is the low solubility of KHT a result of an unfavorable delta H or an unfavorable delta S value
My opinion is that delta H has more influence than delta S on solubility. I would expect delta S to be about the same for solubility for various salts but delta H to be different.
To determine whether the low solubility of KHT (potassium hydrogen tartrate) is a result of an unfavorable ΔH (enthalpy) or an unfavorable ΔS (entropy) value, we can analyze the solubility equilibrium process.
KHT(s) ↔ K+(aq) + HT-(aq)
ΔH represents the enthalpy change associated with the dissolution process and ΔS represents the entropy change. When the dissolution process is endothermic (positive ΔH) and/or the entropy change is unfavorable (negative ΔS), it indicates that the solubility will be lower.
To obtain the answer, we would ideally need the values of ΔH and ΔS. However, without these specific values, we can make some general assumptions.
Generally, salts tend to have favorable ΔH and ΔS values, leading to their high solubility in water. In the case of KHT, however, it has a relatively low solubility, making it an exception.
The low solubility of KHT can be primarily attributed to the unfavorable ΔS value. When a solid dissolves in water, the molecules separate and disperse into the solvent (water) solution. In the case of KHT, the dissociation results in a decrease in disorder (entropy) due to the formation of ions, which are more organized compared to the solid. This reduction in disorder contributes to an unfavorable entropy change.
In summary, while the enthalpy change (ΔH) may also play a role, the low solubility of KHT is predominantly a result of the unfavorable entropy change (ΔS), which causes a decrease in disorder when the solid dissolves, making it less soluble in water.
The low solubility of KHT (potassium hydrogen tartrate) can be attributed to an unfavorable ΔH (enthalpy) value rather than an unfavorable ΔS (entropy) value.
Solubility is influenced by the balance between two factors: the enthalpy change associated with the dissolution process (ΔH) and the entropy change (ΔS) upon dissolution.
In the case of KHT, the low solubility suggests that the enthalpy change associated with the dissolution process is unfavorable, meaning it requires an input of energy to break the bonds between the K+, H+, and tartrate ions in the solid crystal lattice structure. This lack of thermodynamic favorability, or "unfavorable ΔH," makes the process less spontaneous and contributes to the low solubility of KHT.