Why-is -for-H2SO4-in water-

It can be noticed that This is because a neutral H2SO4 has a much higher tendency to lose a proton than the negatively charged . Thus, the former is a muc ...

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Standard XII

Chemistry

Enthalpy of Neutralisation

Why is for H...

Question

Why is for H₂SO₄ in water?

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Solution

It can be noticed that

This is because a neutral H₂SO₄ has a much higher tendency to lose a proton than the negatively charged . Thus, the former is a much stronger acid than the latter.

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Similar questions

Q. Why is

K a_{2} << K a_{1}

for

H_{2} S O_{4}

in water?

Q. Why is

K_{a 2}

≪

K_{a 1}

for

H_{2} S O_{4}

Q. For a polybasic acid, the dissociation constants have different value for each steps, e.g.,

H_{3} A ⇌ H^{+} + H_{2} A^{-}; K = K_{a_{1}}

H_{2} A^{-} ⇌ H^{+} + H A^{2 -}; K = K_{a_{2}}

H A^{2 -} ⇌ H^{+} + A^{3 -}; K = K_{a_{3}}

What is the observed trend of dissociation constants in succesive stage?

100 mL

0.1 M NaOH

solution is titrated with

100 mL

0.05 M H_{2} S O_{4}

solution. The

p H

of the resulting solution is :

(for H_{2} S O_{4}, K a_{1} = \infty, K a_{2} = 10^{- 2})

Q. If

K_{a_{1}}

and

K_{a_{2}}

H_{2} S O_{4}

are

10^{- 2}

and

10^{- 6}

respectively at a certain temperature, then :

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Why is for H₂SO₄ in water?

It can be noticed that

This is because a neutral H₂SO₄ has a much higher tendency to lose a proton than the negatively charged . Thus, the former is a much stronger acid than the latter.

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Why is for H2SO4 in water?

It can be noticed that This is because a neutral H2SO4 has a much higher tendency to lose a proton than the negatively charged . Thus, the former is a much stronger acid than the latter.

COURSES

EXAMS

CLASSES

EXAM PREPARATION

RESOURCES

COMPANY

FOLLOW US

FREE TEXTBOOK SOLUTIONS

STATE BOARDS

FOLLOW US

Why is for H₂SO₄ in water?

It can be noticed that

This is because a neutral H₂SO₄ has a much higher tendency to lose a proton than the negatively charged . Thus, the former is a much stronger acid than the latter.