Chapter 6, Problem 6D.19E

Interpretation Introduction

Interpretation:

The $\text{pH}$ of aqueous methylammonium chloride has to be calculated if $15.5\text{g}$ of ${\text{CH}}_{\text{3}}{\text{NH}}_{\text{3}}\text{Cl}$ is present in $\text{450}\text{m}\text{L}$ of aqueous solution.

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Molarity:

Molarity of a solution is defined as the number of moles of solute dissolved in per liter of a solution.  This can be expressed using the given formula;

    $\text{Molarity}=\frac{\text{number}\text{of}\text{moles}}{\text{volume}\text{of}\text{solution}}$

pH definition:

The concentration of hydrogen ion is measured using $\text{pH}$ scale.  The acidity of aqueous solution is expressed by $\text{pH}$ scale.

The $\text{pH}$ of a solution is defined as the negative base -10 logarithm of the hydrogen or hydronium ion concentration.

  $\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

On rearranging, the concentration of hydrogen ion ${\text{[H}}^{+}\text{]}$ can be calculated using pH as follows,

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