**Acid-Base Titration Standardization Exercise**Constant-boiling HCl can be used as a primary standard for acid–base titrations. A 50.00 mL sample of constant-boiling HCl with a concentration of 0.1296 M was collected and titrated to an endpoint with 38.47 mL of a Ba(OH)₂ solution. What is the molarity of the Ba(OH)₂ solution?**Concentration:** [Text Box] M---For calculations, remember that in a titration, the moles of HCl will equal the moles of Ba(OH)₂ reacting according to their balanced equation. Use the formula:\[ \text{M}_1 \times \text{V}_1 = \text{M}_2 \times \text{V}_2 \]Where:- \(\text{M}_1\) and \(\text{V}_1\) are the molarity and volume of HCl.- \(\text{M}_2\) and \(\text{V}_2\) are the molarity and volume of Ba(OH)₂.Please perform the necessary calculations to find the molarity of the Ba(OH)₂ solution.

Beryllium hydroxide reacts with hydrochloric acid to form barium chloride and water. The equation for the balanced chemical reaction is given below: The stoichiometry of the balanced chemical reaction states that one mole of barium hydroxide reacts with two moles of hydrochloric acid to form one mole of barium chloride and two moles of water.Acid-base titration: Titration is a method to determine the concentration of unknown acid by using the known concentrate base or vice-versa. At the endpoint of the titration, two moles of acid are equal to one mole of the base. The mole of acid or base can be calculated by multiplying of molarity of acid or base by the volume. So, we can say that at the endpoint: Where the volume of acid = 50.00 mL The molarity of the acid is = 0.1296 M The volume of base = 38.47By rearranging the above equation we get: Let's put the above values into this formula to get the molarity of the barium hydroxide:The molarity of Ba(OH)2 solution is = 0.08422 M