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The dissociation constant of weak acid HA is  4.9× 10-8. After making the necessary approximations, calculate pH of 0.1 M acid.

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a
1.155
b
2.155
c
3.155
d
4.155

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detailed solution

Correct option is D

For weak acid Ka =C α2.∴      α = KaC = 4.9× 10-80.1 = 7× 10-4[ H+]=Cα PH=-log [ H+]=-log  Cα     =-log 7× 10-4× 10-1       = 4.1549 = 4.155

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