Ionic Equilibrium - 1

Chemistry Level 3

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

Here cc is the Concentration and kak_a is the acid dissociation constant.

Acid 1 : c1=0.1999N {c}_{1} = 0.1999 N , ka1=2.036×1015 {k}_{\text {a1}} = 2.036 × {10}^{-15}

Acid 2 : c2=0.02367N {c}_{2} = 0.02367 N , ka2=5.0093×1015 {k}_{\text {a2}} = 5.0093× {10}^{-15}

Acid 3 : c3=0.5678N {c}_{3} = 0.5678 N , ka3=3.9925×1016 {k}_{\text {a3}} = 3.9925 × {10}^{-16}

Acid 4 : c4=0.09826N {c}_{4} = 0.09826 N , ka4=6.5762×1016 {k}_{\text {a4}} = 6.5762 × {10}^{-16}

Acid 5 : c5=6.753N {c}_{5} = 6.753 N , ka5=0.7036×1015 {k}_{\text {a5}} = 0.7036 × {10}^{-15}

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


Original!

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