a) Form a precipitate of barium chromate in two test tubes (Sce Test 1a). Remove the solution from the precipitate with a pipette Then,add to the first residue a solution of hydrochloric acid (2M) to the second one 2M solution of acetic acid. Explain how the effects of each acid on the precipitate differ. chaco OH

To form a precipitate of barium chromate, you can mix a solution of barium chloride with a solution of potassium chromate. The reaction will produce a yellow precipitate of barium chromate.<br /><br />In the first test tube, add hydrochloric acid (2M) to the precipitate of barium chromate. Hydrochloric acid is a strong acid and will completely dissociate in water. The hydrogen ions (H+) from the hydrochloric acid will react with the chromate ions (CrO4^2-) in the precipitate to form soluble chromic acid (H2CrO4). This will dissolve the precipitate.<br /><br />In the second test tube, add 2M solution of acetic acid to the precipitate of barium chromate. Acetic acid is a weak acid and will only partially dissociate in water. The hydrogen ions (H+) from the acetic acid will also react with the chromate ions (CrO4^2-) in the precipitate to form soluble chromic acid (H2CrO4). However, since acetic acid is a weak acid, the concentration of hydrogen ions in the solution will be lower compared to the hydrochloric acid solution. This means that the reaction will be slower, and the precipitate may not dissolve completely.<br /><br />In summary, both hydrochloric acid and acetic acid can dissolve the precipitate of barium chromate by forming soluble chromic acid. However, the rate of dissolution will be faster with hydrochloric acid due to its stronger acidity compared to acetic acid.