Gaurang Tandon 8, 10 10 gold badges 55 55 silver badges bronze badges. Ivan Neretin Ivan Neretin These things may or may not coincide. Now to the point: sulfate ion does not hydrolyze in water, since it is a very weak base, like you said.
As for the acetate ion and its basicity: without knowing the pKa of acetic acid, you wouldn't know that. Show 3 more comments. Sign up or log in Sign up using Google. Sign up using Facebook. Sign up using Email and Password. Post as a guest Name.
Email Required, but never shown. Featured on Meta. Now live: A fully responsive profile. Related 2. Hot Network Questions. Skip to main content. The water should become orange. To one hydrometer cylinder add sodium acetate. The solution turns red showing that the solution is basic.
To another cylinder add sodium chloride. No color change is observed. Acid salts can also contain an acidic proton in the anion. Examples of anions with an acidic proton include:. 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.
Anilinium chloride : Anilinium chloride is an example of an acid salt. Some salts, such as ammonium bicarbonate NH 4 HCO 3 , contain cations and anions that can both undergo hydrolysis. Predict the pH of a solution of a salt containing cations and anions, both of which participate in hydrolysis.
Basic salts form from the neutralization of a strong base and a weak acid; for instance, the reaction of sodium hydroxide a strong base with acetic acid a weak acid will yield water and sodium acetate. Acid salts are the converse of basic salts; they are formed in the neutralization reaction between a strong acid and a weak base. The conjugate acid of the weak base makes the salt acidic.
For instance, in the reaction of hydrochloric acid a strong acid with ammonia a weak base , water is formed, along with ammonium chloride. The ammonium ion contains a hydrolyzable proton, which makes it an acid salt. The following is a more complicated scenario in which a salt contains a cation and an anion, both of which are capable of participating in hydrolysis.
A good example of such a salt is ammonium bicarbonate, NH 4 HCO 3 ; like all ammonium salts, it is highly soluble, and its dissociation reaction in water is as follows:. However, as we have already discussed, the ammonium ion acts as a weak acid in solution, while the bicarbonate ion acts as a weak base. The reactions are as follows:. Because both ions can hydrolyze, will a solution of ammonium bicarbonate be acidic or basic? We can determine the answer by comparing K a and K b values for each ion.
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