Which of the following is not a correct statement about enthalpy of solution?

Question

Which of the following is not a correct statement about enthalpy of solution? (A) For most ionic compounds, Δ H°soln. is positive and the dissociation process is endothermic (B) Solubility of most salts increases with increase in temperature (C) If the lattice enthalpy is very high, the dissolution of compound becomes very easy (D) Enthalpy of solution is determined by the selective values of the lattice enthalpy and hydration enthalpy

Tardigrade Admin · Accepted Answer

Dissolution of compound may not take place if lattice enthalpy is very high.

Q. Which of the following is not a correct statement about enthalpy of solution?

For most ionic compounds, $Δ H_{so l n .}^{\circ}$ is positive and the dissociation process is endothermic

Solubility of most salts increases with increase in temperature

If the lattice enthalpy is very high, the dissolution of compound becomes very easy

Enthalpy of solution is determined by the selective values of the lattice enthalpy and hydration enthalpy

Dissolution of compound may not take place if lattice enthalpy is very high.

Q. Which of the following is not a correct statement about enthalpy of solution?

For most ionic compounds, ΔHsoln.∘​ is positive and the dissociation process is endothermic

Solubility of most salts increases with increase in temperature

If the lattice enthalpy is very high, the dissolution of compound becomes very easy

Enthalpy of solution is determined by the selective values of the lattice enthalpy and hydration enthalpy

Dissolution of compound may not take place if lattice enthalpy is very high.

For most ionic compounds, $Δ H_{so l n .}^{\circ}$ is positive and the dissociation process is endothermic