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Why does EDTA dissolve at pH 8? Im using NaOH to dissolve EDTA by raising the pH, and need a molecular level explanation of why this works.
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+ Sodium hydroxide
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Alan Cooper
Why does EDTA dissolve at pH 8? Im using NaOH to dissolve EDTA by raising the pH, and need a molecular level explanation of why this works.
ESTA is more soluble in water in its salt form (like sodium EDTA, disodium ESTA, trisodium EDTA, tetrasodium EDTA) than when when it is in its protonated acidic form. This is true for many acids.
So increasing the PH of the solution helps dissolve EDTA.
Note that EDTA is tetravalent, meaning that it has four carboxylic acids that can be titrated with your sodium hydroxide giving increasing proportions of sodium carboxylate chemical functions by increasing the pH. This can be calculated using the known pKa values of EDTA.
ESTA is more soluble in water in its salt form (like sodium EDTA, disodium ESTA, trisodium EDTA, tetrasodium EDTA) than when when it is in its protonated acidic form. This is true for many acids.
So increasing the PH of the solution helps dissolve EDTA.
Note that EDTA is tetravalent, meaning that it has four carboxylic acids that can be titrated with your sodium hydroxide giving increasing proportions of sodium carboxylate chemical functions by increasing the pH. This can be calculated using the known pKa values of EDTA.
ESTA is more soluble in water in its salt form (like sodium EDTA, disodium ESTA, trisodium EDTA, tetrasodium EDTA) than when when it is in its protonated acidic form. This is true for many acids.
So increasing the PH of the solution helps dissolve EDTA.
Note that EDTA is tetravalent, meaning that it has four carboxylic acids that can be titrated with your sodium hydroxide giving increasing proportions of sodium carboxylate chemical functions by increasing the pH. This can be calculated using the known pKa values of EDTA.
ESTA is more soluble in water in its salt form (like sodium EDTA, disodium ESTA, trisodium EDTA, tetrasodium EDTA) than when when it is in its protonated acidic form. This is true for many acids.
So increasing the PH of the solution helps dissolve EDTA.
Note that EDTA is tetravalent, meaning that it has four carboxylic acids that can be titrated with your sodium hydroxide giving increasing proportions of sodium carboxylate chemical functions by increasing the pH. This can be calculated using the known pKa values of EDTA.
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At pH 8 2 of the 4 carboxyl groups will be almost completely dissociated, crating an ionic compound which will water soluble.
At pH 8 2 of the 4 carboxyl groups will be almost completely dissociated, crating an ionic compound which will water soluble.
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