Chapter 6, Problem 6.47P

Interpretation Introduction

Interpretation:

$\Delta H$ of ${\text{H}}_2\text{O}$ formed when $25.0\text{ mL}$ of $0.500M{\text{ H}}_{\text{2}}{\text{SO}}_4$ is added to $25.0\text{ mL}$ of $1.00M\text{ KOH}$ in a coffee-cup calorimeter at $23.50°\text{C}$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociates completely in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

Weak acids and weak bases are the substance that do not dissociates completely into its ions when dissolved in the solution. They dissociate partially in water to release ${\text{H}}^{+}$ ions and ${\text{OH}}^{-}$ ions.

The driving force of the acid-base reaction is the formation of gaseous product or precipitate in the reaction.

Specific heat capacity $\left(c\right)$ of a substance is the amount of the heat needed to raise the temperature of $1\text{g}$ of a substance by $1\text{K}$. The formula to calculate heat required is as follows:

$q=\left(\text{mass}\right)\left(c\right)\left(\Delta T\right)$        (1)

Here,

$\Delta T$ is the temperature difference.

$q$ is the heat released or absorbed.

$c$ is the specific heat capacity of the substance.

At the constant pressure the value of $q_{\text{p}}$ is equal to $\Delta H$.