Ionic Equilibrium - 1

What is the \(\text{pH}\) of the resultant solution formed by adding these 5 weak acids?

Here \(c\) is the Concentration and \(k_a\) is the acid dissociation constant.

Acid 1 : \( {c}_{1} = 0.1999 N \) , \( {k}_{\text {a1}} = 2.036 × {10}^{-15} \)

Acid 2 : \( {c}_{2} = 0.02367 N \) , \( {k}_{\text {a2}} = 5.0093× {10}^{-15} \)

Acid 3 : \( {c}_{3} = 0.5678 N \) , \( {k}_{\text {a3}} = 3.9925 × {10}^{-16} \)

Acid 4 : \( {c}_{4} = 0.09826 N \) , \( {k}_{\text {a4}} = 6.5762 × {10}^{-16} \)

Acid 5 : \( {c}_{5} = 6.753 N \) , \( {k}_{\text {a5}} = 0.7036 × {10}^{-15} \)

Enter your answer as \( [ \text {pH} ]\) , where [ ] is greatest integer function.

Original!

This is a part of my set Aniket's Chemistry Challenges. (BEST OF JEE - ADVANCED)