Chapter 4.1, Problem 4.1AFP

(a)

Interpretation Introduction

Interpretation:

The strong electrolyte among $\text{LiBr}$, ${\text{Cs}}_2{\text{CO}}_3$ and ${\text{BaCl}}_2$ that is dissolved in the given beaker is to be determined.

Concept introduction:

A solution is a combination of two parts: solute and solvent. A solute is the substance that is present in small quantity and solvent is the substance in which solute is dissolved. When water acts as a solvent then it is known as an aqueous solution.

An electrolyte is a substance that conducts electricity when it is dissolved in water. Ionic compounds like $\text{LiBr}$, ${\text{Cs}}_2{\text{CO}}_3$ and ${\text{BaCl}}_2$ are the examples of the electrolyte.

(b)

Interpretation Introduction

Interpretation:

Mass of ${\text{BaCl}}_2$ when each particle represents $0.05\text{mol}$ is to be determined.

Concept introduction:

An electrolyte is a substance that conducts electricity when it is dissolved in water. Ionic compounds like $\text{LiBr}$, ${\text{Cs}}_2{\text{CO}}_3$ and ${\text{BaCl}}_2$ are the examples of the electrolyte. Mass of compound from mole of each particle is obtained by multiplying the number of particles with a given mole of each particle and molecular weight of the compound.

The expression to calculate the mass of a compound in grams is as follows:

$\begin{array}{c}\text{Mass }\left(\text{g}\right)=\left(\text{number of particles}\right)\left(\frac{\text{mole of one particle}\left(\text{mol}\right)}{1\text{ particle}}\right)\\ \left(\frac{1\text{}\text{mol compound}}{1\text{mol}\text{of}\text{ions}}\right)\left(\frac{\mathrm{molecular}massofcompound\left(\text{g}\right)}{1\text{mol compound}}\right)\end{array}$

The molecular mass of the compound is the sum of the atomic weight of the atoms that are present in the molecular formula of that compound. It is measured in grams. The molar mass of a compound is calculated by adding the molar mass of each element multiplied by its number of atoms present in the chemical formula.