Phosphoric acid ionizes in three steps with their ionization constant values Kₐ₁, Kₐ_₂ and Kₐ_₃ respectively, while K is the overall ionization constant. Which of the following statements are true?
A. log K = log Kₐ₁ + log Kₐ₂ + log Kₐ₃
B. H₃PO₄ is stronger acid than H₂PO₄⁻ and HPO₄²⁻.
C. Kₐ₁ > Kₐ₂ > Kₐ₃
D. Ka= (Ka₃+Ka₂)/2 
Choose the correct answer from the options below:

CONCEPT:

Phosphoric Acid Ionization and Acid Strength

• Phosphoric acid (H₃PO₄) ionizes in three steps, leading to the formation of H₂PO₄^-, HPO₄^2-, and PO₄^3- respectively.
• Each ionization step has an associated ionization constant, denoted as Kₐ₁, Kₐ₂, and Kₐ₃.
• The overall ionization constant (K) is the product of the individual ionization constants: K = Kₐ₁ × Kₐ₂ × Kₐ₃.
• The logarithm of the overall ionization constant is the sum of the logarithms of the individual constants: log K = log Kₐ₁ + log Kₐ₂ + log Kₐ₃.
• The strength of an acid decreases as it ionizes further (i.e., H₃PO₄ is stronger than H₂PO₄^-, which is stronger than HPO₄^2-).

EXPLANATION:

• Statement A: log K = log Kₐ₁ + log Kₐ₂ + log Kₐ₃ is correct because the overall ionization constant is the product of the individual ionization constants, and the logarithm of a product is the sum of the logarithms of the individual factors.
• Statement B: H₃PO₄ is stronger than H₂PO₄^- and HPO₄^2- is correct because the acid strength decreases with successive ionizations. The first ionization constant (Kₐ₁) is the largest, making H₃PO₄ the strongest acid among its ionized forms.
• Statement C: Kₐ₁ > Kₐ₂ > Kₐ₃ is correct because the ionization constants decrease sequentially as the molecule loses protons, reflecting decreasing acid strength with each step.
• Statement D: K = (Kₐ₁ + Kₐ₂)/2 is incorrect because the overall ionization constant is the product of Kₐ₁, Kₐ₂, and Kₐ₃, not an average of the first two constants.

Therefore, the correct answer is A, B, and C only.