Chapter 10, Problem 10.90AP

Interpretation Introduction

Interpretation:

The molarity and normality of solution prepared by dissolving 5 g of $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ to $500mL$ solution should be determined.

Concept Introduction:

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 ${}^{\text{12}}\text{C}$.

$\text{No}\text{. of moles = }\frac{\text{Given mass}}{\text{Molar mass}}$

Normality: It generally expresses the concentration of acid or base as equivalents of acid or base present in one liter of the solution.

$\text{Normality}\left(\text{N}\right)\text{=}\frac{\text{Equivalents of acid/base}}{\text{Liters of solution}}$

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

The normality for any acid or base equals the molarity times of the number of ${\text{H}}^{\text{+}}\text{and}{\text{OH}}^{\text{-}}$ correspondingly.

Equivalent of Acid: Generally, 1 equivalent of ion is the number of ions which has charge of one mole.

Equivalent of Base: In case of bases negative charge is of interest therefore, one equivalent of base consists of 1 mole of $O{H}^{-}$ ions.

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

$\text{Bronsted-Lowry Base}$: If a species receives one proton, then it is considered as $\text{Bronsted-Lowry base}\text{.}$