Which of the following will be more soluble in an acidic solution than in pure water?
SrSO4
CsClO4
CuCN
Ni(OH)2
AgCl
Please help explain why! I've tried submitting the ones that are insoluble in water and it was wrong. I know it has something to do with basic anions but I don't know how to tell if an anion is basic or not :/
came from the future thanks bob
Ah, the solubility dance! Let's put on our spectacles and figure this out with a sprinkle of humor, shall we?
Out of the options listed, CuCN and Ni(OH)2 will be more soluble in an acidic solution than in pure water. Why, you ask? Well, acidic conditions tend to increase the solubility of compounds that contain basic anions.
Now, let's break it down like an acrobat on a tightrope. CuCN contains CN-, which is a basic anion. So, imagine an acid comes along and gives CN- a high-five, turning it into HCN gas. As a result, copper cyanide (CuCN) will dissolve more readily in an acidic solution.
Coming to Ni(OH)2, it contains OH-, which is quite the comedienne—acting both as a basic anion and a base itself. In an acidic solution, this hydroxide (OH-) gets in a tizzy, grabs an H+ ion from the acid, and turns into H2O. With the hydroxide neutralized, the nickel hydroxide (Ni(OH)2) will be more soluble in an acidic solution.
As for SrSO4, CsClO4, and AgCl, they just aren't the life of the party in an acidic environment. They don't have basic anions, so they would rather hang out in pure water, sipping on their non-soluble cocktails.
Remember, a little bit of humor and a dash of understanding can take you a long way in deciphering science!
To determine which compound is more soluble in an acidic solution than in pure water, we need to look at the behavior of the anions in each compound. Anions that can act as bases are more likely to be soluble in acidic solutions.
Now, let's analyze each of the compounds:
1. SrSO4 (strontium sulfate): This compound contains the sulfate anion (SO4^2-). The sulfate ion is a neutral anion and does not exhibit basic properties. Therefore, the solubility of SrSO4 does not significantly increase in an acidic solution compared to pure water.
2. CsClO4 (cesium perchlorate): The perchlorate anion (ClO4^-) is a strongly acidic anion. In pure water, CsClO4 is already highly soluble. However, since ClO4^- is an acidic anion, the solubility of CsClO4 may slightly increase in an acidic solution. Therefore, CsClO4 will be more soluble in an acidic solution than in pure water.
3. CuCN (copper(I) cyanide): In this compound, the cyanide anion (CN^-) is involved. Cyanide ions tend to act as weak bases. Hence, the solubility of CuCN may increase in an acidic solution compared to pure water.
4. Ni(OH)2 (nickel(II) hydroxide): The hydroxide anion (OH^-) is a strong base. In pure water, Ni(OH)2 is insoluble due to the formation of a precipitate. In an acidic solution, the hydroxide ions will react with the acid to form water and, ultimately, decrease the concentration of OH^- ions. This shift in equilibrium favors the dissolution of Ni(OH)2, leading to increased solubility.
5. AgCl (silver chloride): This compound contains the chloride anion (Cl^-) which is a neutral anion and does not exhibit basic properties. Therefore, the solubility of AgCl does not significantly increase in an acidic solution compared to pure water.
In summary, the compounds that are more soluble in an acidic solution than in pure water are CsClO4, CuCN, and Ni(OH)2.
To determine which of the given compounds will be more soluble in an acidic solution compared to pure water, we need to consider the nature of the anions present in each compound.
In an acidic solution, the concentration of hydrogen ions (H+) is higher than in pure water. These hydrogen ions can interact with certain anions, forming water molecules and reducing the concentration of the anions, thus increasing the solubility of the compound.
To identify if an anion is basic or not, we need to consider its conjugate acid. A conjugate acid is formed when a base accepts a proton (H+). If an anion's conjugate acid is weak, it means the anion is a strong base and can easily accept a proton to form a stronger acid. In comparison, if the conjugate acid is strong, the anion is a weak base and less likely to accept a proton.
Let's apply this knowledge to the given compounds:
1. SrSO4:
The sulfate ion (SO4^2-) has a weak conjugate acid (HSO4-), indicating that it is a strong base. Therefore, SrSO4 is insoluble in both pure water and acidic solution.
2. CsClO4:
The perchlorate ion (ClO4-) has a weak conjugate acid (HClO4). CsClO4 is highly soluble in both pure water and acidic solution.
3. CuCN:
The cyanide ion (CN-) has a relatively strong conjugate acid (HCN). Despite this, CuCN is still insoluble in both pure water and acidic solution due to other factors affecting its solubility.
4. Ni(OH)2:
The hydroxide ion (OH-) has a very strong conjugate acid (H2O). Therefore, Ni(OH)2 is insoluble in pure water. However, in an acidic solution, the excess hydrogen ions (H+) can react with the hydroxide ions, forming water molecules (H2O), thus increasing the solubility of Ni(OH)2.
5. AgCl:
The chloride ion (Cl-) has a strong conjugate acid (HCl). AgCl is insoluble in both pure water and acidic solution since its lattice energy is large and the forces holding the ions together are stronger than those formed by the interaction with water molecules.
By considering the nature of the anions and their conjugate acids, we find that CsClO4 and Ni(OH)2 will be more soluble in an acidic solution compared to pure water.
SrSO4, CuCN, and Ni(OH)2 are more soluble in acidic solution than in pure water.
If you don't understand what basic anions are, then look at it this way.
Which anions will hydrolyze with H2O to form a WEAK acid when added to H^+; i.e., an acid that has a Ka (not a strong acid).
Take them one at a time.
SO4^2- + H^+ ==> HSO4^-
HSO4^- is k2 for H2SO4; there is no k1 since H2SO4 is a strong acid for the first H.
ClO4^- + H^+ ==> HClO4
NOPE Won't go because HClO4 is a strong acid.
CN^- + H^+==> HCN
HCN is a weak acid; it has a Ka.
OH^- + H^+ ==>H2O
H2O is a weak electrolyte; it has a Ka/Kb but usually we only talk about Kw.
Cl^- + H^+ ==> HCl
NOPE. HCl is a strong acid; it has no Ka.