Which produce acidic solutions in water

Each of these anions contains a proton that will weakly dissociate in water. Therefore, salts containing these anions—such as potassium bisulfate—will yield weakly acidic solutions in water. From the previous concept, we know that salts containing the bicarbonate ion HCO 3 — are basic, whereas salts containing bisulfate ion HSO 4 — are acidic. Boundless vets and curates high-quality, openly licensed content from around the Internet. This particular resource used the following sources:.

Skip to main content. Acids and Bases. Search for:. Salts that Produce Acidic Solutions. Key Points Acid salts contain a hydrolyzable proton in the cation, anion, or both; for instance, the salt ammonium bisulfate NH 4 HSO 4 contains an acidic proton in both the cation and the anion. The Strong bases have conjugate acids of negligible acidity. The strong base, NaOH, dissociates completely in water. The reverse reaction does not occur.

It has no basic activity. Any combination of these anions and cations will produce neutral solutions. Salts that produce Basic solutions.

Weak acids can be neutralized by strong bases to form water and salts. For example, As we have just learned, HF, a weak acid, does not dissociate completely in water. How can a strong base neutralize the HF completely, when only a small portion of the acid exists in the ionized form? LeChatelier's Principle. It will react with the OH - from the strong base to form water. When this happens, we have removed one of the products of the equilibrium system.

Addition of the strong base will drive the complete dissociation of even a weak acid. In this case,. This will produce 5. NaF is the salt formed in this neutralization reaction.

For example, F - is the conjugate base or the weak acid, HF. This is called a hydrolysis reaction, because a molecule of water is broken up. Why does this happen? Remember that HF was characterized as a weak acid. Most of the HF, in water, exists in the undissociated form, HF. When the salt, NaF, is dissolved in water, the F - ion is created.

In this reaction, OH - is the strongest base. This means that its conjugate acid, H 2 O is the weakest acid in the system.

The equilibrium will favor the reactants. Example 1 A solution is made by adding solid NaClO to enough water to make 2. If the solution has a pH of What reaction is taking place? So, this is a weak base equilibrium problem, like the previous example.

Initial X 0. Equilibrium X — x x x. The assumptions are O. The dissociation is 3. In this example, it was important to recognize that ClO - was the conjugate base of a weak acid. The relationship between acids and their conjugate bases is shown, below, for some common acids and bases. K a Acid Base K b. The K b can always be calculated from the K a and vice versa.