Here are the essential concepts you must grasp in order to answer the question correctly.
Normality
Normality is a measure of concentration equivalent to the number of equivalents of solute per liter of solution. It is particularly useful in acid-base reactions, where it accounts for the reactive capacity of an acid or base. For monoprotic acids, normality is equal to molarity, as they donate one proton per molecule. However, for polyprotic acids, normality can be greater than molarity, reflecting the total number of protons that can be donated.
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Molarity
Molarity is defined as the number of moles of solute per liter of solution. It is a fundamental unit of concentration used in chemistry to express the amount of a substance in a given volume. Molarity does not account for the reactivity of the solute, making it less informative than normality in acid-base chemistry, especially for polyprotic acids, which can release multiple protons.
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Monoprotic vs. Polyprotic Acids
Monoprotic acids are acids that can donate only one proton (H+) per molecule, such as hydrochloric acid (HCl). In contrast, polyprotic acids can donate more than one proton; for example, sulfuric acid (H2SO4) can donate two protons. This distinction is crucial when calculating normality, as polyprotic acids require consideration of all possible protons released, leading to a higher normality compared to their molarity.
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Enantiomers vs Diastereomers Concept 1