## 6c.19 f

Acidity $K_{a}$
Basicity $K_{b}$
The Conjugate Seesaw $K_{a}\times K_{b}=K_{w}$

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Fdonovan 3D
Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

### 6c.19 f

Which is the strongest acid, H2CO3 or H2GeO3? (Justify your answer)

In the answer key, it says H2CO3 is the stronger acid because C is more electronegative. However, I thought that when comparing acids in which the only difference is the central atom, you compare the bond strengths for elements in the same group. Since Ge and C come from the same group (not the same period), shouldn't the justification come from comparing the bond strengths, not the electronegativity?

Ethan Lam 4A
Posts: 69
Joined: Thu Jul 11, 2019 12:17 am

### Re: 6c.19 f

Electronegativity and bond strengths both play a factor in determining acid strength. Since it is more electronegative, it becomes more polar which makes it easier to dissociate.

Ruby Richter 2L
Posts: 103
Joined: Thu Jul 25, 2019 12:17 am

### Re: 6c.19 f

So, in this case, the difference in electronegativity would dominate over the difference in bond strength?

Yun Su Choi 3G
Posts: 61
Joined: Wed Sep 30, 2020 10:09 pm

### Re: 6c.19 f

What does it mean when high electronegativity makes an O-H bond more polar?
Does it mean that the electron density on O is shifted to a high electronegative atom that causes H to have a more partial positive charge?

John Calonia 1D
Posts: 67
Joined: Wed Sep 30, 2020 9:49 pm

### Re: 6c.19 f

I believe the more elctronegative one is more able to stabilize the resulting ion so it is easier for the acid to lose its hydrogen when put into solution.

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