Consider the ionization constants

cyanic acid (HOCN) : Ka= 3.5×10−4; ammonia (NH3): Kb= 1.8×10−5. A solution
of ammonium cyanate (NH4OCN) is
1. acidic, because the cation and the anion hydrolyze to the same extent.
2. acidic, because the anion hydrolyzes to a greater extent than the cation.
3. basic, because the cation hydrolyzes to a greater extent than the anion.
4. basic, because the anion hydrolyzes to a greater extent than the cation.
5. neutral, because the cation hydrolyzes to a greater extent than the anion.
6. neutral, because the anion hydrolyzes to a greater extent than the cation.
7. neutral, because NH4OCN is a weak
base/weak acid salt.
8. basic, because the cation and the anion hydrolyze to the same extent.
9. acidic, because the cation hydrolyzes to a greater extent than the anion.
10. neutral, because the cation and the anion hydrolyze to the same extent.

acidic, because the cation hydrolyzes to a

greater extent than the anion.

Michael is correct. I tried it.

(H^+) for a salt of a weak acid and a weak base = sqrt(KwKa/Kb). Solve for (H^+) and you have your answer.

11. None of the above. It's actually a clown party solution, where the cation, the anion, and all the molecules sing and dance together, making it a fun and festive neutral solution! 🎉🤡

To determine the acidity or basicity of a solution of ammonium cyanate (NH4OCN), we need to consider the ionization constants of its constituent ions, ammonium (NH4+) and cyanate (OCN-). The ionization constants, Ka and Kb, respectively, represent the extent to which an acid (or its conjugate base) or a base (or its conjugate acid) ionizes in water.

In this case, we have the ionization constant for cyanic acid (HOCN) and ammonia (NH3), not for ammonium cyanate directly. However, we can use these values to infer the relative acidity or basicity of NH4OCN.

1. To determine if the solution is acidic, basic, or neutral, we need to compare the hydrolysis of the cation (NH4+) and the anion (OCN-).

2. The hydrolysis of the cation NH4+ can be assessed using the ionization constant of its conjugate acid, ammonia (NH3): Kb = 1.8×10−5. Ammonium ions can accept a proton from water, resulting in the production of hydronium ions (H3O+) and the base NH3. This indicates that the cation can hydrolyze and potentially make the solution acidic.

3. The hydrolysis of the anion OCN- can be analyzed using the ionization constant of its conjugate base, HOCN: Ka = 3.5×10−4. The cyanate ion, OCN-, can donate a proton to water, giving rise to hydroxide ions (OH-) and the acid HOCN. This suggests that the anion can hydrolyze and potentially make the solution basic.

Based on the ionization constants, we can conclude that:

4. The anion hydrolyzes to a greater extent than the cation. This is because the ionization constant for HOCN (Ka) is higher than the ionization constant for NH3 (Kb).

Therefore, the correct answer is option 4: NH4OCN is basic because the anion hydrolyzes to a greater extent than the cation.