State the relationship between normality and molality
I recommend look at the definitions of each: keyword: google search.
The relationship between normality and molality in a solution depends on the type of solute and its behavior in the solution.
Normality (N) is a concentration unit that represents the number of equivalents of a solute per liter of solution. It is usually used for acids and bases, as it relates to the number of hydrogen or hydroxide ions that are involved in the reaction.
Molality (m) is a concentration unit that represents the number of moles of solute per kilogram of solvent. It is used for non-electrolytic solutes, such as a solute that does not dissociate into ions in solution.
The relationship between normality and molality can be determined by considering the dissociation behavior of the solute. If the solute completely dissociates into ions in solution, then the normality can be calculated from the molality using a conversion factor.
For example, let's consider the case of hydrochloric acid (HCl) dissolved in water. When HCl is dissolved in water, it completely dissociates into hydrogen ions (H+) and chloride ions (Cl-). In this case, the normality can be calculated by multiplying the molality by the number of equivalents per mole of solute. Since HCl dissociates into one hydrogen ion and one chloride ion, this conversion factor is 1.
So, the relationship between normality (N) and molality (m) in this case would be:
N = m × 1
Therefore, for hydrochloric acid, the normality will be equal to the molality.
However, it is important to note that the relationship between normality and molality can vary depending on the solute and its behavior in the solution. Some solutes may not completely dissociate, and in such cases, the relationship between normality and molality would be different. It is always important to consider the dissociation behavior and stoichiometry of the solute in order to establish the relationship between these two concentration units.