Why is it easy to work with normality than molarity? Can someone explain this question to me, preferably with an example?
For monoprotic acids, when concentration is expressed as a normality, this is equivalent to the stated molarity. Normality is used with diprotic acids such as sulfuric acid. Because sulfuric acid has 2 equiv protons to donate (i.e. bisulfate anion is a reasonably strong acid) a solution of 0.5 mol per litre sulfuric acid would be referred to as "1 Normal", precisely because it would require 2 equiv for neutralization. Likewise, 1 mol per litre sulfuric acid would be referred to as "2 normal".