Chemical Reaction Stoichiometry: Discover the Magic of Balancing Equations
Have you ever wondered how to calculate the volume of solutions needed to complete a chemical reaction?
Let's explore a scenario where we need to determine the volume of a Ba(OH)2 solution required to react completely with a given volume of HBr solution.
Understanding Chemical Reaction Stoichiometry
Chemical reaction stoichiometry involves the quantitative aspects of chemical reactions, specifically the calculations involving reactants and products in a chemical equation.
In the scenario provided, we are tasked with determining the volume of a 0.149 M Ba(OH)2 solution needed to completely react with 68.1 ml of a 0.116 M HBr solution.
Exploring the Solution
Before diving into the calculations, it is essential to understand the balanced chemical equation for the reaction: Ba(OH)2 + 2 HBr --> BaBr2 + 2 H2O. This equation reveals the stoichiometry of the reaction, where one mole of Ba(OH)2 reacts with two moles of HBr.
To begin solving the problem, we first calculate the moles of HBr present in the given volume: Moles of HBr = Molarity x Volume(L) = 0.116 M x 0.0681 L = 0.007906 moles.
Following the stoichiometry of the reaction, we determine that the moles of Ba(OH)2 required will be half the moles of HBr = 0.007906 / 2 = 0.003953 moles.
Next, to find the volume of the Ba(OH)2 solution needed, we divide the moles of Ba(OH)2 by its molarity: Volume (L) = Moles / Molarity = 0.003953 / 0.149 M = 0.02653 L or 26.53 mL.
By understanding the principles of chemical reaction stoichiometry, we can accurately determine the volume of solutions needed to complete a reaction and achieve desired outcomes in chemistry.