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Electrolysis and Electrolytes

Why conjugate...

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Why conjugate bases of strong acids have less tendency than water to accept protons in aqueous solution?

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Q. Assertion :Assertion : Weak acids have very strong conjugate bases while strong acids have weak conjugate bases. Reason: Reason : Conjugate acid-base pair differ only by one proton.

Assertion: The conjugate acid of sulphate

(S O_{4}^{2 -})

H S O_{4}^{-}

Reason: Bronsted acids have an extra proton in them than their conjugate bases.

Q. Assertion :It is difficult to distinguish the strengths of the strong acids such as

H C l, H_{2} S O_{4}, H N O_{3}, H B r o r H C l O_{4}

in dilute aqueous solutions. Reason: In dilute aqueous solution all strong acids donate a proton to water and are essentially 100 % ionised to produce a solution all strong acids

Q. Aqueous solution of FeCl3 is
strong acid
weak acid
strong base
weak base

Q. Assertion :Heat of neutralisation of strong acid and weak base is less than

57.1 k J

Reason: It is because weak bases do not ionise completely in aqueous solution. Therefore, some energy is required for their complete ionisation and that is why net energy released is less.

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