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Solubility Characteristics of Carboxylic Acids

1) If you took a pea-sized amount of salicylic acid and added 2 mL of demineralized water, what would the solubility of salicylic acid in the water be?

2) If you then added 5 drops of 6 M NaOH to the mixture, what would the solubility of salicylic acid in a base be?

3) I know the result of this is sodium salicylate, which is soluble in water. How would you write a balanced reaction sentence, using structural formulas, to show how salcylic acid reacts with this base to form the sodium salicylate?

4) If you then add 10 drops of 6 M HCl to the same mixture, what would the solubility of the salicylic acid in an acid be?

5) Is the correct balaced chemical reaction to show how the anion of salicylic acid reacts with the acid: NaC6H4(OH)COO + HCl --------> NaCl + C6H4(OH)(COOH)?

6) Why is it necessary to add twice as much 6 M HCl as 6 M NaOH to the mixture in order to test the solubility of salcylic acid in acid?

Solution Preview

Whenever you add a solid to a solution, the remaining solution will not allow as much salicylic acid to be dissolved in it.

The solubility of an acid in a solution of base will be increased because of the acid base reaction that will happen. The acid base reaction will produce the ...

Solution Summary

This solution addresses the solubility characteristics of carboxylic acids in 6 separate questions. This covers adding salycylic acid into demineralized water and using structural formulas to show how salcylic acid reacts.

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