-3
$\begingroup$

Sodium carbonate is used in pools to raise pH. From my understanding, it would dissociate in water like so:

$$\ce{Na2CO3 <=> 2 Na+ + CO3^2-}$$

To raise pH, doesn't it have to absorb hydrogen ion/s? If so then wouldn't it just form carbonic acid that would then just dissociate again?

$\endgroup$
  • $\begingroup$ It's all about equlibrium. Try to write the corresponding equation(s) for hydrolysis and see what dissociates better, sodium hydroxide or hydrocarbonate. Also, the term "to absorb" looks weird in this context. $\endgroup$ – andselisk Jul 14 at 6:30
-1
$\begingroup$

You have the equilibrium in water: $$\ce{H2O <=> H+ + OH-}$$ The protons are removed from the equilibrium: $$\ce{H+ + CO3^2- <=> HCO3-}$$ Now you have more $\ce{OH-}$ in the solution which increases the pH.

$\endgroup$

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.