Determine whether of not each compound will be more soluble in acidic soln than in pure water. Explain.
A). Hg2Br2
B). Mg(OH)2
C). CaCO3
D). AgI
I think acid, neutral,acid,neutral ???
Help please!:) thAnks
An acid, at least for this discussion contains H^+. So what will that combine with in a salt? It will combine with the anion, of course. So if the anion will react with the H^+, then it will be more soluble in an acid.
Hg2Br2 will give HBr but that is a strong acid and will ionize 100%; no reaction. solubility not increased.
Mg(OH)2. Add acid, it reacts with the OH part to make water, solubility increased by adding acid.
I'll leave the other two for you.
Determine whether or not AgI will be more soluble in acidic solution than in pure water.
Let's evaluate each compound individually and determine whether it will be more soluble in an acidic solution than in pure water:
A) Hg2Br2 (Mercury(I) bromide):
Hg2Br2 is insoluble in pure water. However, it can dissolve in an acidic solution. This is because in an acidic solution, protons (H+) are available, which can react with the compound to form soluble species.
B) Mg(OH)2 (Magnesium hydroxide):
Mg(OH)2 is insoluble in pure water. Its solubility is highly dependent on the pH of the solution. In an acidic solution, the hydroxide ions (OH-) will react with the available protons (H+), and solubility will increase. However, in neutral or basic solutions, the OH- ions will compete with OH- from Mg(OH)2, reducing its solubility.
C) CaCO3 (Calcium carbonate):
CaCO3 is insoluble in pure water. Its solubility is inversely proportional to the concentration of carbonate (CO3^2-) and bicarbonate (HCO3-) ions, which increase with decreasing pH. Therefore, calcium carbonate will exhibit slightly higher solubility in acidic solutions compared to pure water.
D) AgI (Silver iodide):
AgI is insoluble in both pure water and acidic solutions. Its solubility does not depend on the pH of the solution. Therefore, AgI will not be more soluble in an acidic solution than in pure water.
In conclusion:
A) Hg2Br2 will be more soluble in an acidic solution.
B) Mg(OH)2 will be more soluble in an acidic solution compared to a basic or neutral solution.
C) CaCO3 will have slightly higher solubility in an acidic solution compared to pure water.
D) AgI solubility is not influenced by pH and will not be more soluble in an acidic solution.
To determine whether a compound will be more soluble in an acidic solution compared to pure water, you need to consider the reaction that takes place between the compound and the acid.
Let's analyze each compound:
A) Hg2Br2 (Mercury(I) bromide)
In the presence of excess acid, the mercury(I) bromide can react with the acid to form a soluble mercury(II) complex. Thus, Hg2Br2 will be more soluble in an acidic solution compared to pure water.
B) Mg(OH)2 (Magnesium hydroxide)
Magnesium hydroxide is a strong base and has low solubility in water. In an acidic solution, the acid can react with the hydroxide ions resulting in the formation of water. This reaction decreases the concentration of hydroxide ions and helps in dissolving magnesium hydroxide. Therefore, Mg(OH)2 will be more soluble in an acidic solution.
C) CaCO3 (Calcium carbonate)
Calcium carbonate is insoluble in pure water because it is a slightly soluble salt. In an acidic solution, the acid can react with the carbonate ions, producing carbon dioxide gas and water. This decreases the concentration of carbonate ions and drives the equilibrium towards dissolving calcium carbonate. Hence, CaCO3 will be more soluble in an acidic solution than in pure water.
D) AgI (Silver iodide)
Silver iodide has low solubility in water. It is insoluble in pure water and also in acidic solutions. Therefore, the solubility of AgI remains the same in both pure water and an acidic solution.
So, the correct solubility ranking would be:
A) More soluble in acidic solution than in pure water.
B) More soluble in acidic solution than in pure water.
C) More soluble in acidic solution than in pure water.
D) Equally insoluble in both pure water and acidic solutions.