The solubility of acidic or basic compounds is pH dependent, and salt forms can be modified by design. Different salts show different equilibrium solubilities. However, the solubility of a strong acid salt is less affected by changes in pH than the solubility of a weak acid salt. In the latter case, when the pH is lower, the salt is hydrolyzed depending on the pH value and the pKa value, resulting in reduced solubility. The pKa value is a number that describes the acidity of a particular molecule. The lower the pKa value, the stronger the acid and the greater its ability to donate its protons.
Solubility is defined as the maximum amount of a substance that can be dissolved in a given amount of solvent at a given temperature. Solubility is a characteristic property of a particular solute-solvent combination, and different substances have greatly different solubility. Most substances become more soluble as temperature increases.
Acidic salts are more soluble in basic solutions (ie solutions with a pH greater than 7) and less soluble in acidic solutions. Basic salts are more soluble in acidic solutions (ie solutions with a pH less than 7) and less soluble in basic solutions. The solubility of neutral salts is not affected by a change in pH.
A pH scale is used to show whether a solution is acidic or basic. Sometimes the pH value falls outside of this range, although this is very rare. Acidic solutions have a pH less than 7, whereas basic solutions have a pH greater than 7.
When carboxylic acid is added to water, hydrogen bonds are formed between individual acid molecules and water molecules. These interactions make carboxylic acids soluble in water. Low carboxylic acids, i.e. up to four carbon atoms, are easily soluble in water due to hydrogen bonding.
By the way, all acids are soluble in water. Most of the known acids are soluble in water, whether inorganic such as hydrochloric acid or sulfuric acid, or organic acids such as acetic acid or benzoic acid.
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