Enthalpy Changes in Solution

Define dissolution.

Describe the method to determine the enthalpy of neutralization.

Select whether the following statement is True or False:

The standard enthalpy of hydration, $∆{{\mathrm{H}}^{\circ }}_{\mathrm{hyd}}$, for an ion is defined as the enthalpy change when $1$ mol of the gaseous ion is added to a solvent other than water, to form a dilute solution.

Define standard enthalpy of hydration for a substance.

If the hydration energy is equal to or greater than the lattice energy, then an ionic solid is water-soluble.

Explain the conditions for the solubility of an ionic solid in terms of lattice energy and hydration energy.

Solvation energy can be defined as the change in Gibbs energy of a solvent when a solute is dissolved in that solvent. 

Define solvation energy.

Matching Type Question

Which of the followings show apparently low heat of neutralisation:

Which is the correct order of ionic mobility in aqueous medium?

The enthalpy of neutralization of ${\mathrm{NH}}_4\mathrm{OH}$ and ${\mathrm{CH}}_3\mathrm{COOH}$is $-10.5 \mathrm{kcal} {\mathrm{mol}}^{-1}$​ and enthalpy of neutralisation of ${\mathrm{NH}}_4\mathrm{OH}$with a strong acid is $-11.7 \mathrm{kcal} {\mathrm{mol}}^{-1}$. The enthalpy of ionization of ${\mathrm{CH}}_3\mathrm{COOH}$ will be

Given, $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{H}\left(\mathrm{a}\mathrm{q}\right)\to \mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}{\mathrm{O}}^{-}\left(\mathrm{a}\mathrm{q}\right)+{\mathrm{H}}^{+}\left(\mathrm{a}\mathrm{q}\right)$
${\text{ΔH}}_{\text{rxn}}^{\text{o}}\text{=}\text{0}\text{.004}\text{kcal}{\text{gm}}^{-\text{1}}$
Enthalpy change when $1$ mole of $\mathrm{B}\mathrm{a}(\mathrm{O}\mathrm{H}{)}_2$ , a strong base, is completely neutralized by $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{H}\left(\mathrm{a}\mathrm{q}\right)$ is ($\mathrm{\Delta }{\mathrm{H}}^{\circ }$ of neutralization of strong acid with strong base is = $-\text{13}\text{.7}\text{kcal}{\text{mol}}^{-\text{1}}$)

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

Study the figure given below and mark the correct expression.

The enthalpy of solution of $\mathrm{X}{\mathrm{Y}}_{\left(\mathrm{s}\right),}\mathrm{\Delta }{\mathrm{H}}_{\mathrm{s}\mathrm{o}\mathrm{l}\mathrm{n}.}^{°}$ In water can be determined by

What would be the heat released in $\text{kJ}$, when an aqueous solution containing $0.5 \mathrm{mole} \mathrm{of} {\mathrm{HNO}}_3$ is mixed with $0.3 \mathrm{mole} \mathrm{of} {\mathrm{OH}}^{-}$?

(Enthalpy of neutralization is $-57.1\mathrm{ }\mathrm{kJ} {\mathrm{equivalent}}^{-1}$)

Report your answer by rounding it up to the nearest whole number.

The heat evolved during the formation of $24.95 \mathrm{g}$ of hydrated copper sulphate from anhydrous copper sulphate (mol.wt = 159.5) is

$\mathrm{C}\mathrm{u}\mathrm{S}{\mathrm{O}}_4+5{\mathrm{H}}_2\mathrm{O}\to \mathrm{C}\mathrm{u}\mathrm{S}{\mathrm{O}}_4.5{\mathrm{H}}_2\mathrm{O}$

$∆\mathrm{H}=-78.2\mathrm{ }\mathrm{K}\mathrm{J}$

The heat of neutralization of a strong acid by a strong base is $57.3\mathrm{ }\mathrm{K}\mathrm{J}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ . The heat released when 0.5 mol $\mathrm{H}\mathrm{N}{\mathrm{O}}_3$ is mixed with 0.2 mol KOH in aqueous medium is

The enthalpies of neutralization $\mathrm{AOH}$ and a strong base $\mathrm{BOH}$ by $\mathrm{HCl}$ are $-12250 \mathrm{cal}/\mathrm{mol}$ and $-13000 \mathrm{cal}/\mathrm{mol}$ respectively. When one mole of $\mathrm{HCl}$ is added to a solution containing $1$ mole of $\mathrm{AOH}$ and $1$ mole of $\mathrm{BOH}$, the enthalpy change was $-12500 \mathrm{cal}/\mathrm{mol}$. In what ratio is the acid distributed between $\mathrm{AOH}$ and $\mathrm{BOH}$ respectively.