Calculate the equilibrium concentration of hydrogen ions

AI Thread Summary
To calculate the equilibrium concentration of hydrogen ions, apply the ICE table method to the dissociation reaction of the weak acid HA. Identify the species involved: HA, H+, and A-. The stoichiometry indicates that for each mole of H+ produced, one mole of HA is consumed. Express the concentrations of HA, H+, and A- in terms of H+ as the unknown variable. This approach simplifies finding the pH, which is the ultimate goal of the calculation.
fender1984
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Thank you for the link Borek but I'm still lost
 
You have to directly apply the ICE table method to your case.

What is your HA? A-?

Basically it is about stoichiometry - from the dissociation reaction you can easily see that for each mole/molecule of A- (H+) produced, one mole/molecule of HA is consumed. You just have to express concentrations of all three substances involved (HA, H+, A-) in terms of one unknown - best approach is to use H+ as the unknown, as you are asked about pH.
 
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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