Silver Bromate Solubility

Silver bromate (AgBrO3) is a sparingly soluble salt in water, which means it only dissolves to a limited extent. The solubility of silver bromate depends on several factors such as temperature, pH, and the presence of other substances.

At room temperature, the solubility of silver bromate in water is approximately 0.5 grams per liter. This means that only a small amount of silver bromate will dissolve in water at this temperature. As the temperature increases, the solubility of silver bromate also increases. At around 70°C, the solubility of silver bromate reaches about 4 grams per liter.

The solubility of silver bromate can also be influenced by the pH of the solution. In acidic solutions, silver bromate is more soluble than in neutral or alkaline solutions. This is because the bromate ion (BrO3-) reacts with hydrogen ions (H+) to form the more soluble hypobromous acid (HOBr) and water:

BrO3- + H+ → HOBr + H2O

In contrast, in alkaline solutions, the bromate ion undergoes hydrolysis to form less soluble bromide ions (Br-) and hydroxide ions (OH-):

BrO3- + 6OH- → Br- + 3H2O

The presence of other substances in the solution can also affect the solubility of silver bromate. For example, the presence of silver nitrate (AgNO3) can increase the solubility of silver bromate due to the common ion effect. When both Ag+ and BrO3- ions are present in solution, the equilibrium shifts towards the formation of the less soluble silver bromate:

Ag+ + BrO3- ↔ AgBrO3(s)

However, if excess silver nitrate is added to the solution, the concentration of Ag+ ions will increase, which will drive the equilibrium towards the dissolution of more silver bromate to maintain a constant Ksp value.

In summary, the solubility of silver bromate is influenced by temperature, pH, and the presence of other substances in the solution.