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Dissociation constants of two acids HA and HB are respectively 4 × 10-10 and 4 × 10-5, whose pH value will be higher for a given molarity

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a
HA
b
HB
c
Both same
d
Can't say

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detailed solution

Correct option is A

HA  ⇌  H++A-HB  ⇌  H++B-For HAKa = α2Cα1  = Ka1C = 4 × 10-101α1 = 2 × 10-5  for C = 1 MSimilarly  ⇒  H+ = Cα = 2 × 10-5 ;  pH =-log [H+] = 4.7For HB:  α2  = Ka2C = 1.8 × 10-51 for  C = 1 Mα2 = 4.2 × 10-3  ⇒  H+=Cα                                                = 4.2 × 10-3 pH =-log  4.2 × 10-3 = 2.37 ;   PH of HA>HB

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