Chemistry Challenge: Titration with Hydrobromic Acid and Barium Hydroxide

How can we calculate the molarity of a hydrobromic acid solution using titration data?

In an aqueous solution of hydrobromic acid standardized by titration with a 0.149 M solution of barium hydroxide, if 13.5 mL of base neutralizes 24.0 mL of the acid, what is the molarity of the hydrobromic acid solution?


The molarity of the hydrobromic acid solution is approximately 0.447 M by chemical equation.

By using the balanced chemical equation and mole ratio, we can calculate the molarity of the hydrobromic acid solution based on the titration data. In this titration, the balanced chemical equation is: HBr(aq) + Ba(OH)₂(aq) → BaBr₂(aq) + 2H₂O(l).

From the equation, we know that 1 mole of HBr reacts with 2 moles of Ba(OH)₂. Given that 13.5 mL of 0.149 M Ba(OH)₂ solution neutralizes 24.0 mL of HBr solution, we can set up a proportion based on the mole ratio: (0.149 M) / 2 = (x M) / 1. Solving for x, the molarity of HBr, we get: x = 0.447 M.

Understanding the chemical equation and the mole ratio is crucial in determining the molarity of the hydrobromic acid solution through titration. This method allows for precise measurements and calculations in chemical analyses.

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