Question

In general, for a diprotic acid, Ka1 >> Ka2. This is reasonable because chose one: (1()Ka1 xKa2 = K for the combined equilibrium. (2)Diprotic acids have 2 protons to donate (3) It is more difficult to remove a proton from the -1 ion that it is from the neutral acid. (4)Ka1 corresponds to a strong acid while Ka2 corresponds to a weak acid. (5)None of the above is correct

Answer 1

For a general diprotic acid , Ka1 >> Ka2 because of the following reason:

• It is more difficult to remove a proton from -1 ion than a neutral acid.

Let us consider a diprotic acid AH2.

$\sf{AH_{2} \overset{ka_{1}}\longrightarrow \: A{H}^{ - } + {H }^{ + } }$

$\sf{A{H}^{ - } \overset{ka_{2}}\longrightarrow \: {A}^{ - } + {H }^{ + } }$

$\boxed{ \sf{ \red{ \huge{ka_{1} > > ka_{2}}}}}$

The proton (H+) can be easily released from the neutral acid (AH2) . However , a uni-negative ion or conjugate base (AH-) doesn't allow the release of another proton very easily.

Hope It Helps.

Answer 2

Explanation:

For a general diprotic acid , Ka1 >> Ka2 because of the following reason:

It is more difficult to remove a proton from -1 ion than a neutral acid.

Let us consider a diprotic acid AH2.

\sf{AH_{2} \overset{ka_{1}}\longrightarrow \: A{H}^{ - } + {H }^{ + } }AH

2

⟶

ka

1

AH

−

+H

+

\sf{A{H}^{ - } \overset{ka_{2}}\longrightarrow \: {A}^{ - } + {H }^{ + } }AH

−

⟶

ka

2

A

−

+H

+

\boxed{ \sf{ \red{ \huge{ka_{1} > > ka_{2}}}}}

ka

1

>>ka

2

The proton (H+) can be easily released from the neutral acid (AH2) . However , a uni-negative ion or conjugate base (AH-) doesn't allow the release of another proton very easily.

Hope It Helps.