Write an equation for the reaction of Al2O3 with hydroxide ions.

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The discussion focuses on the chemical reaction between aluminum oxide (Al2O3) and hydroxide ions (OH^-). Participants propose two equations: Al2O3 + 2NaOH + 7H2O = 2Na[Al(OH)4(H2O)2] and Al2O3 + 2NaOH = 2NaAlO2 + H2O. There is a question regarding the role of sodium (Na) as a spectator ion in these reactions. Clarifications are sought on whether sodium can be included in the final equation. The conversation emphasizes the importance of accurately representing the chemical interactions involved.
tieu
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write an equation for the reaction of Al2O3 with hydroxide ions.

Al2O3 + OH^-1 ----> ?
 
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tieu said:
write an equation for the reaction of Al2O3 with hydroxide ions.

Al2O3 + OH^-1 ----> ?
Al2O3+2NaOH+7H2O=2Na[Al(OH)4(H2O)2]
or melting together
Al2O3+2NaOH=2NaAlO2+H2O
 
geo_alchemist said:
Al2O3+2NaOH+7H2O=2Na[Al(OH)4(H2O)2]
or melting together
Al2O3+2NaOH=2NaAlO2+H2O

ummm Na is spectator ion rite?? are u allowed to put that in??
 
[Al(OH)4(H2O)2]^-1
AlO2^-1
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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