Chapter 10, Problem 10.98CP

(a)

Interpretation Introduction

Interpretation:

The moles of $\text{HCl}$ dissolved in solution prepared by bubbling 15L of $\text{HCl}$ in ${\text{25}}^{\text{o}}\text{C}\text{at}\text{1atm}$ into water of $\text{250mL}$ should be determined.

Concept Introduction:

Ideal gas Equation:

Any gas can be described by using four terms namely pressure, volume, temperature and the amount of gas. It is referred as ideal gas equation.

$\begin{array}{l}\text{V }\propto \frac{\text{nT}}{\text{P}}\\ \text{V = R}\frac{\text{nT}}{\text{P}}\\ \text{PV = nRT}\\ \text{where,}\\ \text{n = moles of gas}\\ \text{P = pressure}\\ \text{T = temperature}\\ \text{R = gas }\text{constant}\end{array}$

Under some conditions gases don not behave like ideal gas that is they deviate from their ideal gas properties. At lower temperature and at high pressures the gas tends to deviate and behave like real gases.

Moles: One mole is equivalent to the mass of the substance consists of same number of units equal to the atoms present in $\text{12}\text{g}$ of ${}^{\text{12}}\text{C}$.

(b)

Interpretation Introduction

Interpretation:

The $\text{pH}$ of $\text{HCl}$ dissolved in solution prepared by bubbling 15L of $\text{HCl}$ in ${\text{25}}^{\text{o}}\text{C}\text{at}\text{1atm}$ into water of $\text{250mL}$ should be determined.

Concept Introduction:

$\text{pH}$: The concentration of hydrogen ion is measured using $\text{pH}$ scale. The $\text{pH}$ of a solution is a figure that expresses the acidity or the alkalinity of a given solution.

It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

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

If the value of $\text{pH}$ is less than $7$, then the solution is acidic whereas if the value of $\text{pH}$ is greater than $7$, then the solution is basic.

Molarity: The concentration for solutions is expressed in terms of molarity as follows,

$\text{Molarity = }\frac{\text{No}\text{. of moles of solute}}{\text{Volume of solution in L}}$

Strong Acids: Acids that dissociates into ions completely which results in easy donation of protons are considered as strong acids. Strong acid forms weaker conjugated base.