(C₂O₄)₂         Lead (IV) oxalate

E. (NH₄)₂C₂O₄       Ammonium oxalate

F. HC₂O₄⁻             Acid oxalate

Explanation:

C₂O₄⁻²  → oxalate anion

This is the conjugate base from the H₂C₂O₄ which is the oxalic acid. A weak dyprotic acid that can release 2 protons.

A. 2K⁺  +  C₂O₄⁻²  → K₂C₂O₄          Potassium oxalate

It can be formed by the neutralization of the acid with the base

H₂C₂O₄  + 2KOH  → K₂C₂O₄  +  2H₂O

B. Cu²⁺ +  C₂O₄⁻²   ⇄  CuC₂O₄  ↓

This is a precipitate.

C.  2Bi³⁺  +  3C₂O₄⁻²   ⇄  Bi₂(C₂O₄)₃  ↓

This is a precipitate.

D.  Pb⁴⁺ +  2C₂O₄⁻²   ⇄  Pb(C₂O₄)₂  ↓

This is a precipitate.

E. 2NH₄⁺  +  C₂O₄⁻²   ⇄  (NH₄)₂C₂O₄  ↓

This is a precipitate.

F. This is the conjugate strong base, for the weak acid

H⁺  +  C₂O₄⁻²   ⇄  HC₂O₄⁻

HC₂O₄⁻  + H₂O  ⇄  C₂O₄⁻²  +  H₃O⁺    Ka

HC₂O₄⁻  + H₂O  ⇄  H₂C₂O₄  +  OH⁻    Kb

HC₂O₄⁻  is an amphoteric compound

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The following data were obtained from the question:

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Equilibrium constant for a reaction is simply the ratio of concentration of the product raised to their coefficient to the concentration of the reactant raised to their coefficient.

The equilibrium constant for the above equation is given below:

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Equilibrium constant (Ka) =

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Equilibrium constant, Ka = 5.71×10¯⁷

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pKa = 6.24

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