(1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.233 M aqueous acetylsalicylic acid (aspirin) and aniline are mixed. It is not necessary to include states such as (aq) or (s).

Complete Question

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 1)  The ionic equation is  

2

  At equilibrium The  aniline will be  favored

3

The pH  of the solution is  

Explanation:

  From the question we are told that

      The concentration of aspirin is  

      The acid dissociation  constant for aspirin is  

       The base  dissociation constant for aniline is  

The molecular formula for aspirin  is  

The molecular formula for aniline  is  

So the net ionic reaction is  

Generally pKa is mathematically evaluated as

Generally pKb is mathematically represented as

Generally

                    pKa + pKb = 14

So for the triethylammonium salt  produced the pKa is

 As a result of the   pKa  of  aspirin being lower that that of  triethylammonium salt at equilibrium it implies that  aniline would be favored

The pH of the solution is mathematically represented as

           Since they are of equal mole

Where pKw is the pKw of water which has a value of 14

Check the explanation

Explanation:

Ka for aspirin =

Therefore,

pKa = - log() = 3.52

Kb for Triethylamine = 5.2 x 10-4

Therefore,

pKb = -log() = 3.28

We have,

pKa + pKb = 14

pKa = 14 – pKb = 10.71

pKa for the triethylammonium salt = 10.71

The net ionic reaction can be written as,

     ⇒      

Since pKa of Aspirin is lower (3.52) than that of triethylammonium salt (10.71), at equilibrium triethyl amine will be favored.

pH of equimolar solution can be calculated as,

pH = ½ (pKw + pKa –pKb) = ½ (14 + 3.52 – 3.28) = 7.12

pH of resulting solution = 7.12

i know insulin is primary but i dont know the others im sorry

explanation:

b.

the accuracy of the data.