Question

A solution made from pure barium hydroxide contained 2.74g in exactly 100cm3 of water. Using phenolphthalein indicator, titration of 20.0cm3 of this solution required 18.7cm3 of a hydrochloric acid solution for complete neutralisation.(Atomic masses: Ba =137, O=16,H=1). (a) Write the equation for the titration reaction. (b) Calculate the concentration of the barium hydroxide solution. (c) Calculate the moles of barium hydroxide neutralised.(d) Calculate the moles of hydrochloric acid neutralised. (e) Calculate the concentration of the hydrochloric acid. ​Barium Hydroxide Titration

- (a) Write the equation for the titration reaction.
- (b) Calculate the concentration of the barium hydroxide solution.
- (c) Calculate the moles of barium hydroxide neutralized.
- (d) Calculate the moles of hydrochloric acid neutralized.

Answer 1

The equation for the titration reaction is HCl(aq) + Ba(OH)₂(aq) → BaCl₂(aq) + 2H₂O (l). To calculate the concentration of the barium hydroxide solution, use the equation concentration = moles/volume.

Step-by-step explanation:

(a) The equation for the titration reaction is:

2HCl(aq) + Ba(OH)₂(aq) → BaCl₂(aq) + 2H₂O (l)

(b) To calculate the concentration of the barium hydroxide solution, we can use the equation:
number of moles of Ba(OH)₂ = mass of Ba(OH)₂ / molar mass of Ba(OH)₂
Concentration of Ba(OH)₂ solution = moles of Ba(OH)₂ / volume of Ba(OH)₂ solution

(c) To calculate the moles of barium hydroxide neutralized, we can use the equation:
moles of Ba(OH)₂ = volume of Ba(OH)₂ solution used in titration x concentration of Ba(OH)₂ solution

(d) To calculate the moles of hydrochloric acid neutralized, we can use the equation:
moles of HCl = volume of HCl solution used in titration x concentration of HCl solution