Find the normality of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) having 50 milli- equivalents in 3 litre.

When delving into the realm of chemistry, understanding the 'equivalent factor' is pivotal to making sense of different chemical solutions. The equivalent factor denotes the number of replaceable hydrogen ions in an acid or hydroxide ions in a base that one mole of the substance can furnish when it reacts. For acids, this factor is simply the amount of H+ ions that can dissociate. In the case of \txn\(\textnormal{H}_2\textnormal{SO}_4\), sulfuric acid, each molecule can give up two hydrogen ions, thus possessing an equivalent factor of 2. To comprehend this better, picture each acid molecule like a fruit with a certain number of seeds (hydrogen ions) that can be planted (dissociate) to potentially grow new entities (react).

Another crux of chemistry is the concept of 'molarity,' referring to the concentration of a solution. Simply put, molarity measures how many moles of a solute are present in one liter of solution. It is depicted by the symbol M and is calculated by taking the ratio of moles of solute to liters of solution. If we consider a sugary drink, the sweetness—the concentration of sugar—relates to how many sugar cubes are dissolved in a given volume of liquid. Molarity is a similar idea, where chemists can understand exactly how 'sweet' (concentrated) their solution is with regard to a particular substance.

The process of 'acid dissociation' is integral to understanding how acids behave in solutions. It involves the separation of hydrogen ions from the acid when it is dissolved in water. The degree to which this separation occurs varies among acids. For sulfuric acid, represented as \txn\(\textnormal{H}_2\textnormal{SO}_4\), complete dissociation in water means releasing two hydrogen ions per molecule, which greatly influences its normality. Think of it as a dance where the acid molecules break their connections and each hydrogen ion takes off to join the watery dance floor as individual dancers.

Lastly, to solve practical problems in chemistry, we need a solid grasp of 'concentration of solution.' This term represents the amount of substance contained in a certain volume of a mixture. In solutions, concentration is not just about how much solute is present, but also how it's distributed throughout the solvent. To picture this, imagine a room filled with balloons. The concentration of balloons is higher where they're tightly packed. Similarly, in solutions, chemists are keen on knowing where the solute particles are densely 'packed'—how concentrated they are—to properly prepare and react substances for experiments and applications.