Balancing Acid-Base Reactions with Acetic Acid and Ethylene Diamine

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The discussion focuses on the acid-base reaction between acetic acid (C2H4O2) and ethylene diamine (C2H8N2), leading to the formation of a salt. Participants explore the balanced chemical equation, noting that both amine groups in ethylene diamine can accept protons. There is uncertainty about the correct product formulation, with suggestions of ionization resulting in C2H3O2- and C2H9N2+. The conversation highlights the complexity of the reaction, emphasizing that acetic acid is a weak acid and ethylene diamine a weak base, necessitating consideration of acid-base equilibria for accurate solution characterization. Overall, the interaction results in the formation of a salt, but precise details depend on the equilibrium states of the reactants.
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Consider the Acid-Base reaction of acetic acid (C2H4O2) with ethylene diamine (C2H8N2) to form the corresponding salt. Then the structural formulas for acetic acid and ethylene diamine were drawn below this.
Write a balanced chemical equation for the reaction, noting both amine groups can accept a proton.

I know that acid + base = water + salt

I'm not sure if what I've come up with is right or not... I don't remember the teacher ever going over anything like this...

C2H4O2 + C2H8N2 --> 2H2O + C4H8N2
 
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No water in products, amine groups get protonated.
 
Would the product be C2H3O2- + C2H9N2+.. and would this ionize and form a salt?
 
Diamine can get protonated twice.

Basically you will have a salt C2H10N2(2+)(2C2H3O2(-))2.

However, that's not whole truth - acetic acid is a weak acid, ethylene diamine is a weak base, so if you will need precise information about the solution, you will have to take all acid/base equilibria into accounts.
 
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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