How Many Moles of HCl and HC3H5O3 to Achieve pH 3.77?

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To achieve a pH of 3.77 in a solution containing 0.1M NaC3H5O3, the required moles of HCl must be calculated using the Henderson-Hasselbalch equation, which is commonly applied in buffer solution problems. The discussion also mentions the addition of NaOH and the need to determine the moles of HC3H5O3 necessary to reach the same pH. The calculations involve understanding the dissociation of the compounds and their concentrations. Participants are encouraged to provide assistance with these calculations. The conversation emphasizes the importance of buffer chemistry in achieving specific pH levels.
dragonlady90
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Hi again,
I have another question. A 1L sol'n of a compound, NaC3H5O3 has an initial con'c of 0.1M. An unknown number of moles of Hcl is then added to bring a final solution to a Ph of 3.77. How many moles of HCl were added and what is the common name of this type of problem?

Can anyone pls help me and reply soon plssssss.

I have one more question...

1.8g of NaOH(s) was dissolved in one litre of H2O. A compound, HC3H5O3 was added. The final pH of the solution was 3.77. How many moles of HC3H5O3 are needed?

Plsssssssssss help me.
 
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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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