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

Question

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

Infinity Learn · Accepted Answer

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

Dissociation constants of two acids HA and HB are respectively $4 \times 10^{- 10}$ and $4 \times 10^{- 5}$ , whose pH value will be higher for a given molarity

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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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Dissociation constants of two acids HA and HB are respectively $4 \times 10^{- 10}$ and $4 \times 10^{- 5}$ , whose pH value will be higher for a given molarity