Chapter 15, Problem 15.59SP

Interpretation Introduction

Interpretation:

$\text{pH}$ of the solution of $\text{100 mL of 0}{\text{.30 M NH}}_{\text{3}}$ should be calculated before and after addition of  $\text{4}{\text{.0 g of NH}}_{\text{4}}{\text{NO}}_{\text{3}}$.

Concept introduction:

Equilibrium expression: The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divides by the concentrate ions of the product of reactants to the power of their coefficient.

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

$\text{K}\text{=}\frac{\text{Product}\text{concentrations}}{\text{Reactant}\text{concentrations}}$

$\text{pH:}$

$\text{pH}$ is a logarithmic expression to express a solution is acidic, basic or neutral.  The $\text{pH}$ scale has values between 1 and 14 and on which 7 is neutral, below 7 values are more acidic in nature and above 7 values are more basic in nature.

$\text{pH}\text{=}{\text{-log}}_{\text{10}}{\text{[H}}^{\text{+}}\text{]}$

Percent dissociations:

The percent ratio of concentration of dissociated ions to initial concentration to gives the percent dissociations.

$\text{\%}\text{=}\frac{\text{Dissociated}\text{concentration}}{\text{Initial}\text{concentration}}\text{×100}$