[cliverlong]

Hi,

   My textbook (Facer, A2 Chemistry - used for UK EdExcel specification) states on page 36 that Silicon Dioxide is a weakly acidic oxide because of the following reaction

SiO₂ + 2NaOH <> Na₂SiO₃ + H₂O (where <> represents the symbol "reversible")

Now, OK, I can see that the reaction is silicon dioxide plus an alkali gives water and a compound (sodium silicate?) that looks "salt-like"

However, everything I have read to date about acids (ignoring Lewis) states an acid is a proton donor.

My problem: where is the H⁺ in SiO₂ ? Because there isn't an H⁺, how can SiO₂  be an acid - even if its reaction with an alkali generates a salt  ? 

Salts, acids, bases 


Clive

[tflint89]

I think the Lewis acid/base theory has a great deal of pertinence in this case!

[Faisal]

Hi,

SiO₂ + 2NaOH <> Na₂SiO₃ + H₂O (where <> represents the symbol "reversible")

There is a reaction in between....btw your doing A-level edexcel...I am doing AS...maybe u can help me

[DevaDevil]

look at the reaction; in particular NaOH, a strong base.

Acting as a Bronsted acid can be by proton donation, or by hydroxide neutralization.
The latter is what happens in this case. As there is less OH^- after reaction, the pOH will be higher, and thus the compound less basic. in other words, the SiO₂ acted as an acid.

[Faisal]

I thought SiO3 simply becomes HSiO3^- in a solution and there is the H⁺ to make it a bronsted lowry acid..

[cliverlong]

I think the Lewis acid/base theory has a great deal of pertinence in this case!

I was afraid it was relevant.

The little I have read on Lewis acids made me think the definition of acids and bases is so broadened and that the concept applies to so many reactions that the "distinctive" nature of acids and bases is lost in the Lewis definition


Ta

Clive

[cliverlong]

look at the reaction; in particular NaOH, a strong base.

Acting as a Bronsted acid can be by proton donation, or by hydroxide neutralization.
The latter is what happens in this case. As there is less OH^- after reaction, the pOH will be higher, and thus the compound less basic. in other words, the SiO₂ acted as an acid.

I haven't read anywhere that "hydroxide neutralisation" of substance A defines A as an acid.

I see where you are coming from, because I used to think all bases were hydroxides and vice versa.

Can you provide a link for this definition of base "neutralisation" of an acid, where the acid does not contain a proton?


Thanks

Clive

[cliverlong]

I thought SiO3 simply becomes HSiO3^- in a solution and there is the H⁺ to make it a bronsted lowry acid..

You may well be right - but I'm not seeing the connection with the equation I wrote.

Can you clarify for me?


Ta,

Clive

[Faisal]

First of all SiO2 has to be dissolved in the solution so therefore it is:
SiO3+H2O->H⁺ + SiO4-(similar to SO3 dissolving in water)
This is can be written as HSO4-
It is this which reacts with NaOH and neutralizes...hope tht clarifies

[cliverlong]

First of all SiO2 has to be dissolved in the solution so therefore it is:
SiO3+H2O->H⁺ + SiO4-(similar to SO3 dissolving in water)
This is can be written as HSO4-
It is this which reacts with NaOH and neutralizes...hope tht clarifies

The question is about SiO₂ not SiO₃

SiO₂ does not dissolve in water - only in heated, strong alkali.

I don't see any connection between Silicon (Si Group 4) and Sulphur (S Group 6) as your argument suggest is relevant.

I think your argument is incorrect for both these reasons.

Please use sub-scripts and superscripts in equations on this forum as relevant - it makes them easier to read.


Regards


Clive

[DevaDevil]

silicon dioxide is relatively insoluble in water; 0.12 g/L


And:
" Neutralization is the reaction between an acid and a base, producing a salt and neutralized base; for example, hydrochloric acid and sodium hydroxide form sodium chloride and water:
        HCl(aq) + NaOH(aq) → H₂O(l) + NaCl(aq) "
Source: e.g. Wiki

In this case substitute SiO₂ for HCl, and you see different products. However, the principle is the same. The SiO₂ acts as the acid in the neutralization reaction.

[Faisal]

Oh right...SiO₂
this is the rx I think it shud be...
SiO₂+H₂O->SiO₃^- + 2H⁺ which can be written as H₂SiO₃

[Faisal]

Maybe cuz its insolube thts y it forms only a weak acid....