High School

Thank you for visiting A 25 0 mL solution of tex Ba OH 2 tex is neutralized with 36 6 mL of 0 250 M tex HBr tex What. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!

A 25.0 mL solution of [tex]Ba(OH)_2[/tex] is neutralized with 36.6 mL of 0.250 M [tex]HBr[/tex]. What is the concentration of the original [tex]Ba(OH)_2[/tex] solution?

Answer :

Final answer:

The concentration of the original Ba(OH)2 solution can be calculated using the given information and the formula for concentration. The concentration is approximately 0.292 M.

Explanation:

To calculate the concentration of the original Ba(OH)2 solution, we can follow these steps:

  • Write the balanced chemical equation for the reaction between Ba(OH)2 and HBr:

Ba(OH)2 + 2HBr → BaBr2 + 2H2O

  • Use the balanced equation to determine the mole ratio between Ba(OH)2 and HBr. In this case, the ratio is 1:2.
  • Calculate the moles of HBr using its concentration and volume:

Moles of HBr = (concentration of HBr) × (volume of HBr solution in liters)

  • Use the mole ratio to calculate the moles of Ba(OH)2:

Moles of Ba(OH)2 = (moles of HBr) / 2

  • Finally, calculate the concentration of the Ba(OH)2 solution:

Concentration of Ba(OH)2 = (moles of Ba(OH)2) / (volume of Ba(OH)2 solution in liters)

Learn more about concentration of a solution here:

https://brainly.com/question/32034739

#SPJ14

Thank you for reading the article A 25 0 mL solution of tex Ba OH 2 tex is neutralized with 36 6 mL of 0 250 M tex HBr tex What. We hope the information provided is useful and helps you understand this topic better. Feel free to explore more helpful content on our website!

Rewritten by : Jeany

Other Questions