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Which of the following salts is NOT more soluble in acidic solution than in pure water?

A. ZnS
B. AgCN
C. Ba3(PO4)2
D. ZnCO3
E. BiI3

The answer is E, but I don't know why or how I would go about answering a question like this. What would I have to consider to determine this?

User Icon for DrBob222 DrBob222 answered
11 years ago

Since acid is H^+ you look for an anion that combines with H^+ to give a WEAK acid (one that has an ionization constant).

ZnS gives H^+ + S^2- ==> HS^- which is k2 for H2S.
AgCN gives H^+ + CN^- ==> HCN which has a Ka.
Ba3(PO4)2 gives H^+ + PO4^3- ==> HPO4^2- which is k3 for H3PO4.
ZnCO3 gives H^+ + CO3^2- ==> HCO3^- which is k2 for H2CO3.
BiI3 gives H^+ + I^- == HI WHICH HAS NO k VALUE BECAUSE IT IS A STRONG ACID; IE., IONIZED 100%.

User Icon for Clown Bot Clown Bot answered
1 year ago

Well, well, my inquisitive friend! Let's dive into this question together and have some fun figuring out the answer.

To determine which salt is NOT more soluble in acidic solution than in pure water, we need to consider a few factors. When a salt dissolves in water, it dissociates into its constituent ions. In an acidic solution, we have the presence of extra H+ ions, which can potentially influence the solubility of salts.

Now, let's check out the options:

A. ZnS: Hmmm, I bet this little guy dissolves more in an acidic solution because Zn2+ ions love to hang out with those H+ ions.

B. AgCN: Silently lurking in the corner, it's one slippery silver cyanide. Well, Ag+ ions would still be attracted to H+ ions in an acidic solution, so it should be more soluble too.

C. Ba3(PO4)2: Oh, boy! This one looks complicated, doesn't it? But remember, we're looking for the salt that's not more soluble in acidic solution. Phosphate ions love being surrounded by water molecules, but I don't think the acidic environment will make them more willing to leave their aquatic friends.

D. ZnCO3: Zinc carbonate, oh my! Carbonate ions can get feisty in acidic solutions, so I'm thinking this one will be more soluble too.

E. BiI3: Ah, the elusive bismuth triiodide. Now, here's the trickster. Bismuth compounds are known to be quite insoluble, even in acidic solutions. So, this little fella stands out from the crowd and is our answer!

And there you have it! By considering the behavior of ions and the solubility characteristics of the salts, we deduce that option E, BiI3, is NOT more soluble in acidic solution than in pure water. Bravo, my friend!

User Icon for Step-by-Step Bot Step-by-Step Bot answered
1 year ago

To determine which of the given salts is NOT more soluble in an acidic solution than in pure water, you need to consider the solubility behavior of salts in different solvent conditions.

The solubility of a salt in a particular solvent is determined by the relative strengths of the attractive forces between the ions in the salt and the solvent molecules. In the case of acidic solutions, the presence of excess H+ ions can significantly affect the solubility of certain salts.

Here are some key principles to consider:

1. Common Ion Effect: If a solution already contains a common ion from the salt's dissociation, the solubility of that salt in the solution decreases. This is due to the Le Chatelier's principle, as the excess of one ion in the solution causes the equilibrium to shift towards the solid salt.

2. Acid-Base Reactions: Some salts can undergo acid-base reactions with the H+ ions in acidic solutions. These reactions can either form more insoluble salts or produce weak acids, reducing the overall solubility of the salt.

Now let's analyze each salt option:

A. ZnS: Zinc sulfide (ZnS) does not contain any acidic or basic ions that could undergo acid-base reactions. Therefore, the solubility of ZnS is not affected by the presence of H+ ions in an acidic solution. It remains equally soluble in both acidic and pure water.

B. AgCN: Silver cyanide (AgCN) contains the CN- ion, which is known to form weak acids in acidic solutions. This can reduce the overall solubility of AgCN in acidic conditions compared to pure water.

C. Ba3(PO4)2: Barium phosphate (Ba3(PO4)2) does not contain any acidic or basic ions that could undergo acid-base reactions. The solubility of Ba3(PO4)2 remains relatively constant in both acidic and pure water conditions.

D. ZnCO3: Zinc carbonate (ZnCO3) contains the CO3 2- ion, which can undergo acid-base reactions with H+ ions in acidic solutions. These reactions produce carbonic acid, H2CO3, which decomposes into water and carbon dioxide. The formation of carbonic acid reduces the overall solubility of ZnCO3 in acidic conditions compared to pure water.

E. BiI3: Bismuth iodide (BiI3) does not contain any acidic or basic ions that could undergo acid-base reactions. Therefore, the solubility of BiI3 is not affected by the presence of H+ ions in an acidic solution. It remains equally soluble in both acidic and pure water.

Based on the above analysis, the salt that is NOT more soluble in an acidic solution than in pure water is E. BiI3.

User Icon for Explain Bot Explain Bot answered
1 year ago

To determine which salt is NOT more soluble in acidic solution than in pure water, you need to consider the solubility behavior of salts in different conditions.

In general, the solubility of salts can be influenced by factors such as pH, temperature, and the presence of other ions. When it comes to comparing solubilities in acidic solutions and in pure water, you should consider the behavior of the ions involved.

In an acidic solution, the concentration of hydrogen ions (H+) increases, which can compete with the cations of the salt, affecting their solubility. Based on this, salts with cations that can react with the H+ ions and form insoluble compounds would be less soluble in acidic solutions than in pure water.

Using this information, let's consider each salt option and try to eliminate them one by one:

A. ZnS: Zinc sulfide (ZnS) is a slightly soluble salt in water and is not expected to form insoluble compounds with H+ ions. Therefore, its solubility may not differ significantly between acidic solutions and pure water.

B. AgCN: Silver cyanide (AgCN) is sparingly soluble in water, and it is not likely to form insoluble compounds with H+ ions. So, its solubility might not differ significantly between acidic solutions and pure water.

C. Ba3(PO4)2: Barium phosphate (Ba3(PO4)2) is less soluble in water, and it can form insoluble compounds with some H+ ions, leading to lower solubility in acidic solutions compared to pure water.

D. ZnCO3: Zinc carbonate (ZnCO3) is slightly soluble in water but can react with H+ ions to form insoluble compounds. Thus, its solubility can be expected to decrease in acidic solutions compared to pure water.

E. BiI3: Bismuth triiodide (BiI3) is insoluble in water, and it is unlikely to react with H+ ions to form insoluble compounds. Consequently, its solubility is expected to be similar in acidic solutions and pure water.

Therefore, based on the analysis above, the salt that is NOT more soluble in acidic solution than in pure water is E. BiI3.