Compute the concentration of the acetate ion

Reference no: EM13132341

Calculating the concentration of the acetate ion when dissociation of acetic acid occurs in water and over varying pH conditions?
I am a process engineer in wood pulping operation in which we use steam to digest hardwood chips. This is non-chemical pulping, but the residual "wood juice" for lack of a better term has a pH as low as 3.0 and contains significant concentrations of acetic acid.

Now consider that acetic acid in a water solution in which the pH is 3.0. Assume more water is added to the solution so that via dilution the pH increases to 4.5, and then again to 6.5.

How would I calculate the change in the acetate ion concentration at pH 3.0, 4.5, and 6.5?

I know the acetate ion would have a strong attraction to cations in the water solution such as Na, Ca, and Zn if present....would you think that the presence of the acetate ion would inhibit downstream ionic bonding of highly anioinc resins and waxes that we put in the wood pulp after steaming?

Please help me understand the logic and the relevant calculations and the goods and bads about acetate concentrations in a water solution.

Reference no: EM13132341

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